In the reaction `X^(-)+XO_(3)^(-)+H^(+)rarrX_(2)+H_(2)O` , the molar ratio in which `X^(-)` and `XO_(3)^(-)` react is :

In the balanced equation I_(2)+xO_(3)rarr I_(4)O_(9)+O_(2) the ' x ' is

(A): OX^(-) on heating in the presence of OH^(-) gives X^(-) and XO_(3)^(-) (R): Conversion of OX^(-) to X^(-) and XO_(3)^(-) , is called disproportionation.

At the temperature T(K) for the reaction X_(2)O_(4) (l) rarr 2XO_(2)(g) Delta U = x kJ mol^(-1), Delta S = y JK^(-1) mol^(-1) . Gibbs energy change for the reaction is (Assume X_(2)O_(4), XO_(2) are ideal gases) Delta U = x kJ mol^(-1), Delta S = y JK^(-1) mol^(-1)

For the reaction at 25^(@)C, C_(2)O_(4)(l) rarr 2XO_(2)(g) Delta H =2.1 kcal and DeltaS=20 cal K^(-1) . The reaction would be :

For the reaction at 25^(@)C, C_(2)O_(4)(l) rarr 2XO_(2)(g) Delta H =2.1 kcal and DeltaS=20 cal K^(-1) . The reaction would be :

H_(3)BO_(3)overset("Red heat")rarrX .X in the reaction is

When pentane , C_(5) H_(12) is burned in excess oxygen , the products of the reaction are CO_(2)(g) and H_(2)O (l) . The balanced equation for this combustion is C_(5) H_(12)(g) + xO_(2)(g) rarr 5CO_(2)(g) + 6 H_(2) O (l) The coefficient (x) of oxygen should be

When pentane , C_(5) H_(12) is burned in excess oxygen , the products of the reaction are CO_(2)(g) and H_(2)O (l) . The balanced equation for this combustion is C_(5) H_(12)(g) + xO_(2)(g) rarr 5CO_(2)(g) + 6 H_(2) O (l) The coefficient (x) of oxygen should be