Answer:
To separate a metal from its ore using acid and preserving desirable products such as gold.
Explanation:
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Which of the following sets of descriptors matches the molecule below?
Image of two hydrogen atoms bonded to one oxygen atom to form H2O, or water.
A. Simple structure, molecule, single bonds, two elements
B. One element, triple bond, molecule, diatomic
C. Giant structure, single bond, compound, one element
D. Compound, allotrope, double bond, giant structure
Answer: A. Simple structure, molecule, single bonds, two elements
NH3 is produced by the reaction of 0.450 moles of N2 and 0.600 moles of H2 according to the following equation: 2N2 + 3H2 ⟶ 2NH3. (a) How many moles of NH3 are produced? (b) What is the percent yield if 5.52g of NH3 is produced?
The moles of nitrogen produced is 0.40 moles of ammonia.
The Percent yield of ammonia is 81.2%
What moles of ammonia is produced?The moles of ammonia produced is obtained from the mole ratio of the reaction.
The mole ratio of hydrogen to nitrogen is 3 : 2
Based on the mole ratio, the limiting reactant is hydrogen.
Moles of nitrogen produced = 0.600 * 2/3 = 0.40 moles of ammonia.
mass of ammonia expected = 0.4 * 17 g = 6.8 g
Percent yield = 5.52/6.8 * 100% = 81.2%
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determine how many grams of N2 are produced from the reaction of 8.73
g of H2O2 and 5.16
g of N2H4.
Taking into account the reaction stoichiometry, 4.515 grams of N₂ can be produced from 8.73 grams of H₂O₂ and 5.16 grams of N₂H₄.
Reaction stoichiometryIn first place, the balanced reaction is:
N₂H₄ + 2 H₂O₂ → N₂ + 4 H₂O
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
N₂H₄: 1 mole H₂O₂: 2 molesN₂: 1 mole H₂O: 4 molesThe molar mass of the compounds is:
N₂H₄: 32 g/moleH₂O₂: 34 g/moleN₂: 28 g/moleH₂O: 18 g/moleThen, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:
N₂H₄: 1 mole ×32 g/mole= 32 gramsH₂O₂: 2 moles ×34 g/mole= 34 gramsN₂: 1 mole ×28 g/mole= 28 gramsH₂O: 4 moles ×18 g/mole= 18 gramsLimiting reagentThe limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.
Limiting reagent in this caseTo determine the limiting reagent, it is possible to use a simple rule of three as follows: if by stoichiometry 34 grams of H₂O₂ reacts with 32 grams of N₂H₄, 8.73 grams of H₂O₂ reacts with how much mass of N₂H₄?
[tex]mass of N_{2} H_{4} =\frac{8.73 grams of H_{2} O_{2}x 32 grams of N_{2} H_{4} }{34grams of H_{2} O_{2}}[/tex]
mass of N₂H₄= 8.22 grams
But 8.22 grams of N₂H₄ are not available, 5.16 grams are available. Since you have less mass than you need to react with 8.73 grams of H₂O₂, N₂H₄ will be the limiting reagent.
Mass of N₂ formedConsidering the limiting reagent, the following rule of three can be applied: if by reaction stoichiometry 32 grams of N₂H₄ form 28 grams of N₂, 5.16 grams of N₂H₄ form how much mass of N₂?
[tex]mass of N_{2} =\frac{5.16 grams of N_{2} H_{4} x28 grams of N_{2}}{32 grams of N_{2} H_{4} }[/tex]
mass of N₂= 4.515 grams
Then, 4.515 grams of N₂ can be produced from 8.73 grams of H₂O₂ and 5.16 grams of N₂H₄.
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A cup of water is warmed from 29 °C to 97 °C. What is the difference between these two temperatures, in kelvins
Answer:
I believe it is 68
Explanation:
to convert Celsius to kelvins you must add it to 273.15 for example 29 + 273.15 is 302.15
im so very sorry if im wrong.
Read the given equation.
2Na+ 2H₂O 2NaOH + H₂
During a laboratory experiment, a certain quantity of sodium metal reacted with water to produce sodium hydroxide and hydrogen gas. What was the initial quantity of
sodium metal used if 7.80 liters of H₂ gas were produced at STP?
07:29 grams
09.30 grams
12.2 grams
16.0 grams
Calcular la normalidad de 1 Kg de sulfuro de aluminio en 5000 ml de solucion.
Calculate the normality of 1 Kg of aluminum sulfide in 5000 ml of solution.
Normality comes out to be 8.11
Given Mass of solute: 1000gVolume of solution (V): 5000 ml = 5 liters Equivalent mass of solute (E) = molar mass / n-factorn-factor for [tex]Al_{2}S_{3}[/tex] is 6 and molar mass is 148g
So, on calculating equivalent mass is equal to 24.66g
FORMULAE of Normality (N) = (Mass of the solute) / (Equivalent mass of the solute (E) × Volume of the solution (V)
N=[tex]\frac{1000}{24.66*5}[/tex]
N=8.11
Therefore, normality of 1 kg aluminum sulfide is 8.11
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Question 5 of 30
Which best describes a gamma ray that is given off during nuclear decay?
A. High-energy electromagnetic waves
B. A stream of small, positively charged particles
C. Low-energy electromagnetic waves
D. A stream of small, negatively charged particles
Gamma rays are high-energy electromagnetic waves given off during nuclear decay; option A.
What are electromagnetic waves?Electromagnetic waves are waves which are produced as a result of the interaction of the magnetic and electric fields.
Types of electromagnetic waves include gamma rays, radio waves, ultraviolet waves.
Gamma rays are high-energy electromagnetic waves given off during nuclear decay
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A vessel with a volume of 25.1 L contains 2.80 g of nitrogen gas, 0.605 g of hydrogen gas, and 79.9 g of argon gas. At
25°C, what is the pressure in the vessel?
Select one:
a. 58.7 atm
b. 2.73 atm
c. 0.196 atm
d. 81.0 atm
e. 2.34 atm
2.73 atm is the pressure in the vessel. Hence, option B is correct.
What is an ideal gas equation?The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).
PV=nRT, where n is the moles and R is the gas constant. Then divide the given mass by the number of moles to get molar mass.
Given data:
P= ?
V= 25.1 L
[tex]n= \frac{m}{molar \;mass \;of \;nitrogen} + \frac{m}{molar \;mass \;of \;hydrogen } +\frac{m}{molar \;mass \;of \;argon}[/tex]
[tex]n= \frac{2.80 g}{14} + \frac{0.605 g}{1} +\frac{79.9 g}{40}[/tex]
n= 2.8025
R= [tex]0.082057338 \;L \;atm \;K^{-1}mol^{-1}[/tex]
T=25°C + 273= 298 K
Putting value in the given equation:
[tex]\frac{PV}{RT}=n[/tex]
[tex]2.8025 = \frac{P\; X \;25.1 \;L}{0.082057338 \;L \;atm \;K^{-1}mol^{-1} X 298}[/tex]
P = 2.73 atm
2.73 atm is the pressure in the vessel. Hence, option B is correct.
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How many valence electrons does Rb (rubidium) have?
Answer:
The total number of electrons in a valence shell is called valence electrons. The electron configuration of rubidium shows that the last shell of rubidium has an electron. Therefore, the valence electrons of rubidium(Rb) are one.
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In the scientific sense the two examples of people doing work is: A and D
Meaning of WorkWork can be defined as a result of applying force to a particular object that changes its displacement in the direction of the applied force.
Work can only be done when their is a force that is being applied and a displacement that occurs.
In conclusion, In the scientific sense the two examples of people doing work is: A and D
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Which of the following tool components is unlikely to present a hazard
Gloves is the tool component which will unlikely present a hazard in this scenario.
What is Hazard?
This is referred to as potential source of harm when performing various types of activities.
Gloves will unlikely cause harm as it is used to prevent the risk of electric shock when handling electrical devices which is why it is the most appropriate choice.
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Pure water boils at 100°C.
What happens to the water particles when water
boils?
A They gain energy and move further apart.
B They gain energy and stay close together.
C They lose energy and move further apart.
D They lose energy and stay close together.
Answer:
A
Explanation:
What is the electron configuration of a sodium atom?
1s¹, 2s², 2p6, 356
1s¹, 2s2, 2p6, 3s¹
2s², 2s², 2p6, 3s¹
1s², 2s², 2p6, 3s¹
Answer:
1s²,2s²,2p6,3s¹.Atomic no. of sodium is 11electronic configuration = 2,8,1.that Is 1s²,2s²,2p6,3s1.for electromic configuration - only 2 electron can be there in a single orbital there are 1 s orbital, 3 p orbital ...and so on.equivalent weight of cacl2
Answer:
55 grams
Explanation:
55 grams of calcium chloride is the equivalent weigh because 55 grams of calcium chloride would supply one mole of positive or negative charges when dissolved in water.
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Al + 0₂ → Al₂O3 help
Answer:
4Al +3O₂ → 2Al₂O₃
Explanation:
To balance the chemical equation, start by identifying the number of atoms of each element on both sides of the equation.
Al +O₂ → Al₂O₃
Reactants (right-hand side of the arrow)
Al➭ 1
O➭ 2
Products (left-hand side of the arrow)
Al➭ 2
O➭ 3
Balancing the equation means that we need to ensure the number of atoms of each element is the same on both sides of the equation.
Let's balance the number of O atoms.
Al +3O₂ → 2Al₂O₃
Reactants
Al➭ 1
O➭ 3(2)= 6
Products
Al➭ 2(2)= 4
O➭ 2(3)= 6
Balancing the number of Al atoms:
4Al +3O₂ → 2Al₂O₃
Reactants
Al➭ 4
O➭ 6
Products
Al➭ 4
O➭ 6
The equation is now balanced.
Additional:
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The properties of an element depend on the electron structure within its atoms. The electrons are arranged in different
orbitals, at different energy levels and sublevels. Match each sublevel to the maximum number of electrons it can
accommodate?
The electrons are arranged in different orbitals, at different energy levels and sublevels.
What are Orbitals ?An atomic orbital is a function describing the location and wave-like behavior of an electron in an atom.
This function can be used to calculate the probability of finding any electron of an atom in any specific region around the atom's nucleus.
Following are the sublevel with the maximum number of electrons that can be accommodated by it ;
2 Electrons : S-SubshellTherefore, S-Subshell has 2 electrons, P-subshell has 3 electrons, d-subshell has 10 electrons and f-subshell has 14 electrons.
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Which of the following is non polar covalent bond?
electronegativities:
C = 2.5, H = 2.1, P = 2.1, Cl = 3.0, N = 3.0, O = 3.5
N -O
N-Cl
P-O
H-Cl
Answer:
N-Cl
Explanation:
Look at the chart below. Since N-Cl bond has a electronegativity difference of (3.0-3.0) zero, they are non-polar.
What would be the mass, in grams, of 2.408 x 1024 molecules of tetraphosphorus decaoxide?
Answer:
1,135 grams P₄O₁₀
Explanation:
To find the mass, you need to (1) convert molecules to moles (via Avogadro's Number) and then (2) convert moles to grams (via molar mass from periodic table values). It is important to arrange the ratios/ conversions in a way that allows for the cancellation of units (the desired unit should be in the numerator). The final answer should have 4 sig figs to reflect the given value (2.408 x 10²⁴).
Avogadro's Number:
1 mole = 6.022 x 10²³ molecules
tetraphosphorus decaoxide = P₄O₁₀
Molar Mass (P₄O₁₀): 4(30.974 g/mol) + 10(15.998 g/mol)
Molar Mass (P₄O₁₀): 283.876 g/mol
2.408 x 10²⁴ molecules P₄O₁₀ 1 mole 283.876 g
------------------------------------------- x ------------------------------------ x -----------------
6.022 x 10²³ molecules 1 mole
= 1,135 grams P₄O₁₀
3A. The following skeletal oxidation-reduction reaction occurs under basic conditions. Write the balanced REDUCTION half reaction.
Cl- + SiO32- Cl2 + Si
Reactants Products
3B.
The following skeletal oxidation-reduction reaction occurs under basic conditions. Write the balanced OXIDATION half reaction.
Bi + HPO32-Bi(OH)3 + H2PO2-
Reactants Products
4A. The following skeletal oxidation-reduction reaction occurs under acidic conditions. Write the balanced REDUCTION half reaction.
Cd + SO42- Cd2+ + H2SO3
Reactants Products
4B. The following skeletal oxidation-reduction reaction occurs under acidic conditions. Write the balanced OXIDATION half reaction.
Mn2+ + NiO2MnO4- + Ni2+
Reactants Products
The balanced redox equations of the reactions are:
[tex]SiO_{3}^{2-} + 3\:H_{2}O + 4\:e^{-} \rightarrow Si + 6\:OH^{-}[/tex][tex]2\:Bi + 6\:OH^{-} \rightarrow 2\:Bi(OH)_{3} + 6\:e^{-}[/tex] [tex]SO_{4}^{2-} + 4\:H^{+} + 2\:e^{-} \rightarrow H_{2}SO_{3} + H_{2}O[/tex][tex]Mn^{2+} + 4\:H_{2}O \rightarrow MnO_{4}^{-} +8\:H^{+} + 5\:e^{-}[/tex]What are balanced redox equations?Balanced redox equations are those in which the atoms and electrons transferred are equal on both sides of the equation.
The balanced redox equations of the reactions are given below:
(3a) Balanced REDUCTION half reaction of the equation under basic conditions:
[tex]SiO_{3}^{2-} + 3\:H_{2}O + 4\:e^{-} \rightarrow Si + 6\:OH^{-}[/tex](3b)Balanced OXIDATION half reaction of the equation under basic conditions:
[tex]2\:Bi + 6\:OH^{-} \rightarrow 2\:Bi(OH)_{3} + 6\:e^{-}[/tex](4a) Balanced REDUCTION half reaction of the equation under acidic conditions:
[tex]SO_{4}^{2-} + 4\:H^{+} + 2\:e^{-} \rightarrow H_{2}SO_{3} + H_{2}O[/tex](4b) Balanced OXIDATION half reaction of the equation under acidic conditions:
[tex]Mn^{2+} + 4\:H_{2}O \rightarrow MnO_{4}^{-} +8\:H^{+} + 5\:e^{-}[/tex]Therefore, the balanced oxidation and reduction half reactions are balanced by adding the numerical coefficients to the reacting species as well hydrogen ions, hydroxide ions, water molecules and electrons to the appropriate side of the reactions.
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A 8.63 g sample of a compound contains 5.51 g of iron, Fe, 1.02g of phosphorus, P, and oxygen, O. Calculate the empirical formula for the compound
The empirical formula for the compound is [tex]Fe_3PO_4[/tex] if A 8.63 g sample of a compound contains 5.51 g of iron, Fe, 1.02g of phosphorus, P, and oxygen, O.
What is the empirical formula?An empirical formula tells us the relative ratios of different atoms in a compound.
We need to calculate the number of moles:
Given data:
Mass of iron - 5.51 g
Mass of phosphorus -1.02g
Mass of oxygen -2.1 g
Moles of iron - [tex]\frac{mass}{molar \;mass}[/tex]
Moles of iron - [tex]\frac{5.51 g}{56 g/mol}[/tex]
0.098 mole
Moles of phosphorus [tex]-\frac{mass}{molar \;mass}[/tex]
Moles of phosphorus - [tex]\frac{1.02g}{31 g/mol}[/tex]
0.032 moles
Moles of oxygen -[tex]\frac{mass}{molar \;mass}[/tex]
Moles of oxygen - [tex]\frac{2.1 g}{16 g/mol}[/tex]
0.13moles
Dividing each mole using the smallest number that is divided by 0.032moles.
Fe:P:O :: 3:1:4
The empirical formula for the compound is [tex]Fe_3PO_4[/tex].
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If 44.7 g of KCI (MM = 74.55 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of KCI in the resulting solution?
1.199 M is the concentration of KCI in the resulting solution.
What are moles?A mole is defined as 6.02214076 × [tex]10^{23}[/tex] of some chemical unit, be it atoms, molecules, ions, or others. The mole is a convenient unit to use because of the great number of atoms, molecules, or others in any substance.
No.of moles of KCI
[tex]Moles = \frac{mass}{molar \;mass}[/tex]
[tex]Moles = \frac{44.7 g}{74.5513 g/mol}[/tex]
= 0.599 moles
Vol.of the solution,V= 500 ml
= 0.5 liter
Molarity
[tex]Molality = \frac{Moles \;solute}{Volume \;of \;solution \;in \;litre}[/tex]
[tex]Molality = \frac{0.599 moles}{0.5 liter}[/tex]
= 1.199 M
Hence, 1.199 M is the concentration of KCI in the resulting solution.
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draw a diagram to show how you will separate the salt from sugar using the solvent ethanol
If 4.5 moles of an ideal gas has a temperature of 286 K and a pressure 9.4 atm, what is the volume of the container
Answer:
V = 11 L
Explanation:
To find the missing value, you need to use the Ideal Gas Law. The equation looks like this:
PV = nRT
In this formula,
----> P = pressure (atm)
----> V = volume (L)
----> n = number of moles
----> R = constant (0.0821 atm*L/mol*K)
----> T = temperature (K)
You have been given all of the values in the correct units. Therefore, you can plug these values into the equation and simplify to find volume. The answer should have 2 sig figs to match the given value with the lowest amount of sig figs.
PV = nRT
(9.4 atm)V = (4.5 moles)(0.0821 atm*L/mol*K)(286 K)
(9.4 atm)V = 105.6627
V = 11 L
A scientist places a large beaker containing 325 g of 50degree Celsius water into a microwave. He has to run the microwave for 3 minutes until the water reaches a temperature at 92 degree Celsius. Calculate the amount of energy absorbed by the water.
The amount of energy absorbed by the 325g of water is 57,057J. Details about calorimetry can be found below.
How to calculate energy?The energy absorbed by a mass of substance can be calculated using the following formula;
Q = mc∆T
Where;
Q = quantity of heat absorbedm = mass of substancec = specific heat capacity∆T = change in temperatureQ = 325g × 4.18 × (92 - 50)
Q = 57,057J
Therefore, the amount of energy absorbed by the 325g of water is 57,057J.
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Here: Describe the non metal elements .What group number are non metals
Answer:
A nonmetal is a chemical element that generally lacks a predominance of metallic properties. Non-metals are mostly found in groups 5, 6 and 7. These non-metals will have 5, 6 or 7 electrons in the outer shell.
The outer shell of a non-metal is, therefore, more than half full of electrons.
Fe + H₂O → Fe3O4+H₂ help
Answer:
3Fe + 4H₂O --> Fe3O4 + 4H2
The heat of fusion of water is 79.9cal/g, the heat of vaporization of water is 540cal/g, and the specific heat of water is 1.00cal/deg/g. How much ice at 0 celsius could be converted to steam at 100 celsius by 9522cal of heat?
The amount of ice converted into steam is 13.23 gram.
What is Heat of Vaporisation ?Heat of Vaporisation is the amount of heat required to convert 1 gm to liquid at its boiling point to vapour.
Let x gram of ice is there
At first x gm of ice will melt
The heat required is x * Heat of fusion = x * 79.9 = 79.9x
Then the heat required to rise the temperature of x gm of water from 0 degree to 100 degree Celsius .
= mc ΔT
= x * 1 * 100 = 100x
The heat required to convert x gm of liquid into x gm of steam
= x * 540 = 540x
The total heat supplied is 9522 cal
79.9x + 100x + 540x = 9522
719.9 x = 9522
x = 13.23 gm
The amount of ice converted into steam is 13.23 gram.
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Which TWO of the following processes will increase the concentration of al solution?
(a) Increase the amount of solute.
(b) Decrease the amount of solute.
(c) Increase the amount of solvent.
(d) Decrease the amount of solvent.
Answer:
B decrease the amount of solute
10. How many grams of CoCl₂ in 0.5 liters would be used to make a 1.0 molar solution? I
a. Predict the outcome if 0.5 liters of water is added to 0.5 liters of 0.70M solution of CuSO4
b. Describe what could happen is there is evaporation in the original 0.5 liters of 0.70M
solution of CuSO4
The weight of CoCl₂ used to make 0.5 ltr 1 Molar solution is 49.5g.
How to Calculate weight of substance ?The weight of a substance can be calculated by multiplying the number of moles of the substance by its molar mass.
However,
the number of moles of CoCl₂ must be calculated using the following formula:
no of moles = 0.5L × 1M
no of moles = 0.5moles
Molar mass of CoCl₂ = 99g/mol
mass of CoCl₂ = 0.5 × 99
mass of CoCl₂ = 49.5g
Hence, the weight of CoCl₂ used to make 0.5 ltr 1 Molar solution is 49.5g.
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Please help !!!
Suppose there are 29.9 g of butane gas in a barbecue lighter. How many moles of butane gas is that ?
