10 moles of CH4 at R.T.P would produce what volume of CO2?
Options:
a) 2.4e5 dm3 b) 2.4e2 dm3 c)2.4e4 dm3 d) 2.4e6 dm3
Options:
a) 2.4e5 dm3 b) 2.4e2 dm3 c)2.4e4 dm3 d) 2.4e6 dm3
1 Answer
Explanation:
This problem involves the combustion of methane. In a combustion reaction, oxygen is added to a hydrocarbon to produce carbon dioxide and water.
Here's the unbalanced equation:
#CH_4 + O_2 -> CO_2 + H_2O#
And here's the balanced equation:
#CH_4 + 2O_2 -> CO_2 + 2H_2O#
Since
To find the volume of
#P# is the pressure in#"atm"# #V# is the volume in#"L"# #n# is the number of moles#R# is the universal gas constant,#("0.0821 atm" * "L") / ("mol" * "K")# #T# is the temperature in#"K"#
At RTP, room temperature and pressure, the pressure is
Substitute all of the known values into the equation.
#PV = nRT#
#"1 atm" * V = "10 mol" * ("0.0821 atm" * "L") / ("mol" * "K") * "298 K"#
#V = ("10" cancel "mol" * ("0.0821" cancel "atm" * "L") / (cancel "mol" * cancel "K") * "298" cancel "K")/ ("1" cancel "atm")#
#V = "240 L"#
A total volume of
Thus, the answer is