The ideal gas law PV = nRT relates pressure P, volume V, temperature T, and numb
ID: 513957 • Letter: T
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 08206 L middot atm/(K middot mol) or 8.3145 J/(K middot mol). The equation can be rearranged as follows to solve for pi: 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. mass of CaCo_3 = 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. Volume of CO_2 =Explanation / Answer
A)
At STP, volume of any 1 mol of gas = 22.4 L
MOL of CO2 = 77.0 / 22.4 mol = 3.44 mol
from reaction,
mol of CaCO3 required = mol of CO2 formed = 3.44 mol
molar mass of CaCO3 = 100.1 g/mol
mass of CaCO3 = number of mol * molar mass
= 3.44 mol * 100.1 g/mol
= 344 g
Answer: 344 g
B)
molar mass iof C4H10 = 4*12 + 10*1 = 58 g/mol
number of mol of butane = mass / molar mass
= 3.80 / 58 mol
= 0.0655 mol
from reaction ,
mol of CO2 formed = (8/2)*mol of butane burnt
= (8/2)*0.0655 mol
= 0.262 mol
P = 1.00 atm
n = 0.262 mol
T= 23 oC = (23+273) K = 296 K
use:
P * V = n*R*T
1.00 atm * Vi = 0.262 mol* 0.0821 atm.L/mol.K * 296 K
V = 6.37 L
Answer: 6.37 L
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