Question #17a18

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Answer 1 · 2018-01-29T02:04:14

The mass of #CO_2# produced will be 62.7 g

First, we use the ideal gas law to determine the number of moles of methane:

#PV=nRT#

which we will write as

#n=(PV)/(RT) = (749 xx 35.0)/(62.36 xx295) = 1.425 "mol"#

Now, the balanced equation for the reaction:

#CH_4 + 2 O_2 rarr CO_2 + 2H_2O#

Since the ration of #CH_4# to #CO_2# is one-to-one, there will be 1.425 mol of #CO_2# produced, with a mass of

#1.425 "mol" xx 44g/"mol"=62.7 g#