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Consider the following balanced equation:
C7H16(g) + 11 O2(g) 7 CO2(g) + 8 H2O(l)
a) How many moles of carbon dioxide are produced if 5.0 mol heptane, C7H16, is burned?
b) If 3.01 x 10^23 molecules of heptane are consumed, how many molecules of water are produced?
C7H16(g) + 11 O2(g) 7 CO2(g) + 8 H2O(l)
a) How many moles of carbon dioxide are produced if 5.0 mol heptane, C7H16, is burned?
b) If 3.01 x 10^23 molecules of heptane are consumed, how many molecules of water are produced?