a) When heated, calcium carbonate decomposes to yield calcium oxide and carbon d

Question

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 55.0 L of carbon dioxide at STP?

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 2.00 g of butane?

Explanation / Answer

a)

at SSTP = 22.4 L is 1 mol

then

55/22.4 = 2.4553 mol of CO2 present

then, since ratio is 1:1: there is 2.4553 mol of CaCO3

mass of CaCO3 = 2.4553*100 = 245.3 g of CaCO3

B)

2 g of butane

mol = mass/MW = 2/58 = 0.03448 mol o fbutane

then expect

2:8 = 4*0.03448 = 0.13792 mol of CO2

apply ideal gas law

PV = nRT

V = nRT/P

V = 0.13792*0.082*(23+273)/(1) = 3.3475 L of CO2

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