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

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?atm/(K?mol) or 8.3145 J/(K?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.

Part A

When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction

CaCO3(s)?CaO(s)+CO2(g)

What is the mass of calcium carbonate needed to produce 29.0L of carbon dioxide at STP?

Part B

Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is

2C4H10(g)+13O2(g)?8CO2(g)+10H2O(l)

At 1.00 atm and 23 ?C, what is the volume of carbon dioxide formed by the combustion of 2.00g of butane?

-Stoichiometric relationships w/ gases-

Explanation / Answer

Part A
at STP 1 mole occupies 22.4 L
S 29 L is 1.3 mole
1 mole of CaCO3 generates 1 mole CO2
so we need 1.3 mole of CaCO3(molecular weight 100 grams) = 130 grams

Part B

108 grams of butane gives 352 grams of CO2

2 grams give 6.5 grams f CO2 =0.15 mole
As PV=nRT bu substituting the values you get V= 3.6L

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