The combustion of methane is written as
`CH_(4)(g)+2O_(2)(g)toCO_(2)(g)+2H_(2)O(l)`
The difference between enthalpy change and energy change is equal to:

For the reaction C_(2)H_(4(g))+3O_(2(g)) rarr 2CO_(2(g))+2H_(2)O_((l)) the difference between enthalpy change and internal energy change is

Estimate the enthalpy of combustion of methane in KJ .mol^(-1) CH_(4)(g)+2O_(2)(g)to CO_(2)(g)+2H_(2)O(g)

Balance the following equations : CH_(4(g))+O_(2(g))toCO_(2(g))+H_(2)O_((g))

For the given reaction, CH_(4)(g)+2O_(2)(g)toCO_(2)(g)+2H_(2)O(l) Select the correct option for Delta_(r)H .

The heat evolved in the combustion of methane is given by the following equation : CH_(4)(g)+2O_(2)(g)to CO_(2)(g)+2H_(2)O(l) , Delta H = -890.3 kJ How many grams of methane would be required to produce 445.15 kJ of heat of combustion ?

The heat evolved in the combustion of methane is given by the following equation : CH_(4)(g)+2O_(2)(g)to CO_(2)(g)+2H_(2)O(l) , Delta H = -890.3 kJ How many grams of methane would be required to produce 445.15 kJ of heat of combustion ?

A balanced equation for combustion of methane is given below: CH_(4(g)) + CO_(2(g)) to CO_(2(g)) + 2H_2O_(g) Which of the following statements is not correct on the basis of the above chemical equation?

In a fuel cell methanol is oxidised with oxygen as : CH_(3)OH(l) + 3/2O_(2)(g) to CO_(2)(g) + 2H_(2)O(l) Calculate the standard Gibbs energy change for the reaction that can be converted into electrical works. If standard enthalpy of combustion for methanol is 726 kJ mol^(-1) , calculate the efficiency of conversion of Gibbs energy into useful work. The standard Gibbs energies of formation, Delta_(f)G^(@)(kJ mol^(-1)) are : CO_(2)(g) = -394.4, H_(2)O(l) = -237.2, CH_(3)OH(l) = -166.2 .

In the reaction C_(3)H_(6)(g)+nO_(2)(g)toCO_(2)(g)+H_(2)O(l) . The ratio of the coefficients of CO_(2) and H_(2)O is