mod 8 chem
2 NH3 + 3 CuO --> 3 Cu + N2 + 3 H2O In the above equation how many moles of N2 can be made when 148.6 grams of CuO are consumed? Round your answer to the nearest tenth. Use the following molar masses: Hydrogen = 1 Nitrogen = 14 Copper = 63.5 Oxygen = 16
.6
3 Cu + 8HNO3 --> 3 Cu(NO3)2 + 2 NO + 4 H2O In the above equation how many moles of water can be made when 101.1 grams of HNO3 are consumed? Round your answer to the nearest tenth. Use the following molar masses: Hydrogen = 1 Nitrogen = 14 Copper = 63.5 Oxygen = 16
.8
S + 6 HNO3 --> H2SO4 + 6 NO2 + 2 H2O In the above equation how many moles of water can be made when 190.7 grams of HNO3 are consumed? Round your answer to the nearest tenth. Use the following molar masses: Hydrogen = 1 Nitrogen = 14 Sulfur = 32 Oxygen = 16
1
3 Cu + 8HNO3 --> 3 Cu(NO3)2 + 2 NO + 4 H2O In the above equation how many grams of water can be made when 8 grams of HNO3 are consumed? Round your answer to the nearest tenth. Hydrogen = 1 Nitrogen = 14 Copper = 63.5 Oxygen = 16
1.1
3 Cu + 8HNO3 --> 3 Cu(NO3)2 + 2 NO + 4 H2O In the above equation how many moles of water can be made when 178.9 grams of HNO3 are consumed? Round your answer to the nearest tenth. Use the following molar masses: Element Molar Mass Hydrogen = 1 Nitrogen = 14 Copper = 63.5 Oxygen = 16
1.4
S + 6 HNO3 --> H2SO4 + 6 NO2 + 2 H2O In the above equation how many moles of H2SO4 can be made when 65 moles of HNO3 are consumed?
11
Sodium chlorate decomposes into sodium chloride and oxygen gas as seen in the equation below. 2NaClO3 --> 2NaCl +3O2 How many moles of O2 were produced by 7 moles of NaClO3? Round your answer to the nearest whole number.
11
S + 6 HNO3 --> H2SO4 + 6 NO2 + 2 H2O In the above equation how many moles of water can be made when 59 moles of HNO3 are consumed?
20
2 NH3 + 3 CuO g 3 Cu + N2 + 3 H2O In the above equation how many grams of N2 can be made when 180 grams of CuO are consumed? Round your answer to the nearest tenth. Hydrogen = 1 Nitrogen = 14 Copper = 63.5 Oxygen = 16
21.1
For the reaction C + 2H2 → CH4, how many grams of hydrogen are required to produce 5.4 moles of methane, CH4 ? Round your answer to the nearest tenth. Use the following molar masses: H = 1 C = 12
21.6
2 NH3 + 3 CuO g 3 Cu + N2 + 3 H2O In the above equation how many moles of water can be made when 17 moles of NH3 are consumed?
26
For the reaction 2HNO3 + Mg(OH)2 → Mg(NO3) 2 + 2H2O, how many grams of magnesium nitrate are produced from 3 grams of nitric acid, HNO3 ? Hydrogen = 1 Magnesium = 24 Nitrogen = 14 Oxygen = 16
3.5
For the reaction C + 2H2 → CH4, how many grams of hydrogen are required to produce 8.8 moles of methane, CH4 ? Round your answer to the nearest tenth. Use the following molar masses: H = 1 C = 12
35.2
S + 6 HNO3 → H2SO4 + 6 NO2 + 2 H2O In the above equation, how many grams of water can be made when 6.2 moles of HNO3 are consumed? Round your answer to the nearest tenth. Use the following molar masses: H = 1 N = 14 Sulfur = 32 O = 16
37.2
3 Cu + 8HNO3 --> 3 Cu(NO3)2 + 2 NO + 4 H2O In the above equation how many moles of water can be made when 77 moles of HNO3 are consumed?
39
Sodium chlorate decomposes into sodium chloride and oxygen gas as seen in the equation below. 2NaClO3 --> 2NaCl +3O2 How many grams of NaClO3 were needed to produce 2 grams of O2? Round your answer to the nearest whole number. Sodium = 23 Chlorine = 35.5 Copper = 63.5 Oxygen = 16
4
For the reaction C + 2H2 → CH4, how many moles of hydrogen are needed to make 182 grams of methane, CH4 ? Round your answer to the nearest tenth. Use the following molar masses: Hydrogen = 1 Carbon = 12
45.5
What is the mass of 4 moles of Carbon? (mass is rounded to 1 decimal place)
48.0 g
Sodium chlorate decomposes into sodium chloride and oxygen gas as seen in the equation below. 2NaClO3 --> 2NaCl +3O2 How many moles of NaClO3 were needed to produce 9 moles of O2? Round your answer to the nearest whole number.
6
3 Cu + 8HNO3 → 3 Cu(NO3)2 + 2 NO + 4 H2O In the above equation, how many grams of water can be made when 7.3 moles of HNO3 are consumed? Round your answer to the nearest tenth. Use the following molar masses: H = 1 N = 14 Cu = 63.5 O = 16
65.7
2 NH3 + 3 CuO g 3 Cu + N2 + 3 H2O In the above equation how many moles of N2 can be made when 21 moles of CuO are consumed?
7
3 Cu + 8HNO3 g 3 Cu(NO3)2 + 2 NO + 4 H2O In the above equation how many moles of NO can be made when 37 moles of HNO3 are consumed?
9
Sodium chlorate decomposes into sodium chloride and oxygen gas as seen in the equation below. 2NaClO3 --> 2NaCl +3O2 How many moles of NaCl were produced by 9 moles of NaClO3? Round your answer to the nearest whole number.
9
2 NH3 + 3 CuO → 3 Cu + N2 + 3 H2O In the above equation, how many grams of N2 can be made when 10.1 moles of CuO are consumed? Round your answer to the nearest tenth. Use the following molar masses: H = 1 N = 14 Cu = 63.5 O = 16
94.3
A compound has a chemical composition of 97.6 g carbon, 4.9 g hydrogen, 52 g oxygen, and 45.5 g nitrogen. What is the empirical formula? a) C5H3O2N2 b) C3H3O2N2 c) C10H6O4N4
a
A(n) ___________ formula is one that shows the lowest whole-number ratio of the elements in a compound. a) Empirical b) Chemical c) Molecular
a
Find the percent composition of water in barium chloride dihydrate. Round your answer to the nearest whole number. a) 15% b) 85.3% c) 8%
a
Fluorine gas reacts with a solution of sodium bromide in a single replacement reaction, producing aqueous sodium fluoride and bromine gas. Which of the following is the correct balanced equation for this reaction? a) F2(g) + 2NaBr(aq) ⟶ 2NaF(aq) + Br2(l) b) 2F2(g) + NaBr(aq) ⟶ NaF(aq) + 2Br2(l) c) F2(g) + NaBr(aq) ⟶ NaF(aq) + Br2(l)
a
For the following equation, which is NOT a valid mole ratio? 2SO3 ⟶ 2SO2 + O2 a) 2𝑚𝑜𝑙𝑂2 / 2𝑚𝑜𝑙𝑆𝑂3 b) 2𝑚𝑜𝑙𝑆𝑂3 / 1𝑚𝑜𝑙𝑂2 c) 2𝑚𝑜𝑙𝑆𝑂2 / 2𝑚𝑜𝑙𝑆𝑂3
a
How many atoms of hydrogen atoms are found in 3.94 mol of NH5? a) 1.19 x 1025 hydrogen atoms b) 4.57 x 1021 hydrogen atoms c) 3.395 x 1025 hydrogen atoms
a
How many carbon atoms are present in 0.92 moles of CH3? a) 1.66 x 1024 atoms b) .92 C atoms c) 1.3 x 10-23 atoms
a
How many hydrogen atoms are present in 0.46 moles of NH3? a) 8.3 x 1023 hydrogen atoms b) 2.77 x 1023 hydrogen atoms
a
How many molecules are in 1.95 moles of H2O? a) 1.17 x 1024 molecules b) 1.70 x 1025 molecules c) 35.5 molecules
a
How many moles are there in 2.6 x 1024 atoms of calcium? a) 4.3 moles b) 7.0 x 10-24 moles of Ca c) 168.36 moles
a
How many moles of ammonia are produced when 5.0 moles of hydrogen react with excess nitrogen? 𝑁2(𝑔)+3𝐻2(𝑔)⟶2𝑁𝐻3(𝑔) a) 3.3 mol b) 10.0 mol c) 2.0 mol
a
N2(g) + 3H2(g) ⟶⟶ 2NH3(g) The equation above is the equation for the Haber process. In a certain reaction, you start with 3.0 moles of nitrogen and 5.0 moles of hydrogen. Which molecule is the excess reactant? a) Nitrogen b) Neither is excess c) Hydrogen
a
Name the following hydrate: CuSO4 · 5H2O a) Copper(II) sulfate pentahydrate b) Copper(I) sulfate pentahydrate c) Copper(II) sulfite pentahydrate
a
Name the following hydrate: FeSO4 · 9H2O a) Iron(II) sulfate nonahydrate b) Iron(III) sulfate nonahydrate c) Iron(II) sulfate nine hydrate
a
What factors can contribute to a percent yield that is greater than 100%? a) Impurities in the product b) Allowing too much time for the reaction to occur c) In real life, a percent yield greater than 100% is impossible d) Spills during the experiment
a
What is the empirical formula for C3H6O9? a) CH2O3 b) CH6O3 c) C3H2O3
a
What is the empirical formula for P4O10? a) P2O5 b) P4O5 c) P4O10
a
What is the percent composition of hydrogen in H2O? a) 11.2% b) 18.02% c) 88.8%
a
Which of the following is NOT an empirical formula? a) C6H12O6 b) MgCl2 c) N2O5
a
In a certain reaction, 5.0 moles of hydrogen react with excess nitrogen. To determine how many moles of ammonia (NH3) are produced based on the 5.0 moles of hydrogen, what conversion factor(s) should be used? Select all that apply. 𝑁2 + 3𝐻2 ⟶ 2𝑁𝐻3 a) [3𝑚𝑜𝑙𝐻2 / 2𝑚𝑜𝑙𝑁𝐻3] b) [2𝑚𝑜𝑙𝑁𝐻3 / 5𝑚𝑜𝑙2𝑁2] c) [2𝑚𝑜𝑙𝑁𝐻3 / 3𝑚𝑜𝑙𝐻2]
a c
4Fe(s) + 3O2(g) ⟶⟶ 2Fe2O3(g) In a certain reaction, 27.3 g of iron reacts with 45.8 g of oxygen. How many grams of iron(III) oxide are produced in the reaction? a) 61.3 g b) 39.0 g c) 30.7 g d) 152 g
b
A certain reaction produced 14.80 moles of carbon dioxide. How many moles of both Fe2O3 and CO reacted? 𝐹𝑒2𝑂3 + 3𝐶𝑂 ⟶ 2𝐹𝑒 + 3𝐶𝑂2 a) 14.80 moles of Fe2O3 and 4.933 moles of CO b) 4.933 moles of Fe2O3 and 14.80 moles of CO
b
A compound has a chemical composition of .62 g carbon, .10 g hydrogen, and .28 g oxygen. What is the empirical formula? a) C1.5H6O b) C3H6O c) C6H12O2 d) CHO
b
A compound has a chemical composition of 47% carbon, 6% hydrogen, and 47% oxygen. What is the empirical formula? a) C2H3O1.5 b) C4H6O3 c) CHO
b
A sample of an unknown compound consists of 12.01 g C, 2.02 g H, and 16.0 g O, and has a molar mass of 180 g/mol. What is the molecular formula? a) C3H4O3 b) C6H12O6 c) C6H4O6
b
Calculate the mass of carbon in 250 grams of C2H3O2. a) 27 grams b) 101.73 grams c) 13.22 grams
b
Calculate the mass of oxygen in 250 grams of C2H3O2. a) 47 grams b) 135.44 grams c) 39.17 grams
b
Fluorine gas reacts with a solution of sodium bromide in a single replacement reaction, producing aqueous sodium fluoride and bromine gas. If a reaction starts with 0.480 moles of fluorine gas, how many moles of sodium fluoride are produced? a) 1.92 moles of NaF b) 0.960 moles of NaF c) 0.480 moles of NaF
b
How many molecules are in 3.9 moles of water? a) 6.5 x 10-24 molecules of water b) 2.3 x 1024 molecules of water c) .22 molecules of water
b
How many moles of CO are required to completely react with 2.45 moles of Fe2O3? 𝐹𝑒2𝑂3 + 3𝐶𝑂 ⟶ 2𝐹𝑒 + 3𝐶𝑂2 a) 4.90 mol CO b) 7.35 mol CO c) 1.63 mol CO
b
How many moles of Fe2O3 are necessary to produce 0.824 moles of CO2? 𝐹𝑒2𝑂3 + 3𝐶𝑂 ⟶ 2𝐹𝑒 + 3𝐶𝑂2 a) 0.824 mol Fe2O3 b) 0.275 mol Fe2O3 c) 2.47 mol Fe2O3
b
If the empirical formula of a compound is C2OH4, and the molar mass is 88 g/mol, what is the molecular formula? a) C3O2H5 b) C4O2H8 c) C5O2H6
b
If the empirical formula of a compound is CH2, and the molar mass is 70.0 g/mol, what is the molecular formula? a) C6H12 b) C5H10 c) C3H6
b
If the empirical formula of a compound is known, what is needed in order to determine the molecular formula? a) The coordination numbers b) The molar mass c) The molecular geometry
b
In a chemical reaction, one reactant, called the ___________ reactant, will control the extent of the reaction. A portion of the other reactants, called the ___________ reactants, will remain. a) Excess; limiting b) Limiting; excess c) Control; extra d) Product; extra
b
N2(g) + 3H2(g) ⟶ 2NH3(g) The equation above is the equation for the Haber process. In a certain reaction, you start with 3.0 moles of nitrogen and 5.0 moles of hydrogen. Which molecule is the limiting reactant? a) Nitrogen b) Hydrogen c) Neither is limiting
b
N2(g) + 3H2(g) ⟶⟶ 2NH3(g) The equation above is the equation for the Haber process. In a certain reaction, you start with 3.0 moles of nitrogen and 5.0 moles of hydrogen. How much of the excess reactant will be left over after the reaction? a) 2.0 mol b) 1.3 mol c) 1.67 mol d) 3.3 mol
b
The coefficient of a particular substance in a balanced equation represents ___________. a) Moles b) Moles, molecules, and formula units c) Mass
b
The empirical formula of a compound is CH2. Which could NOT be the molecular formula? a) C4H8 b) C12H22 c) C7H14
b
What is the molar mass of KMnO4? (mass has been rounded to 1 decimal place) K = 39.1 g Mn = 55 g O = 16 g a) 159 g b) 158.1 g c) 110.1 g d) 34,408 g
b
What is the percent composition of sulfur in N2S2? a) 30.4% b) 69.6% c) 15%
b
2HgO(s) ⟶⟶ 2Hg(l) + O2(g) In a certain reaction, 4.37 g of HgO is decomposed, producing 3.21 g of Hg. What is the percent yield of the reaction? a) 126% b) 54.2% c) 79.3% d) 92.5%
c
4Fe(s) + 3O2(g) ⟶⟶ 2Fe2O3(g) In a certain reaction, 27.3 g of iron reacts with 45.8 g of oxygen. What is the limiting reactant? a) O2 b) Fe2O3 c) Fe d) There is no limiting reactant
c
If some of the product is spilled before it is weighed, how will that affect the actual yield? a) It will not affect the actual yield b) The theoretical yield will be less than the actual yield c) The actual yield will be less than the theoretical yield d) This cannot be determined
c
Methyl acetate has a chemical composition of 48.64% carbon, 8.16% hydrogen, and 43.20% oxygen. What is the empirical formula? a) C2H3O b) CHO c) C3H6O2
c
The actual yield of a certain reaction is 44.0 g, while the theoretical yield is 50.0 g. Calculate the percent yield. a) 76.0% b) 80.0% c) 88.0% d) 132%
c
To convert from mass of A to mass of B in a stoichiometry problem, which are the correct steps to follow? a) Mass of A ⟶ Moles of A ⟶ Mass of B b) Mass of A ⟶ Mass of B c) Mass of A ⟶ Moles of A ⟶ Moles of B ⟶ Mass of B d) Mass of A ⟶ Moles of B ⟶ Moles of A ⟶ Mass of B
c
To convert from mass of A to moles of B in a stoichiometry problem, which are the correct steps to follow? a) Mass of A ⟶ Moles of B b) Mass of A ⟶ Mass of B ⟶ Moles of B c) Mass of A ⟶ Moles of A ⟶ Moles of B d) Mass of A ⟶ Moles of A ⟶ Mass of B ⟶ Moles of B
c
What is the name of the procedure that determines the composition of the elements in a compound? a) Mole determination b) Dimensional analysis c) Elemental analysis
c
What is the percent composition of nitrogen in NH4? a) 11.8% b) 47.1% c) 77.6%
c
What pieces of information do we need in order to calculate the percent yield? a) The total number of atoms on both sides of the chemical reaction b) The mass of the reactants and the products c) The maximum amount possible of product and the amount experimentally recovered d) The mole ratio of the reactants and the products
c
Which of the following is(are) conserved in a chemical reaction? a) Both are correct b) Number of molecules c) Number of atoms and mass
c
Write the formula for copper(II) sulfate hexahydrate. a) CuSO4 · 5H2O b) CuSO4 · H2O c) CuSO4 · 6H2O
c
Write the formula for magnesium sulfate trihydrate. a) Mg2SO4 · 3H2O b) MgSO4 · 4H2O c) MgSO4 · 3H2O
c
2HgO(s) ⟶⟶ 2Hg(l) + O2(g) In a certain reaction, 4.37 g of HgO is decomposed, producing 3.21 g of Hg. What is the theoretical yield of Hg? a) 1.74 g b) 3.47 g c) 3.27 g d) 4.05 g
d
Ga2O3(s) + 3SOCl2(l) ⟶⟶ 2GaCl3(s) + 3SO2(g) In a certain reaction, 35.9 g of Ga2O3 reacts with 55.4 g of SOCl2. The GaCl3 produced is collected, and its mass is found to be 48.83 g. What is the limiting reactant? a) SO2 b) Ga2O3 c) GaCl3 d) SOCl2
d
N2(g) + 3H2(g) ⟶⟶ 2NH3(g) The equation above is the equation for the Haber process. If 2.0 moles of nitrogen are available for a reaction, what amount of hydrogen represents the correct stoichiometric ratio? a) 2.0 mol b) 8.0 mol c) 4.0 mol d) 6.0 mol
d
N2(g) + 3H2(g) ⟶⟶ 2NH3(g) The equation above is the equation for the Haber process. In a certain reaction, you start with 3.0 moles of nitrogen and 5.0 moles of hydrogen. How many moles of ammonia will be produced in the reaction? a) 6.0 mol b) 1.7 mol c) 7.5 mol d) 3.3 mol
d
To convert from mass of A to mass of B in a stoichiometry problem, which are the correct steps to follow? a) Mass of A ⟶ Moles of B ⟶ Moles of A ⟶ Mass of B b) Mass of A ⟶⟶ Mass of B c) Mass of A ⟶ Moles of A ⟶ Mass of B d) Mass of A ⟶ Moles of A ⟶ Moles of B ⟶ Mass of B
d
To convert from moles of A to mass of B in a stoichiometry problem, which are the correct steps to follow? a) Moles of A ⟶ Moles of B ⟶ Mass of A b) Moles of A ⟶ Mass of B c) Moles of A ⟶ Moles of B ⟶ Mass of A ⟶ Mass of B d) Moles of A ⟶ Moles of B ⟶ Mass of B
d
What factors can contribute to a percent yield that is less than 100%? a) Incomplete reaction b) Unwanted side reaction c) Spills during the experiment d) All of these
d
