Consider the combustion (burning) of methane, CH4, in oxygen. CH4(g) + 2O2(g) CO2(g) + 2H2O(l) The heat
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CH4(g) + 2O2(g) →CO2(g) + 2H2O(l)
The heat of reaction at 25oC and 1.00 atm is 890.2 kJ. What is the change in volume when 1.00 mol CH4 reacts with 2.00 mol O2? (You can ignore the volume of liquid water, which is insignificant compared with volumes of gases.) What is w for this change? Calculate ∆U for the change indicated by the chemical equation.
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At 100 atm and 25C the volume occupied by 100 mol of any of the gases in the equation is 2241 L x ...View the full answer
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