Home
Class 11
CHEMISTRY
Combustion of hydrogen in a fuel cell at...

Combustion of hydrogen in a fuel cell at 300 K is represented as `2H_(2(g))+O_(2(g)) rarr 2H_(2)O_((g))`. If `Delta H` and `Delta G` are `-241.60 kJ mol^(-1)` and `-228.40 kJ mol^(-1)` of `H_(2)O`. The value of `DeltaS` for the above process is

A

`4.4kJ`

B

`-88j`

C

`+88J`

D

`-44J`

Text Solution

Verified by Experts

The correct Answer is:
B
`DeltaS=DeltaH-TDeltaS`
Promotional Banner

Similar Questions

Explore conceptually related problems

For hydrogen oxygen fuel cell with reaction 2H_(2)(g)+O_(2)(g) rarr 2 H_(2)O(l) DeltaG_(f)^(c-)(H_(2)O)=-237.2kJ mol^(-1) . Hence, EMF of the fuel cell is

The enthalpy change for the formation of 3.6 kg water is _____ . H_(2(g))+1/2 O_(2(g)) to H_2 O_((l)), Delta H=-284.5 kJ mol^-1

Compute the value of DeltaS at 298K for the reaction, H_(2)(g)+1//2O_(2)(g)toH_(2)O(g) given that, DeltaG=-228.6kJ and DeltaH=-241.8kJ

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)

H_(2)(g) +(1)/(2)O_(2)(g) rarr H_(2)O(g) DeltaH =- 242 kJ mol^(-1) Bond energy of H_(2) and O_(2) is 436 and 500 kJ mol^(-1) , respectively. What is bond energy of O-H bond?

For the reaction : C_(2)H_(5)OH(l)+3O_(2)(g)rarr2CO_(2)(g)+3H_(2)O(g) if Delta U^(@)= -1373 kJ mol^(-1) at 298 K . Calculate Delta H^(@)

The enthalpy of combustion of H_(2(g)) to give H_(2)O_((g)) is -249 kJ mol^(-1) and bond enthalpies of H-H and O=O are 433 mol^(-1) and 492 kJ mol^(-1) respectively. The bond enthalpy of O-H is

The enthalpy of vapourisation of liquid water using the data : H_(2)(g)+1//2O_(2)(g)rarr H_(2)O(l) , Delta =-285.77 KJ mol^(-1) H_(2)(g)+1//2O_(2)(g)rarr H_(2)O(g) , Delta H=-241.84 KJ mol^(-1)