Question

What mass of C4H6 must react to produce 43.2 L of CO2 gas at 499 K and 2.57 atm. 

2C4H6(g)+11O2(g)⟶8CO2(g)+6H2O(l)

 

First, use the ideal gas equation to calculate the moles of CO2.

Then, calculate the mass of C4H6 from the moles of CO2. Show the conversions required to solve this problem.

Answer 1

V = 43.2L, T = 499K, P = 2.57atm

R = 0.0821 L*atm/moll*K

PV = nRT

n = PV/RT, n(CO₂) = (2.57*43.2) / (0.0821*499) = 111.024/40.9679 = 2.71 moll

m(C₄H₆) = (2Mr(C₄H₆)*V(CO₂)) / 8V_m(CO₂)

V(CO₂) = n(CO₂) * V_m(CO₂), V(CO₂) = 2.71*22.4 = 60,7 L

m(C₄H₆) = ((2*54)*60.7)/8*22.4 = 36.58 g