Chapter 9 – Review
9.1 Stoichiometry Basics; and 9.2 Mole-Mass and Mass-Mass Calculations
- Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following:
- The number of moles and the mass of chlorine, Cl2, required to react with 10.0 g of sodium metal, Na, to produce sodium chloride, NaCl.
- The number of moles and the mass of oxygen formed by the decomposition of 1.252 g of mercury(II) oxide.
- The number of moles and the mass of sodium nitrate, NaNO3, required to produce 128 g of oxygen. (NaNO2 is the other product.)
- The number of moles and the mass of carbon dioxide formed by the combustion of 20.0 kg of carbon in an excess of oxygen.
- The number of moles and the mass of copper(II) carbonate needed to produce 1.500 kg of copper(II) oxide. (CO2 is the other product.)
- Determine the number of moles and the mass requested for each reaction in Q.1 a) to f) above. Check Answer: [1]
- Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following
- The number of moles and the mass of Mg required to react with 5.00 g of HCl and produce MgCl2 and H2.
- The number of moles and the mass of oxygen formed by the decomposition of 1.252 g of silver(I) oxide.
- The number of moles and the mass of magnesium carbonate, MgCO3, required to produce 283 g of carbon dioxide. (MgO is the other product.)
- The number of moles and the mass of water formed by the combustion of 20.0 kg of acetylene, C2H2, in an excess of oxygen.
- The number of moles and the mass of barium peroxide, BaO2, needed to produce 2.500 kg of barium oxide, BaO (O2 is the other product.)
- Determine the number of moles and the mass requested for each reaction in Q3. a) to f) above. Check Answer: [2]
- I2 is produced by the reaction of 0.4235 mol of CuCl2 according to the following equation: [latex]2\text{CuCl}_2 + 4\text{KI} \longrightarrow 2\text{CuI} + 4\text{KCl} + \text{I}_2[/latex].
(a) What mass of I2 is produced?
- Silver is often extracted from ores such as K[Ag(CN)2] and then recovered by the reaction
[latex]2 \text{K} [\text{Ag(CN)}_2](aq) + \text{Zn}(s) \longrightarrow 2\text{Ag}(s) + \text{Zn(CN)}_2(aq) + 2\text{KCN}(aq)[/latex](a) What mass of Zn(CN)2 is produced? Check Answer: [3] -
What mass of CO2 is produced by the combustion of 1.00 mol of CH4? Check Answer: [4]
CH4(g) + 2O2(g) → CO2(g) + 2H2O(ℓ)
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What mass of H2O is produced by the combustion of 1.00 mol of CH4?
CH4(g) + 2O2(g) → CO2(g) + 2H2O(ℓ)
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What mass of HgO is required to produce 0.692 mol of O2? Check Answer: [5]
2HgO(s) → 2Hg(ℓ) + O2(g)
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What mass of NaHCO3 is needed to produce 2.659 mol of CO2?
2NaHCO3(s) → Na2CO3(s) + H2O(ℓ) + CO2(g)
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How many moles of Al can be produced from 10.87 g of Ag? Check Answer: [6]
Al(NO3)3(s) + 3Ag → Al + 3AgNO3
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How many moles of HCl can be produced from 0.226 g of SOCl2?
SOCl2(ℓ) + H2O(ℓ) → SO2(g) + 2HCl(g)
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How many moles of O2 are needed to prepare