2C4H10(g)+13O2(g)→10H2O(g)+8CO2(g) Calculate the mass of water produced when 4.16 g of butane reacts with excess oxygen.
Ans-- given balence reaction is
2C4H10(g)+13O2(g)→10H2O(g)+8CO2(g)
we can use dimensional analysis, and equation coefficients, to change 4.16 g of butane to moles of butane, to moles of water, to grams of water. We shall need the following equalities to set up conversion factors.
1 mol C4H10 = 56.108 g C4H10
2 mol C4H10 = 10 mol H2O
1 mol H2O = 18.015 g H2O
[(4.16 g C4H10)/1][(1 mol C4H10)/(56.108 g C4H10)][(10 mol H2O)/(2
mol C4H10)][(18.015 g H2O)/(1 mol H2O)] = 6.38248 g of H2O or 6.39
g H2O rounded to three significant figures
Answer: The mass of water produced when 4.16 of butane reacts with
excess oxygen is 6.39 g.
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