The entropy `(S^(o))` of the following substances are:
`CH_(4)(g)` `186.2JK^(-1)mol^(-1)`
`O_(2)(g)` `205.0JK^(-1)mol^(-1)`
`CO_(2)(g)` `213.6JK^(-1)mol^(-1)`
`H_(2)O(l)` `69.9JK^(-1)mol^(-1)`
The entropy change `(DeltaS^(o))` for the reaction `CH_(4)(g)+2O_(2)(g)rarr CO_(2)(g)+2H_(2)O(l)` is `(J/(K.mol))`

The internal energy change (DeltaU) for the reaction CH_(4)(g) + 2O_(2)(g) to CO_(2)(g) + 2H_(2)O(l) is -885 kJ mol^(-1) at 298K. What is DeltaH at 398 K?

Delta H_(1)^(@) for CO_(2)(g) , CO(g) and H_(2)O(g) are -393.5,-110.5 and -241.8 kJ mol^(-1) respectively. Standard enthalpy change for the reaction CO_(2)(g)+H_(2)(g) rarr CO(g) + H_(2)O(g) is

Standard heat of formation of CH_(4)(g), CO_(2)(g) and H_(2)O(l) are -75, -393.5, -286 kJ respectively. Find out the change in enthalpy for the reaction. CH_(4)(g)+2O_(2)(g)rarr CO_(2)(g)+2H_(2)O(l)

The DeltaH_(f)^(@) for CO_(2)(g) , CO(g) and H_(2)O(g) are -395.5,-110.5 and -241.8" kJ" mol^(-1) respectively. The standard enthalpy change in (in kJ) for the reaction CO_(2)(g)+H_(2)(g)toCO(g)+H_(2)O(g) is

Given the following entropy values ( in JK^(-1) "mol"^(-1) ) at 298 K and 1 atm: H_(2)(g):130.6, Cl_(2)(g):223.0, HCl(g): 186.7 . The entropy change (in JK^(-1) "mol"^(-1) ) for the reaction H_(2)(g) + Cl_(2)(g) to 2HCl(g) , is (a) +540.3 (b) +727.0 (c) -166.9 (d) +19.8

Calculate the change in entropy for the following reaction 2CO(g) +O_(2)(g) rarr 2CO_(2)(g) Given: S_(CO)^(Theta)(g)=197.6 J K^(-1)mol^(-1) S_(O_(2))^(Theta)(g)=205.03 J K^(-1)mol^(-1) S_(CO_(2))^(Theta)(g)=213.6 J K^(-1)mol^(-1)

Calculate enthalpy of formation of methane (CH_4) from the following data : (i) C(s) + O_(2)(g) to CO_(2) (g) , Delta_rH^(@) = -393.5 KJ mol^(-1) (ii) H_2(g) + 1/2 O_(2)(g) to H_(2)O(l) , Deta_r H^(@) = -285.5 kJ mol^(-1) (iii) CH_(4)(g) + 2O_(2)(g) to CO_(2)(g) + 2H_(2)O(l), Delta_(r)H^(@) = -890.3 kJ mol^(-1) .

Calculate the standard free energy change for the following reaction at 27^@C . H_2(g) + I_2(g) to 2HI(g) , DeltaH^@ = + 51.9 kJ [Given : DeltaS_(H_2)^@ = 130.6 JK^(-1) mol^(-1) DeltaS_(I_2)^@ = 116.7 JK^(-1) mol^(-1) DeltaS_(HI)^@ = 206.3 JK^(-1) mol^(-1)] . Predict whether the reaction is feasible at 27°C or not.

Calculated the equilibrium constant for the following reaction at 298K : 2H_(2)O(l) rarr 2H_(2)(g) +O_(2)(g) Delta_(f)G^(Theta) (H_(2)O) =- 237.2 kJ mol^(-1),R = 8.314 J mol^(-1) K^(-1)

Calculate DeltaG^(Theta) for the following reaction: CO(g) +((1)/(2))O_(2)(g) rarr CO_(2)(g), DeltaH^(Theta) =- 282.84 kJ Given, S_(CO_(2))^(Theta)=213.8 J K^(-1) mol^(-1), S_(CO(g))^(Theta)= 197.9 J K^(-1) mol^(-1), S_(O_(2))^(Theta)=205.0 J K^(-1)mol^(-1) ,