2H2 + 1O2 --> 2H2O


Suppose you had 20. 76 moles of H2 on hand and plenty of O2, how many moles of H2O could you make?

The commonly used rules of thumb used by chemists to make buffers are:

Buffers are solutions that resist changes in pH when small amounts of acid or base are added to them. They are commonly used in many chemical and biological applications. The rules of thumb mentioned above provide guidelines for making effective buffers. Rule a) ensures that there is an adequate amount of buffering capacity in the solution. Rule b) is based on the fact that weak acids have a pH-dependent dissociation constant, and therefore, the pH of a buffer made from a weak acid will be close to the pKa of the weak acid.

Similarly, the pH of a buffer made from a weak base will be close to the pKa of the conjugate acid. Rule c) ensures that the buffering capacity of the solution is optimized by selecting the appropriate pKa value. Overall, these rules of thumb help chemists to design effective buffers that can maintain a stable pH over a range of conditions.

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If the algae disappeared, the tiny animals would not have enough food.

Small fish that eat the tiny animals would also run out of food, which might lead to a drop in their number. As a result, less oxygen would be accessible for other organisms and the amount of oxygen the fish produce would decrease.

However, since the plants may still obtain their carbon dioxide from other sources, the loss of the algae would not have a direct impact on them.

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Answer: 652.8 g of iron (III) oxide produced.

Explanation:

To calculate the amount of iron (III) oxide produced, we use the enthalpy change of the reaction to determine the amount of energy released and convert it to moles of Fe2O3 produced. Then, we multiply by the molar mass of Fe2O3 to obtain the mass of Fe2O3 produced. Using these calculations, we get 652.8 g of iron (III) oxide produced.

580.84 grams of iron (III) oxide will be produced when 4300 kJ of heat energy is released.

Given:

Enthalpy change (∆H) value: ∆H = -1652 kJ

Amount of heat energy released: 4300 kJ

From the balanced equation:

4Fe + 3O₂ → 2 Fe₂O₃

The molar ratio between Fe₂O₃ and ∆H is 2:1652 kJ.

To find the molar amount of Fe₂O₃ produced, the following calculation:

[tex]4300 \times \frac{2}{1652}[/tex] = 5.20 mol Fe₂O₃

To convert this into grams, it is required to multiply the molar amount by the molar mass of Fe₂O₃:

5.20  × 2  × 55.85 = 580.84 g

Therefore, 580.84 grams of iron (III) oxide will be produced when 4300 kJ of heat energy is released.

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The new concentration of the solution can be calculated using the dilution formula, which states that the initial concentration multiplied by the initial volume (V1) is equal to the new concentration multiplied by the new volume (V2).

In this case, the equation would be: (3.5M)(0.20L) = (xM)(0.90L). Solving for x, we get the new concentration of the solution as 3.17M.

In other words, when a 3.5M solution of lici is diluted from 0.20L to 0.90L, the new concentration of the solution is 3.17M. This is because when the volume of a solution is increased, the concentration of the solution decreases proportionately.

Thus, when the volume of the solution is increased by a factor of four and a half, the concentration of the solution is reduced by the same factor.

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The chemical energy referred to in the transfer from producers to consumers is the energy stored in the organic molecules synthesized by the producers during photosynthesis.

Producers, such as plants and algae, use energy from sunlight to convert carbon dioxide and water into glucose and other organic molecules through the process of photosynthesis. The energy from the sunlight is converted into chemical energy and stored in the organic molecules.

Consumers, such as herbivores and carnivores, obtain this stored chemical energy by consuming the organic molecules synthesized by the producers. The organic molecules are broken down during cellular respiration to release the stored chemical energy, which is used by the consumer to power its cellular processes.

Thus, the transfer of chemical energy from producers to consumers is a fundamental process in the food chain, and it is essential for the maintenance of life on earth.

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The third quantum number of a 2p³ electron in phosphorus is M = -1. Option A is the answer.

The electronic configuration of phosphorus is 1s²2s²2p⁶3s²3p³. The 2p subshell has three orbitals, which can hold up to six electrons. The three orbitals are labeled as 2p_x, 2p_y, and 2p_z, where each orbital can hold a maximum of two electrons with opposite spins.

The three quantum numbers that define the state of an electron in an atom are n, l, and m. Here, n represents the principal quantum number, l represents the azimuthal quantum number, and m represents the magnetic quantum number.

The values of l for the 2p subshell are 1, and the possible values of m for l = 1 are -1, 0, and 1. The electron in question is in the 2p subshell, so its value of l is 1. Since the possible values of m for this electron are -1, 0, and 1, we can rule out options B, C, and D. Therefore, the correct answer is A, M = -1. Hence, option A is the answer.

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At STP, typically defined as a temperature of 0°C (273.15K) and a pressure of 1 atm, the volume of a gas is equal to 30 L.

When the temperature of the gas is increased, the kinetic energy of the gas particles increases, causing them to move more quickly and expand. This expansion of the gas increases its volume.

Using the ideal gas law, the new volume of the gas can be calculated by multiplying the original volume by the ratio of the new temperature (323.15K) to the original temperature (273.15K) and raising that to the power of 1/273.15.

In this case, the new volume of the gas is 33.53 L. In conclusion, when the temperature of a gas is raised, its volume increases.

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A helium filled balloon has a volume of 50. 0L at 25⁰C and 1. 00 atm.  43.6 L will it have at 0. 855 atm and 10. 0⁰C.

To solve this problem, we can use the combined gas law, which relates the pressure, volume, and temperature of a gas. The formula is:

[tex]\frac{{P_1V_1}}{{T_1}} = \frac{{P_2V_2}}{{T_2}}[/tex]

Where P1, V1, and T1 are the initial conditions, and P2, V2, and T2 are the final conditions. Plugging in the given values, we get:

[tex]\left(\frac{{1.00 , \text{atm} \cdot 50.0 , \text{L}}}{{298 , \text{K}}}\right) = \left(\frac{{0.855 , \text{atm} \cdot V2}}{{283 , \text{K}}}\right)[/tex]

Solving for V2, we get:

[tex]V2 = \frac{{1.00 , \text{atm} \cdot 50.0 , \text{L}}}{{298 , \text{K}}} \times \frac{{283 , \text{K}}}{{0.855 , \text{atm}}} = 43.6 , \text{L}[/tex]

Therefore, the helium-filled balloon will have a volume of 43.6 L at 0.855 atm and 10.0⁰C.

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40.32 grams of hydrogen gas will be produced.

According to the balanced chemical equation:

1 mol of Zn reacts with 2 mol of HCl to produce 1 mol of H2

So if 20.0 mol of Zn is added to excess HCl, all the Zn will react to produce:

20.0 mol Zn × 1 mol H2 / 1 mol Zn = 20.0 mol H2

To calculate the mass of H2 produced, we need to use its molar mass, which is 2.016 g/mol:

Mass of H2 = number of moles of H2 × molar mass of H2

Mass of H2 = 20.0 mol × 2.016 g/mol

Mass of H2 = 40.32 g

Therefore, 40.32 grams of hydrogen gas will be produced.

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The chemical formula for cassiterite is SnO2, which means that there are two moles of oxygen for every one mole of tin in the compound.

Given that there are 3.316 moles of tin in the sample, we can use the mole ratio to determine the number of moles of oxygen:

1 mole Sn : 2 moles O

3.316 moles Sn : x moles O

x = (3.316 moles Sn) x (2 moles O / 1 mole Sn) = 6.632 moles O

Therefore, there are 6.632 moles of oxygen in the sample of cassiterite.

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The mole ratio of [tex]NaNO_3[/tex] to [tex]Na_2O[/tex] is 2:1 in the balanced equation

The reasonable compound condition[tex]2NaNO_3 + PbO → Pb(NO_3)_2 + Na_2O[/tex] shows that two moles of sodium nitrate[tex](NaNO_3)[/tex] respond with one mole of lead oxide [tex](PbO)[/tex]to create one mole of sodium oxide [tex]Na_2O[/tex] and one mole of lead nitrate[tex](Pb(NO_3)_2)[/tex] .

In this way, the mole proportion of [tex]NaNO_3[/tex] to [tex]Na_2O[/tex]is 2:1. This intends that for each two moles of [tex]NaNO_3[/tex] utilized, one mole of[tex]Na_2O[/tex] is delivered.

This mole proportion is significant in deciding how much  [tex]Na_2O[/tex]delivered when a known measure of [tex]NaNO_3[/tex] is utilized. For instance, assuming we have 2 moles of [tex]NaNO_3[/tex], we can establish that we will deliver 1 mole of [tex]Na_2O[/tex]. Assuming that we have 4 moles of[tex]NaNO_3[/tex] , we will create 2 moles of [tex]Na_2O[/tex].

Knowing the mole proportion likewise permits us to compute the hypothetical yield of [tex]Na_2O[/tex] in light of how much [tex]NaNO_3[/tex]  utilized. In any case, practically speaking, the genuine yield might contrast because of exploratory mistake or different elements.

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Answer:

Explanation:

it's 2:1 the top person is right and how i know that is because when i was in school i have my notes so the top of me is right!!! :)

Answer:

The chemical equation for the conversion of glucose to ethanol during fermentation is:

C6H12O6 → 2C2H5OH + 2CO2

From the equation, we can see that for every mole of glucose (C6H12O6) that reacts, two moles of ethanol (C2H5OH) are produced. The molar mass of glucose is 180.16 g/mol, while the molar mass of ethanol is 46.07 g/mol.

Therefore, to calculate the mass of ethanol produced from 500.0 grams of glucose, we need to convert the mass of glucose to moles, then use the mole ratio from the balanced chemical equation to calculate the moles of ethanol produced, and finally convert the moles of ethanol to mass.

Step 1: Convert the mass of glucose to moles

Number of moles of glucose = mass of glucose ÷ molar mass of glucose

Number of moles of glucose = 500.0 g ÷ 180.16 g/mol

Number of moles of glucose = 2.776 mol

Step 2: Use the mole ratio to calculate the moles of ethanol produced

From the balanced equation, 1 mol of glucose produces 2 mol of ethanol

Therefore, 2.776 mol of glucose will produce:

2.776 mol glucose × (2 mol ethanol / 1 mol glucose) = 5.552 mol ethanol

Step 3: Convert moles of ethanol to mass

Mass of ethanol = number of moles of ethanol × molar mass of ethanol

Mass of ethanol = 5.552 mol × 46.07 g/mol

Mass of ethanol = 255.2 g

Therefore, 500.0 grams of glucose will produce 255.2 grams of ethanol during fermentation.

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We can use the formula for calculating heat:

Q = m × c × ΔT

where Q is the amount of heat transferred, m is the mass of the substance, c is its specific heat, and ΔT is the change in temperature.

Plugging in the given values, we get:

8250 J = m × 0.9025 J/g ·°C × 40.0 °C

Simplifying, we get:

8250 J = m × 36.1 J/g

Solving for m, we get:

m = 8250 J ÷ 36.1 J/g

m ≈ 228.26 g

Therefore, the mass of the aluminum is approximately 228.26 g.

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The dissociation reaction for the salt AB3 is:

AB3(s) ↔ A3+(aq) + 3B-(aq)

Let's assume the solubility of AB3 in water at 25 °C is x mol/L. Then, the equilibrium concentrations of A3+ and B- can be expressed as x and 3x, respectively.

The Ksp expression for AB3 is:

Ksp = [A3+][B-]^3 = x(3x)^3 = 27x^4

The molar mass of AB3 is 305 g/mol, so the number of moles in 4.30 g (the solubility) is:

n = 4.30 g / 305 g/mol = 0.0141 mol/L

Therefore, the solubility of AB3 at 25 °C is:

x = 0.0141 mol/L

Substituting this into the Ksp expression:

Ksp = 27x^4 = 27(0.0141)^4 = 5.6 x 10^-9

Therefore, the Ksp of AB3 at 25 °C is 5.6 x 10^-9.

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To solve this problem, we need to use the ideal gas law which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature. Rearranging this equation, we can solve for n by dividing both sides by RT.

n = PV/RT
Now, we can plug in the given values:
n = (4.2 atm)(128 L)/(0.0821 L*atm/mol*K)(382 K)

n = 16.4 moles
Therefore, 16.4 moles of gas occupy 128L at a pressure of 4.2 atm and a temperature of 382K.

It's important to note that the ideal gas law is only applicable to ideal gases, which follow certain assumptions such as having no intermolecular forces and having particles with negligible volume. Real gases can deviate from these assumptions, especially at high pressures and low temperatures. However, for most practical purposes, the ideal gas law provides a good approximation of gas behavior.

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The volume-to-temperature ratio calculated by the students would be affected differently by each procedural change.

A) Failing to replenish boiling water would result in the flask being heated at a lower temperature than intended, leading to a smaller volume-to-temperature ratio.

B) Partially immersing the flask in the ice-water bath would lead to slower cooling and a higher temperature at the end of the cooling period, resulting in a larger volume-to-temperature ratio.

C) Neglecting to close the pinch clamp would allow air to enter the flask during cooling, leading to a lower pressure and a larger volume-to-temperature ratio.

D) Using 125 mL as the volume of the flask would result in an inaccurate volume-to-temperature ratio, as the actual volume of the flask may be different. It is important to measure the volume of the flask accurately to obtain reliable results.

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The metal has a specific heat of 0.385 J/g°C.

To solve for the specific heat of the metal, we need to use the equation:
Q = mCΔT
where Q is the heat transferred, m is the mass of the substance, C is the specific heat, and ΔT is the change in temperature.

In this case, the heat transferred from the metal to the water can be calculated as:
Q = mcΔT
where c is the specific heat of water (4.184 J/g°C) and ΔT is the change in temperature of the water (from 24.0°C to 32.5°C).

Q = (50.0 g)(4.184 J/g°C)(32.5°C - 24.0°C)
Q = 1743.8 J

The heat transferred from the metal to the water is equal to the heat absorbed by the metal:
Q = mCΔT

where m is the mass of the metal and ΔT is the change in temperature of the metal (from 100.0°C to 32.5°C).
1743.8 J = (23.8 g)C(100.0°C - 32.5°C)
C = 0.385 J/g°C

Therefore, the specific heat of the metal is 0.385 J/g°C.

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The pH of a 0.10 M solution of hypochlorous acid with a Ka value of 2.9 x 10-8 is approximately 4.77.

Hypochlorous acid, also known as HOCl, is a weak acid that can dissociate in water to form hydrogen ions (H+) and hypochlorite ions (OCl-). The dissociation constant of HOCl, also known as Ka, is a measure of the strength of the acid. In this case, the Ka value of HOCl is 2.9 x 10-8.

To calculate the pH of a 0.10 M solution of HOCl, we need to use the Ka value and the expression for the equilibrium constant:

Ka = [H+][OCl-]/[HOCl]

We can assume that the concentration of HOCl at equilibrium is equal to the initial concentration, since it is a weak acid and only partially dissociates. We also know that the concentration of H+ is equal to the concentration of the acid that dissociated, so we can substitute these values into the expression:

Ka = [H+]^2/[HOCl]
[H+]^2 = Ka x [HOCl]
[H+]^2 = 2.9 x 10-8 x 0.10
[H+] = 1.7 x 10-5 M

Now that we have calculated the concentration of H+, we can use the pH equation to find the pH:

pH = -log[H+]
pH = -log(1.7 x 10-5)
pH = 4.77

Therefore, the pH of a 0.10 M solution of hypochlorous acid with a Ka value of 2.9 x 10-8 is approximately 4.77.

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The heating process is often used in experiments to evaporate liquid and concentrate the sample. If the heating was stopped before all of the liquid could evaporate, this would have a significant impact on the results of the experiment.

Firstly, the concentration of the sample would be lower than expected. This could affect the accuracy and precision of any measurements or analyses performed on the sample.

For example, if the sample was being analyzed for the presence of a certain compound, the lower concentration may make it more difficult to detect or quantify the compound accurately.

Additionally, the incomplete evaporation of the liquid could lead to contamination of the sample. If the liquid is not fully evaporated, there may be impurities or other compounds present in the final sample that were not accounted for in the experimental design. This could affect the validity of the results and the interpretation of the data.

In summary, the premature stopping of heating in an experiment could lead to lower sample concentration and potential contamination, both of which could have significant implications for the results and conclusions drawn from the experiment.

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To accurately measure a very small volume of liquid like 0.03 ml, a micropipette would be the most appropriate measuring tool to use.

A micropipette is a laboratory instrument commonly used in biology, chemistry, and other related fields to accurately and precisely measure and transfer small volumes of liquids. It typically operates through a piston-driven air displacement system, allowing for very precise measurements in the microliter (μL) or even nanoliter (nL) range.

Micropipettes are commonly used in applications such as DNA sequencing, PCR, and protein assays, where precise and accurate liquid handling is essential for accurate results.

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The pH of the buffer solution will decrease by 0.28 units when 0.081 mol of HI is added

To solve this problem, we need to use the Henderson-Hasselbalch equation:

pH = pKa + log([A-]/[HA])

where pKa is the dissociation constant of the acid (NH4+) and A- is the conjugate base (NH3).

First, we need to find the pKa of NH4+ by using the equation:

pKa = -log(Ka)

where Ka is the acid dissociation constant. The Ka for NH4+ is 5.6 x 10^-10, so:

pKa = -log(5.6 x 10^-10) = 9.25

Next, we need to calculate the concentrations of NH4+ and NH3 in the buffer solution after the addition of HI. We can use the equation:

Cfinal = Cinitial + moles added / volume

The volume of the buffer is 1.00 L, and we are adding 0.081 mol of HI, which will react with NH3 according to the equation:

HI + NH3 -> NH4+ + I-

Since the reaction is 1:1, we will end up with 0.081 mol of NH4+ and 0.081 mol of I-. Therefore:

[C(NH4+)]final = [C(NH4+)]initial + 0.081 mol / 1.00 L = 0.380 M
[C(NH3)]final = [C(NH3)]initial - 0.081 mol / 1.00 L = 0.246 M

Now we can calculate the pH of the buffer before and after the addition of HI. Using the Henderson-Hasselbalch equation:

pHbefore = 9.25 + log([NH3] / [NH4+])
         = 9.25 + log(0.327 / 0.299)
         = 9.25 + 0.074
         = 9.32

pHafter = 9.25 + log([NH3]final / [NH4+]final)
        = 9.25 + log(0.246 / 0.380)
        = 9.25 - 0.210
        = 9.04

Finally, we can calculate the pH change:

pHchange = pHafter - pHbefore
        = 9.04 - 9.32
        = -0.28

Therefore, the pH of the buffer solution will decrease by 0.28 units when 0.081 mol of HI is added.

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After four half-lives, 12.5 grams of the parent isotope will be left in a sample that originally contained 140 grams of an unstable isotope.

The amount of the parent isotope remaining after a certain number of half-lives can be calculated using the formula:

Remaining amount = Initial amount x (1/2)^(number of half-lives)

For this problem, the initial amount of the unstable isotope is 140 g, and it goes through 4 half-lives.

One half-life is the time it takes for half of the original sample to decay, and the number of half-lives is equal to the total time elapsed divided by the length of one half-life.

If we know the half-life of the isotope, we can find the total time elapsed. Let's assume the half-life of the isotope is 10 days.

After 10 days, half of the initial sample will remain:

Remaining amount = 140 g x (1/2)¹ = 70 g

After another 10 days (20 days total), half of the remaining sample will decay:

Remaining amount = 70 g x (1/2)¹ = 35 g

After another 10 days (30 days total), half of the remaining sample will decay again:

Remaining amount = 35 g x (1/2)¹ = 17.5 g

After another 10 days (40 days total), half of the remaining sample will decay once more:

Remaining amount = 17.5 g x (1/2)¹ = 8.75 g

Therefore, after 4 half-lives (40 days), there will be approximately 8.75 g of the parent isotope remaining.

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The standard molar entropy change for the combustion of methane gas is 9.9 J/(mol·K).

The balanced equation for the combustion of methane is:

[tex]CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)[/tex]

The standard molar entropy change can be calculated using the formula:

ΔS° = ΣS°(products) - ΣS°(reactants)

The standard molar entropy values for the species involved in the reaction are:

ΔS°(CH4) = 186.3 J/(mol·K)

ΔS°(O2) = 205.0 J/(mol·K)

ΔS°(CO2) = 213.6 J/(mol·K)

ΔS°(H2O(l)) = 69.9 J/(mol·K)

Using these values, we can calculate the standard molar entropy change:

ΔS° = [ΔS°(CO2) + ΔS°(2H2O(l))] - [ΔS°(CH4) + ΔS°(2O2(g))]

ΔS° = [(213.6 J/(mol·K)) + (2 × 69.9 J/(mol·K))] - [(186.3 J/(mol·K)) + (2 × 205.0 J/(mol·K))]

ΔS° = 9.9 J/(mol·K)

Therefore, the standard molar entropy change for the combustion of methane gas is 9.9 J/(mol·K).

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When zinc reacts with hydrochloric acid, the response bubbles vigorously as hydrogen fueloline is produced.

The manufacturing of a fueloline is likewise an illustration that a chemical response is occurring. When dilute hydrochloric acid is introduced to granulated zinc positioned in a take a look at tube, zinc metallic is transformed to zinc chloride and hydrogen fueloline is developed withinside the response. In the response we will see that a zinc chloride salt is fashioned and hydrogen fueloline is developed. The developed hydrogen fueloline is colourless and odourless. When Zinc granules reacts with Hydrochloric acid ,it'll produces hydrogen fueloline and zinc chloride.

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Answer:

Rn has the most stable nucleus

Rn (Radon) has the most stable nuclei due to its closer proximity to the magic number 126.

Option (3) is correct.

The stability of a nucleus depends on the arrangement of protons and neutrons within it. Certain numbers of protons and neutrons result in more stable nuclei. These numbers are known as magic numbers, and they correspond to complete nuclear shells.

Among the given atoms:

Ra (Radium) has 88 protons and a varying number of neutrons.

Po (Polonium) has 84 protons and a varying number of neutrons.

Rn (Radon) has 86 protons and a varying number of neutrons.

Au (Gold) has 79 protons and a varying number of neutrons.

Radon (Rn) has the most stable nuclei because it is closer to the magic number 126 for neutrons. Elements with magic numbers of protons or neutrons tend to have more stable configurations, making Rn the most stable among the options provided.

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Translating the given balanced chemical equation into words : B)Barium nitride reacts with water to yield barium hydroxide and nitrogen hydrogen.

Barium nitride (Ba₃N₂) is an ionic compound composed of three barium cations (Ba²⁺) and two nitride anions (N³⁻). It is a gray or black crystalline solid that is highly reactive and is used in the production of other chemicals, such as barium azide (Ba(N₃)₂) and barium cyanide (Ba(CN)₂).

Barium nitride can also be used as a reducing agent in the synthesis of metals and alloys. When it reacts with water, it produces barium hydroxide (Ba(OH)₂) and ammonia gas (NH₃).

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The excess reactant will be oxygen.

To determine the excess reactant, we need to compare the amount of moles of each reactant to the stoichiometry of the balanced equation. The stoichiometric ratio between magnesium and oxygen is 2:1, which means that for every 2 moles of magnesium, 1 mole of oxygen is required for complete reaction.

In this case, we have 7.8 moles of magnesium and 4.7 moles of oxygen. Based on the stoichiometric ratio, we can see that 7.8 moles of magnesium require 3.9 moles of oxygen (2 moles of oxygen for every 1 mole of magnesium). Since we only have 4.7 moles of oxygen, it is the limiting reactant, and magnesium will be in excess.

Therefore, after the reaction is complete, all of the magnesium will be consumed, and some oxygen will be left over. The product of the reaction will be 7.8 moles of magnesium oxide.

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Bond energy refers to the amount of energy required to break a bond between two atoms. This energy is required because bonds are formed when electrons are shared between atoms, and breaking a bond requires energy to be put into the system to overcome the electrostatic forces holding the atoms together.

In the case of the reaction given, h-h + i-i ---> 2h-i, we are asked to determine the energy change associated with breaking the H-H and I-I bonds and forming two new H-I bonds. To do this, we can use the bond energies of the individual bonds involved.

According to a standard table of bond energies, the H-H bond has a bond energy of 432 kJ/mol, while the I-I bond has a bond energy of 149 kJ/mol. The H-I bond has a bond energy of 436 kJ/mol. Using these values, we can calculate the energy change for the reaction as follows:

(2 x H-I bond energy) - (H-H bond energy + I-I bond energy)
= (2 x 436 kJ/mol) - (432 kJ/mol + 149 kJ/mol)
= 293 kJ/mol

So the energy change for the reaction is 293 kJ/mol. This means that the reaction is exothermic, as energy is released when the bonds are formed. This energy can be used to do work or heat up the surroundings.

Finally, you mentioned the term "marking brainliest". I assume you are referring to the "Brainliest Answer" feature on certain online platforms, where the person who asks a question can choose which answer they found most helpful or accurate. If this is the case, I hope my answer has been helpful and informative!

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Unknown + Potassium Carbonate → Potassium Nitrate + Unknown Carbonate

[tex]Sr(NO_3)_2[/tex] + [tex]K_2CO_3[/tex] → [tex]2KNO_3[/tex] + [tex]SrCO_3[/tex] (if the unknown is strontium nitrate)

[tex]Mg(NO_3)_2[/tex]+ [tex]K_2CO_3[/tex] → [tex]2KNO_3[/tex] + [tex]MgCO_3[/tex] (if the unknown is magnesium nitrate)

Here are the balanced molecular equations for the reactions that could have occurred between the unknown solution (either strontium nitrate or magnesium nitrate) and potassium carbonate and potassium sulfate: Unknown + potassium carbonate → potassium nitrate + magnesium or strontium carbonate (depending on the unknown)

Unknown + potassium sulfate → potassium nitrate + magnesium or strontium sulfate (depending on the unknown)

Unknown + Potassium Sulfate → Potassium Nitrate + Unknown Sulfate

[tex]Sr(NO_3)_2[/tex] + [tex]K_2SO_4[/tex] → [tex]2KNO_3[/tex] + [tex]SrSO_4[/tex] (if the unknown is strontium nitrate)

[tex]Mg(NO_3)_2[/tex] + [tex]K_2SO_4[/tex] → [tex]2KNO_3[/tex] + [tex]MgSO_4[/tex] (if the unknown is magnesium nitrate)

To determine which reaction occurred, you would need to observe which products were formed. If [tex]SrCO_3[/tex] or [tex]SrSO_4[/tex] were formed, then the unknown was strontium nitrate.

If [tex]MgCO_3[/tex] or [tex]MgSO_4[/tex] were formed, then the unknown was magnesium nitrate.

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Answer:

4 valence electrons.

Explanation:

Carbon has 4 valence electrons because it is in the 14th group on the Periodic Table.