At `25^(@)C` and 1 atm, the standard reaction enthalpy for the reaction C(graphite, s)`+O_(2)(g)toCO_(2)(g)` is the _____ of `CO_(2)(g)`.

At 25^(@)C and 1 atm, standard reaction enthalpy for the reaction, CH_(4)(g) +2O_(2)(g)toCO_(2)(g)+2H_(2)O(l) is _____ of CH_(4)(g) .

For the reactions : C(s) + O_(2) (g) to CO_(2) (g)

At 25^(@)C , the standard reaction enthalpy for the reaction, 2C(graphite, s) +O_(2)(g)to2CO(g) is -221.0kJ. Does this enthalpy change indicate the standard enthalpy of formation of CO(g) ? If not, then what would be the value of the enthalpy of formation of CO(g) at 25^(@)C ?

(a) At 25^(@)C , standard reaction enthalpy for the reaction 2 C(graphite, s) +O_(2)(g)to 2CO(g) is -221.0 kJ. Does this value indicate the standard enthalpy of formation of CO(g) ? If not, then what would be the value of enthalpy of formation of CO(g) at 25^(@)C ? (b) A gas is allowed to expand against zero external pressure. Explain with reason whether the procss is reversible or not.

For the reaction : C(s) + O_(2)(g) rarr CO_(2)(g)

At 25^(@)C the standard reaction enthalpy for the reaction AB_(3)(g)to(1)/(2) A_(2)(g)+(3)/(2)B_(2)(g) is DeltaH^(0) . Find the standard reaction enthalpy for the reaction A_(2)(g)+3B_(2)(g) to 2AB_(3)(g) at 25^(@)C .

At 25^(@) C, is the standard reaction enthalpy for the reaction 2H(g) +O(g)toH_(2)O(l) the same as the standard enthalpy of formation of H_(2)O(l) ?

Why are the standard reaction enthalpies of the following two reactions different? (1) C(graphite, s) +O_(2)(g)toCO_(2)(g),DeltaH^(0)=-393.5kJ (2) C(diamond, s) +O_(2)(g)toCO_(2)(g),DeltaH^(0)=-395.4kJ

The standard entropy change Delta S_r^@ for CH_(4(g)) + 2O_(2(g)) to CO_(2(g)) + 2H_2O_((l)) is -242.98 JK^(-1) at 25^@C . Calculate the standard reaction enthalpy for the above reaction if standard Gibbs energy of formation of CH_(4(g)), CO_(2(g)) and H_2O_((l)) are -50.72, -394.36 and - 237.13 kJ mol^(-1) respectively.