Hydrogen peroxide `(H_(2)O_(2))` decomposes according to the equation
`2H_(2)O_(2)hArr 2H_(2)O(l)+O_(2)(g)`
From the following data at `25^(@)C` calculate the value of `K_(p)` at 400 K for the above reaction,
`DeltaH^(@)=-196.0 kJ Deltas^(@)=125.65J//K`.
`["Given : "10^(-.15)=1.41]`

For the reaction 2H_(2)(g)+O_(2)(g)hArr 2H_(2)O(g)-K_(p)=K_(c)(RT)^(x) . Find the value of x.

Hydrogen peroxide is ionise as : H_(2)O_(2) hArr H^(+)+HO_(2)^(-) . If p^(h) of H_(2)O_(2) is 5.91 at 25^(@)C the ionic product of H_(2)O_(2) is

For the following reaction at 298 K, H_(2(g))+1/2 O_(2(g))to H_2 O_((l)) , Which of the following alternative is CORRECT?

For the following reaction at 298 K, H_(2(g))+1/2 O_(2(g))to H_2 O_((l)) , Which of the following alternative is CORRECT?

Diborane is a potential rocket fuel which undergoes combustion according to the reaction, B_(2)H_(6) (g) + 3O_(2) (g) rarr B_(2) O_(3) (s) + 3H_(2) O (g) From the following data, calculate the enthalpy change for the combustion of diborane: (i) 2 B (s) + ((3)/(2)) O_(2) (g) rarr B_(2) O_(3) (s) , Delta H = 0 1273 k J//mol (ii) H_(2) (g) + ((1)/(2)) O_(2) (g) rarr H_(2) O (l), Delta H = -286 kJ//mol (iii) H_(2) O (l) rarr H_(2)O (g) Delta H = 44 kJ//mol (iv) 2B (s) + 3H_(2) (G) rarr B_(2) H_(6) (g), Delta H = 36 kJ//mol

For the equilibrium reaction: 2H_(2)(g) +O_(2)(g) hArr 2H_(2)O(l) at 298 K DeltaG^(Theta) = - 474.78 kJ mol^(-1) . Calculate log K for it. (R = 8.314 J K^(-1)mol^(-1)) .