`Delta_(f)H^(Theta)` of hypothetical `MgCI` is `-125 kJ mol^(-1)` and for `MgCI_(2)` is `-642 kJmol^(-1)`. The enthalpy of disporportionation of `MgCI is -49x`. Find the value of `x`.

Delta_(f)H^(Theta) of hypothetical MgCl is -125 kJ mol^(-1) and for MgCl_(2) is -642 kJmol^(-1) . The enthalpy of disporportionation of MgCl is -49x . Find the value of x .

Delta_(f)H^(ɵ) of hypothetical MX is -150 kJ mol^(-1) and for MX_(2) is -600 kJ mol^(-1) . The enthalpy of disproportionation of MX is =-100 x kJ mol^(-1) . Find the value of x.

Delta_(f)H^(ɵ) of hypothetical MX is -150 kJ mol^(-1) and for MX_(2) is -600 kJ mol^(-1) . The enthalpy of disproportionation of MX is =-100 x kJ mol^(-1) . Find the value of x.

The enthalpy of formation of hypothetical MgCI is -125kJ mol^(-1) and for MgCI_(2) is -642 kJ mol^(-1) . What is the enthalpy of the disproportionation of MgCI .

The enthalpy of formation of hypothetical MgCl is -125kJ mol^(-1) and for MgCl_(2) is -642 kJ mol^(-1) . What is the enthalpy of the disproportionation of MgCl .

The standard enthalpy of formation of hypothetical MgCl is -125kJ mol^(-1) and for MgCl_(2) is -642 kJ mol^(-1) . What is the enthalpy of the disproportionation of MgCl ?

The standard enthalpy of formation of hypothetical MgCl is -125kJ mol^(-1) and for MgCl_(2) is -642 kJ mol^(-1) . What is the enthalpy of the disproportionation of MgCl ?

The enthalpy of formation of hypothetical CaCl(s) is found to be - 180 kJ mol^(-1) and that of CaCI_(2) (s) is -800 kJ mol^(-1) . Calculate Delta_(f)H^(@) for the disproportionation reaction: 2CaCI(s) to CaCI_(2)(s) + Ca(s)

Given, the enthalpy of formation of MgCl_((s)) is -125 kJ mol^(-1) and the entahpy of formation of MgCl_(2(s)) is -642kJ mol^(-1) . Predict whether MgCl will undergo disproportionnation or not? If yes, calculate the enthalpy of disproportion.