What are the reactants in the reaction?

What are/is the product of the reaction?

Answer:

= 6.21x10^21

Explanation:

It's the train track method, where you try to cancel all the units and end with units that you need. Here we want to end with number of atoms of N.

500 mg N x 1 g N/1000 mg N x 1 mol N/194.19 g N x 4 mol N/1 mol of caffeine x (6.022 x 10^23 particles of N / 1 mol N)

= 6.21x10^21

Answer:

0.07

Explanation:

to find mole you divide mass by the relative atomic mass

Now you find the relative atomic of of moles pf he number sodium sulfide

then you thequation for finding moles to find mole of sodium

Due to its higher oxygen content and based on its structure dietheylene glycol has a higher energy efficiency (cal/g) compared to isopropanol and paraffin wax.

The calorific value of a fuel is the amount of heat energy released from the combustion of the fuel under standard conditions.

Dietheylene glycol, isopropanol and paraffin wax are all used as fuels.

However, due to it higher oxygen content and based on its structure, diethethylene glycol has a higher calorific value than either isopropanol or paraffin wax.

Therefore, dietheylene glycol has a higher energy efficiency (cal/g) compared to isopropanol and paraffin wax.

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The pH of the solution in which 4.85g of HCl is present is 1.3.

pH of the solution will be calculated by using the below equation:
pH = -log[H⁺]

Relation between the mass and moles of any substance will be represented as:

Moles of HCl = 4.85g / 36.4g/mol = 0.13 moles

Given volume = 2.5 L

Concentration in terms of molarity will be calculated as:
M = n/V

M = 0.13mol / 2.5L = 0.05 M

So, 0.05M HCl solution have the same amount of concentration of H⁺ ion. Now pH will be calculated as:

pH = -log(0.05) = 1.3

Hence required pH of the solution is 1.3.

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Answer: Mass of substance / Mass of one mole.

Explanation:

Answer:

As metals are giant lattice structures, the number of electrostatic forces to be broken is extremely large

Explanation:

This means that the melting point and boiling point of metals are more similar to those for ionic compounds than for covalent substances.

Answer:

7.5 kcal

Explanation:

1.0 cal /g-C   * 100 g * (100- 25 C) = 7500 cal = 7.5 kcal

The amount of heat energy necessary to raise the temperature of 100 g of water at room temperature (25°C) to the boiling point (100°C) is 7.5 kcal.

Given to us the mass of water, the specific heat of water, and the change in temperature, we need to calculate the amount of heat energy.

m = 100 g

c = 1.0 cal/g°C

ΔT = (100 °C - 25 °C) = 75 °C

To calculate the amount of heat energy required, we can use the formula:

Q = m × c× ΔT

Where:

Q = heat energy (in calories)

m = mass of water (in grams)

c = specific heat of water (in cal/g°C)

ΔT = change in temperature (in °C)

Substituting the values into the formula:

Q = 100 g × 1.0 cal/g°C × 75 °C

Q = 7500 cal

7500 cal = 7.5 kcal

Therefore, the amount of heat energy required to raise the temperature of 100 g of water from 25 °C to 100 °C is 7500 calories, which is equivalent to 7.5 kcal.

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Balanced chemical equation for the given reaction is Ba(OH)₂(aq) + 2HNO₃(aq) → Ba(NO₃)₂(aq) + 2H₂O(l).

Balanced equations are those equation in which all entities are present in equal amount on the reactant side as well as on the product side of the chemical reaction.

Balanced chemical reaction will be represented as:

Ba(OH)₂(aq) + 2HNO₃(aq) → Ba(NO₃)₂(aq) + 2H₂O(l)

In the above reaction all entities are present in the equal amount on both side of the chemical reaction.

Hence balanced chemical equation is Ba(OH)₂(aq) + 2HNO₃(aq) → Ba(NO₃)₂(aq) + 2H₂O(l).

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Answer:

.846 grams of H2

Explanation:

Answer: Atoms with a lower atomic mass have a greater density than the atom with the higher atomic weight because the atoms are tightly packed together. The volume of a material can change with temperature and pressure. This can also modify the density of the material.

Explanation: HOPE IT HELPS YOU . PLEASE GIVE BRAINLIEST . THANKS .

Answer:

70.1 mL

Explanation:

First let's look at the formula for magnesium nitrate, and get the molar mass, we should end up with Mg(NO3)2 for the formula and this should have a molar mass of 148.3 g/mol.

Lets get the number of moles of the magnesium by taking the number of grams over the molar mass, (21.94 g)/(148.3 g/mol). grams cancel and we're left with approximately 0.148 moles.

Now let's plug our numbers into the molarity formula, M = n/L, this should give us 2.11 mol/L = (0.148 mol)/L, now let's solve for L, divide both sides by 0.148 which will give us 14.26 L^-1 = 1/L now we take the inverse of both sides to get 0.07012 L = L.

Now we have the liters, but the question askes for milliliters, so let's multiply by 1000, and then after rounding to sig figs we will get 70.1 mL as our answer. (Note: I used the exact values instead of the approximations throughout this explanation, so if you calculate the answer by plugging in these values, it might be slightly off.)

Answer:

reactants are hydrogyn and oxygen, the product is water

Explanation:

Reactants are what start the reaction, they are joined together making a reaction that can result in a mix of both or a really new product. The product is, as named, the product of the reactants reaction, it is the outcome. In this case, hydrogen and oxygen join together, making a reaction that ended up with water(the product).

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5.76 g of [tex]O_2[/tex] are consumed when [tex]C_6H_1_2[/tex] is burned to yield 5.3 grams of [tex]CO_2[/tex].

A mole is defined as 6.02214076 × [tex]10^{23}[/tex] of some chemical unit, be it atoms, molecules, ions, or others.

Calculating moles of [tex]CO_2[/tex]

Number of mole of [tex]CO_2[/tex] = [tex]\frac{\;Given \;mass}{\;Molar \;mass}[/tex]

[tex]\frac{\;Given \;mass}{\;Molar \;mass}[/tex] = [tex]\frac{5.3g}{44 g/mol}[/tex] = 0.12 mol

As is clear from the reaction stoichiometry, 9 moles of [tex]O_2[/tex] are consumed to yield 6 moles of [tex]CO_2[/tex].

Calculating the number of moles of [tex]CO_2[/tex]

[tex]\frac{0.12 X 9}{6}[/tex] = 0.18 mol

Mass of [tex]O_2[/tex] consumed is = 0.18 X 32.0 =2.7 g =5.76 g

Hence, 5.76 g of [tex]O_2[/tex] are consumed when [tex]C_6H_1_2[/tex] is burned to yield 5.3 grams of [tex]CO_2[/tex].

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BATHTUB BATHTUB BATHTUB

Answer:

1. East on the box they are facing, West on the side from behind, North on the left side, South on the right side.

2. Because they all were facing towards the sun and the sun rise from east.

3. This one's answer is in the first answer.

4. The picture shows early morning because the shadow of the boys are in a flat position but if would have been late morning then it would not been covering that much area.

Answer:

0.16 atm

Explanation:

Let's look at the formula PV=nRT. First of all, T should be in kelvin, so let's add 273. Now solve for P so we get P = nRT/V.

Now let's plug these in...

P = (0.034 mol)(0.08206 L atm mol^-1 K^-1)(298 K)/5.1 L

After solving and rounding to sig figs we get 0.16 atm

[tex]\qquad\qquad\huge\underline{{\sf Answer}}[/tex]

The Correct choice is A. H+ , F- and HF

Since HF is a weak acid, it behaves like an weak electrolyte in water. so, there is incomplete dissociation of HF in water. Therefore, there will be HF molecules present in the solution along with the ions ~

Answer:

3 moles

Explanation:

The balanced chemical equation between Calcium Hydroxide and Hydrochloric acid is:

Ca(OH)₂ + 2HCl → CaCl₂ + 2H₂O

The ratio of HCl to H₂O is  2 : 2

So if 3 moles of hydrochloric acid is added, 3 moles of water will be formed:

[x is the no of moles of H₂O produced]

2 : 2

3 : x  

[Cross multiply]

2x = 2 × 3

2x = 6

x = [tex]\frac{6}{2}[/tex] = 3 moles

From the calculations and the data provided in the question, the required temperature is 380 K.

The Clasius Clapeyron equation is used to obtain the vapor pressure of a substance at two different temperatures.

Hence;

lnP2/P1 = -ΔHvap/R(1/T2 - 1/T1)

ln(145/1) = -40.7 * 10^3/8.314(1/T2 - 1/273)

4.977 = -(4811)(1/T2 - 1/273)

4.977/-(4811) = (1/T2 - 1/273)

-0.00103 = 1/T2 - 1/273

-0.00103 +  1/273 =  1/T2

0.002633 =1/T2

T2 = 380 K

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The percent yield of methane is 85.5%.

The percent yield of a reaction is the ratio of the actual yield and the expected yield expressed as a percentage.

Equation of reaction is given below:

1 mole of methane produces 2 moles of water

16 g of methane produces 36 grams of water

52 g of methane will produce 117 g of water

Percent yield = 100/117 × 100% = 85.5%

Therefore, the percent yield of methane is 85.5%.

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1) Heat is transferred from the bath to the bottle. This will cause the temperature of the gas molecules to increase, and thus their kinetic energy will increase. As a result, the size of the balloon will increase.

2) The size of the balloon would decrease because since the temperature is decreasing, the particles have less kinetic energy, and thus are packed more closely together.

Answer:

17.92L or 17.92dm³1

Explanation:

number of moles of a gas = volume of that gas/ 22.4(S.V.P)

0.8 mol = x / 22.4

cross multiplication

x = 22.4 × 0.8

x = 17.92

:. the volume of 0.8 mol of nitrogen gas is 17.92dm³ or 17.92L

5.76 g of [tex]O_2[/tex] are consumed when [tex]C_6H_1_2[/tex] is burned to yield 5.3 grams of [tex]CO_2[/tex].

A mole is defined as 6.02214076 × [tex]10^{23}[/tex] of some chemical unit, be it atoms, molecules, ions, or others.

Calculating moles of [tex]CO_2[/tex]

Number of mole of [tex]CO_2[/tex] = [tex]\frac{\;Given \;mass}{\;Molar \;mass}[/tex]

[tex]\frac{\;Given \;mass}{\;Molar \;mass}[/tex] = [tex]\frac{5.3g}{44 g/mol}[/tex] = 0.12 mol

As is clear from the reaction stoichiometry, 9 moles of [tex]O_2[/tex]6 moles of [tex]CO_2[/tex].

Calculating the number of moles of [tex]CO_2[/tex]

[tex]\frac{0.12 X 9}{6}[/tex] = 0.18 mol

Mass of [tex]O_2[/tex] =5.76 g

Hence, 5.76 g of [tex]O_2[/tex] are consumed when [tex]C_6H_1_2[/tex] yield 5.3 grams of [tex]CO_2[/tex].

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The following steps can be taken

Answer:

The volume of the gas decreases.Explanation:

Answer:

0.72 grams

Explanation:

Dalton's Law

P tot = P H₂O + P gas

769 = 23.8 + P gas

P gas = 745.2 torr

Answer:

The vapor pressure of the pure solvent will be equal to 55.7 mmHg.

You're dealing with a solution of sucrose, which is your solute, dissolved in ethanol, which is your solvent.

Since sucrose is a non-volatile solute, the vapor pressure of the solution can be expressed using the mole fraction of the solvent - this is known as Raoult's Law.

P

solution

=

χ

solvent

⋅

P

∘

solvent

, where

P

solution

- the vapor pressure of the solution;

χ

solvent

- the mole fraction of the solvent;

P

∘

solvent

- the vapor pressure of the pure solvent.

The mole fraction of the solvent is defined as the number of moles of ethanol divided by the total number of moles present in the solution.

Use sucrose and ethanol's respective molar masses to determine how many moles of each you have

10.0

g

⋅

1 mole sucrose

342.3

g

=

0.0292 moles sucrose

and

100.0

g

⋅

1 mole ethanol

46.07

g

=

2.171 moles ethanol

The total number of moles will be

n

total

=

0.0292

+

2.171

=

2.20 moles

The vapor pressure of the pure solvent will thus be

P

∘

solvent

=

P

solution

χ

solvent

P

∘

solvent

=

55.0 mmHg

2.171

moles

2.20

moles

=

55.7 mmHg

Explanation: