Calculate the equilibrium constant for the reaction at 298K 4 Br + O2 + 4H+ → 2 Br2 + 2H2O Given that Ecell = 0.16V​

Calculate the equilibrium constant, K_(C) for the reaction 3Sn^(4+)+2Cr to 3Sn^(2+)+2Ce^(3+) , at 298K given E_(cell)^(@)=0.83V

Using the standerd half-cell potential listed, calculate the equilibrium constant for the reaction : Co(s)+2H^(+)(aq)toCo^(2+)(aq)+H_(2)(g)" at 298 K" Co^(2+)(aq)+2e^(-)toCo(s) E^(@)=-0.277 V

Calculate the enthalpy change in the reaction, 4NH_(3) + 3O_(2) to 2N_(2) + 6H_(2) O at 298 K,given that the enthalpy of formation at 298 K for NH_(3) and H_(2)O are - 46.0 and - 286.0 KJ mol^(-1) respectively.

Calculate the oxidation number of O in H2O

Calculate the oxidation number of O in H2O

Calculate the formula mass of CuSO4.5H2O

Write the reaction of XeF_4 with H_2O .

Write the equilibrium constant expression for the following reactions. CH_(4)(g) + 2O_(2)(g) hArr CO_(2)(g) + 2H_(2)O(l)

For the reaction 2NO_(2)(g)+(1)/(2)O_(2)(g)hArrN_(2)O_(5)(g) if the equilibrium constant is K_(p) , then the equilibrium constant for the reaction 2N_(2)O_(5)(g)hArr4NO_(2)(g)+O_(2)(g) would be :

Assertion : The molecularity of the reaction H_2 + Br_2 rarr 2HBr is 2. Reason : Order of the reaction 3/2.