a) Write a balanced equation for the combustion of butane gas. b) If at a given

Question

a) Write a balanced equation for the combustion of butane gas. b) If at a given moment butane is reacting at a rate of 0.400 mol L?1s?1, what are the rates of formation of products? c) What is the rate at which oxygen is reacting? I found the balanced equation, (2C4H10 + 13O2 --> 8CO2 + 10H2O) but I don't know how to get b and c from that

Explanation / Answer

b)2C4H10+ 13O2 ------- > 8CO2 + 10H20 if formation rate of butane is .400, then formation of co2 is 4 times that value = 1.600 formation of h20 is 5 times that value = 2.00 2) oxygen is reacting 13/2 times butane =0.4*13/2 = 2.600

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