The ideal gas law PV = nRT relates pressure P, volume V, temperature T, and numb

Question

The ideal gas law PV = nRT relates pressure P, volume V, temperature T, and number of moles of a gas, n. The gas constant R equals 0.08206 L middot atm/(K middot mol) or 8.3145 J/(K middot mol). The equation can be rearranged as follows to solve for n: n = PV/RT This equation is useful when dealing with gaseous reactions because stoichiometric calculations involve mole ratios. When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction CaCO_3 (s) rightarrow CaO (s) + CO_2 (g) What is the mass of calcium carbonate needed to produce 77.0 L of carbon dioxide at STP? Express your answer with the appropriate units. Butane, C_4H_10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C_4H_10 (g) + 13O_2 (g) rightarrow 8CO_2 (g) + 10H_2O(l) At 1.00 atm and 23 degree C, what is the volume of carbon dioxide formed by the combustion of 3.80 g of butane? Express your answer with the appropriate units.

Explanation / Answer

A)

Mass required for

V at STP of CO2 = 77 L

1 mol = 22.4 L

mol = 77/22.4 = 3.4375 mol of cO2

so

ratio is 1:1

3.4375 mol of CaCO3 required

MW of CaCO3 = 100 g

mass = mol*MW = 3.4375*100 = 343.75 g of CaCO3 required

B)

T = 23°C = 273+23 = 296 K

m = 3.8 g of butane

mol = mass/MW = 3.8/58.12 = 0.06538 mol of butane

ratio is

2 mol of butane --> 8 mol of CO2 + 10 mol of H2O

0.06538 mol of butane --> 4*0.06538 = 0.26152 mol of CO2

find V

PV = nRT

V = nRT/P

V = (0.26152)(0.082)(296)/(1) = 6.34761 L

V of CO2 = 6.34761 L

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