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EQUATIONS and STOICHIOMETRY PRACTICE TEST
1. Consider the combustion of carbon monoxide with oxygen gas to produce carbon dioxide. Starting with
3.60 moles of carbon monoxide, calculate the grams of carbon dioxide produced. 2 CO + O2 → 2 CO2
a) 158
b) 5.66
c) 79.2
d) 2.83
2. Silicon tetrachloride can be prepared by heating silicon in chlorine gas. How many moles of chlorine gas
must be used to produce 201 g of silicon tetrachloride? The unbalanced reaction is as follows:
Si + Cl2 → SiCl4
a) 1.18
b) 2.36
c) 168
d) 83.9
3. If you drop 12 moles of copper into a beaker containing nitric acid, how many moles of NO would be
produced? 3 Cu + 8 HNO3 → 3 Cu(NO3)2 + 2 NO + 4 H2O
a) 2.0
b) 4.0
c) 8.0
d) 12
4. How many liters of oxygen gas react completely with 1.2 L of hydrogen at STP? 2 H2 + O2 → 2 H2O
a) 1.2 L
b) 0.60 L
c) 2.4 L
d) 4.8 L
5. CaCO3 → CaO + CO2
If 50.0 g of CaCO3 react, how many liters of CO2 are produced at STP?
a) 1.14 L
b) 25.5 L
c) 11.2 L
d) 0.500 L
6. When the equation for the double replacement reaction below is balanced, what will be the coefficient for
KCl?
SnCl4 + K3PO4 → Sn3(PO4)4 + KCl
a) 3
b) 4
c) 6
d) 12
7. The coefficients in a chemical equation represent the _____.
a) masses in grams of all reactants and products
b) relative number of moles of reactants and products
c) number of atoms of each element in each compound in a reaction
d) number of valence electrons involved in a reaction
8. In a chemical reaction, the mass of the products
a) is less than the mass of the reactants
b) is greater than the mass of the reactants
c) is equal to the mass of the reactants
d) has no relationship to the mass of the reactants
9. Calculate the moles of HNO3 that are needed to neutralize 24.5 moles of Ca(OH)2.
2 HNO3 + Ca(OH)2 → Ca(NO3)2 + 2 H2O
a) 12.3 mol
b) 49.0 mol
c) 22.4 mol
d) 24.5 mol
Use pages 6 and 7 of the NCDPI Reference Tables for Chemistry where applicable.
10. tin + iron (II) sulfate →
a) Sn + FeSO4 → SnSO4 + Fe
c) Sn + FeSO3 → SnSO3 + Fe
11. silver nitrate + nickel (II) chloride →
a) Ni2+ + 2 NO31- → Ni(NO3)2
b) Ni + 2 NO3 → Ni(NO3)2
c) Ag1+ + Cl1- → AgCl
d) Ag + Cl → AgCl
{HINT: Use tin (II)}
b) 2 Sn + Fe(SO4)2 → 2 SnSO4 + Fe
d) no reaction
What is the net ionic equation?
Equations and Stoichiometry Practice Test - page 1
12. zinc iodide + bromine →
a) ZnI + Br → ZnBr + I
c) ZnI2 + Br2 → ZnBr2 + I2
b) 2 ZnI + Br2 → 2 ZnBr + I2
d) no reaction
13. chromium (III) selenide →
a) CrSe3 → Cr + 3 Se
c) 2 Cr2Se3 → 4 Cr + 3 Se2
b) 2 CrSe3 → 2 Cr + 3 Se2
d) Cr2Se3 → 2 Cr + 3 Se
14. calcium oxide + water →
a) CaO + H2O → H2CaO2
c) CaO + H2O → Ca(OH)2
b) Ca2O + H2O → Ca(OH)2
d) CaO + H2O → 2 CaOH
15. sulfur dioxide + water →
a) SO2 + H2O → H2SO4
c) S2O + H2O → 2 HSO
b) SO2 + H2O → H2SO3
d) S2O + H2O → H2SO3
16. tin + oxygen gas →
a) 2 Sn + O2 → 2 SnO
c) Sn + O → SnO
{HINT: Use tin (II)}
b) Sn + O2 → SnO2
d) Sn + 2 O → SnO2
17. mercury (II) chlorate →
a) 2 HgClO3 → HgCl2 + 3 O2
c) Hg(ClO3)2 → HgCl + 3 O2
b) 2 HgClO3 → 2 HgCl + 3 O2
d) Hg(ClO3)2 → HgCl2 + 3 O2
18. gold (I) carbonate →
a) Au2CO3 → Au2O + CO2
c) Au2(CO3)3 → 2 AuO + 3 CO2
b) Au2CO3 → AuO + CO2
d) Au2(CO3)3 → Au2O3 + 3 CO2
19. sodium sulfate + barium nitrate →
a) BaSO4
b) NaNO3
Predict the products. What is formula for the precipitate formed?
c) Ba2(SO4)2
d) Na(NO3)2
20. sodium + water (cold) →
a) Na + H2O → NaOH + 2 H
c) 2 Na + 2 H2O → 2 NaOH + H2
b) 2 Na + H2O → Na2O + H2
d) no reaction
Classify the following unbalanced reactions. Choose (a) for synthesis, (b) for decomposition,
(c) for single-replacement, (d) for double-replacement, and (e) for combustion.
___ 21. H3PO3 → P2O3 + H2O
___ 22. Li + Fe(C2H3O2)3 → LiC2H3O2 + Fe
___ 23. Al + H2 → AlH3
___ 24. Sn(ClO3)2 → SnCl2 + O2
___ 25. Ag2CO3 → Ag2O + CO2
___ 26. C5H8 + O2 → CO2 + H2O
___ 27. HBr + NH4OH → NH4Br + H2O
___ 28. BaO + H2O → Ba(OH)2
29. The equation A + BX → AX + B is the general equation for a _____ reaction.
a) double-replacement
b) decomposition
c) single-replacement
Equations and Stoichiometry Practice Test - page 2
d) combustion