The combustion of a sample of butane, c4h10 (lighter fluid), produced 2.46 grams of water. 2 c4h10 + 13 o2 > 8 co2 + 10 h2o (a) how many moles of water formed? (b) how many moles of butane burned? (c) how many grams of butane burned? (d) how much oxygen was used up in moles? in grams?

The reactions shown here can be combined to make the overall reaction c(s) + h2o(g) ⇌ co(g) + h2(g) by reversing some and/or dividing all the coefficients by a number. a. c(s) + o2(g) → co2(g) k=1.363×10^69 b. 2 h2(g) + o2(g) → 2 h2o(g) k=1.389×10^80 c. 2co(g) + o2 (g) → 2 co2(g) k=1.477×10^90