Part A Determine the mass of CO2 produced by burning enough of methane to produc

Question

Part A Determine the mass of CO2 produced by burning enough of methane to produce 1.50 × 102 kJ of heat. CH4(g) + 202(g) CO2(g) + 2H20(g) Ho -802.3 kJ Express your answer using three significant figures Submit My Answers Give Up Incorrect; Try Again; 2 attempts remaining Part B Determine the mass of CO2 produced by burning enough of propane to produce 1.50 × 102 kJ of heat. C3H8(g) + 5O2(g) 3 CO2 (g) + 4H20(g) Hrx,--2217 kJ Express your answer using three significant figures mco Submit My Answers Give U Incorrect; Try Again; 2 attempts remaining Part C Determine the mass of CO2 produced by burning enough of octane to produce 1.50 × 102 kJ of heat. C8H18(1) + 25/2 O2(g) 8 CO2(g) + 9H20(g) Hrxn=-5074.1 kJ Express your answer using three significant figures Submit My Answers Give Up Incorrect Try Again; 3 attempts remaining

Explanation / Answer

a)

Q = 1.5*10^2 = 150 kJ required

n = Q/HRxn= 150/802.3 = 0.18696 mol of CH4 required

mol of CO2 = 0.18696

mass = mol*MW = 0.18696*44 = 8.22624 g of CO2

B)

similarly

n = Q/HRxn = 150/2217

n = 0.06765 mol of propane

mol of CO2= 3xproane = 3*0.06765

mol of CO2 = 0.20295

mass = mol*MW = 0.20295*44

mass of CO2 =8.9298 g

c)

n = Q/HRxn = 150/5047.1

n = 0.02972 mol of octane

mol of CO2 = 8*0.02972

mol of CO2 = 0.23776

mass = mol*MW = 0.23776*44 = 10.46144 g of CO2

D)

the best fuel is CH4, methane, since it produces less CO2 per kJ

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