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 as : CH_(4)(g) + 2O_(2)(g) to CO_(2)(g) + 2H_(2)O(l) Delta_(r)H^(@) = 890.3 kJ Calculate : (a) how many grams of methane would be required to produce 445.15 kJ of heat on combustion? How many grams of CO_(2) would be formed when 445.15 kJ heat is evolved? (c) what volume of O_(2) at S.T.P would be used in the above combustion process ?

Calculate the calorific value of methane if it burns according to the equation CH_4(g) + 2O_2(g) to CO_2(g) + 2H_2O(l) , DeltaH = -890.0 kJ

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)

Consider the following reactions, CH_(4)(g) + 2O_(2)(g) to CO_(2)(g) + 2H_(2)O(g) How many moles of methane are required to produce 22g of CO_(2) (g) after combustion?

Consider the following reactions, CH_(4)(g) + 2O_(2)(g) to CO_(2)(g) + 2H_(2)O(g) How many moles of methane are required to produce 22g of CO_(2) (g) after combustion?

CH_(4)(g) +2O_(2)(g) rarr CO_(2)(g) +2H_(2)O(l), DeltaH =- 890 kJ what is the calorific or fuel value of 1kg of CH_(4) ?

CH_(4)(g) +2O_(2)(g) rarr CO_(2)(g) +2H_(2)O(l), DeltaH =- 890 kJ what is the calorific or fuel value of 1kg of CH_(4) ?