Answer :
The following is a balanced reaction equation: 2CH4 + O2 > 2CH3OH
Let us first compute the delta H reaction using the conventional enthalpy of formation numbers.
Delta H rxn = sum of delta Hf product and delta Hf reactant
- [CH3OH *2] = [CH4*2]
= [-201.2 kJ/mol x 2] + [-74.87 kJ/mol * 2]
= -252.66 kJ
As a result, 2 mol CH4 produces -252.66 kJ of heat.
Let us now calculate the 38.8 g CH4
2.42 mol CH4 = 38.8 g CH4 * 1 mol / 16.04 g
-252.66 kJ = 2 mol CH4
2.42 mol = ? kJ
-306 kJ = 2.42kJ * (-252.66 kj) / 2 mol
As a result, the 38.8 g CH4 will produce 306 kJ (-306kJ) of heat.
Because of the exothermic reaction, a negative sign is assigned.
To learn more about an exothermic reaction click here
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