Calculate the standard enthalpy change for the reaction
`CH_4 (g) + 2O_2(g) to CO_2(g) + 2H_2O(l)`,
given that the standard heatds of formation of `CH_4(g, CO_2(g) and H_2O (l) ` are` -74.91 mol^(-1), -394.12 kJ mol^(-1) and -286.31 kJ mol^(-1)` respectivley.

Use the standard enthalpies of formation and calculation the enthalpy changes accompanying the following reaction: a. CH_(4)(g)+2O_(2)(g) rarr CO_(2)(g)+2H_(2)O(l) Given, enthalpies of formation of CH_(4) ,CO_(2) and H_(2)O are 74.8 kJmol^(-1) ,−393.5 kJmol^(−1) ,−286 kJmol^(−1) respectively.

Calculate the standard free energy change for the reaction 4NH_3(g) + 5O_2(g) to 4NO(g) + 6H_2O(l) Given that the standard free energy of formation (Delta_f G^@)" for " NH_3(g) NO(g) and H_2O (l) are -16.8, + 86.7 and -237.2 kJ mol^(-1) respectively. Predict the feasibility of the above reaction at the standard state.

Calculate the standard enegry change for the reaction: OF_(2)(g) +H_(2)O(g) rarr O_(2)(g) +2HF(g) at 298K The standard enthalpies of formation of OF_(2)(g), H_(2)O(g) , and HF(g) are +20, -250 , and -270 kJ mol^(-1) , respectively.

Calculate Delta_(r ) H^(Θ) for the reaction : C_(6)H_(6)(l)+7.5O_(2)(g)rarr 6CO_(2)(g)+3H_(2)O(l) Given the standard heat of formations (Delta_(f)H^(Θ)) of H_(2)O(l), CO_(2)(g) and C_(6)H_(6)(l) are -57.80 kcal/mol, -94.05 kcal/mol and 19.8 kcal/mol respectively.

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

Find the value of Delta_(f) H^(@) for the reaction N_(2) O_(4) (g) + 3 CO(g) rarr N_(2) O (g) + 3 CO_(2) (g) Standard enthalpies of formation of CO(g), CO_(2) (g), N_(2) O (g) , and N_(2) O_(4) (g) are - 110, - 393, 81 , and 9.7 kJ mol^(-1) , respectively. Strategy : The standard enthalpy change of a reaction is equal to the sum of the standard molar enthalpie of formation of the products each multiplied by its stiochiometric coefficient in the balanced equation, minus the corresponding sum of the standard molar enthalpies of formation of the reactants

CH_4(g) + 2O_2(g) to CO_2(g) + 2H_2O(g), Delta H = -809 kJ The calorific value of 1 kg of CH_4(g) is ………… kJ/kg.

Calculate the standard internal energy change for the following reactions at 25^(@)C : 2H_(2)O_(2)(l) rarr 2H_(2)O(l) +O_(2)(g) Delta_(f)H^(Theta) at 25^(@)C for H_(2)O_(2)(l) =- 188 kJ mol^(-1) H_(2)O(l) =- 286 kJ mol^(-1)

The standard enthalpies of formation of CO_(2)(g) and HCOOH (l) are -393.7 kJ"mol"^(-1) and -409.2 kJ"mol"^(-1) respectively. Which of the following statements are correct?

Calculate the standard enthalpy change (in kJ "mol"^(-1) ) for the reaction H_(2)(g)+O_(2)(g)toH_(2)O_(2)(g) , given that bond enthalpy of H-H, O=O,O-H and O-O (in kJ "mol"^(-1) ) are respectively 438, 498, 464 and 138.