`2NOBr(g)hArr2NO(g)+Br2(g).` If nitrosyl bromide (NOBr) `40%` dissociated at certain temp. and a total pressure of `0.30` atm `K_(p)` for the reaction `2NO(g)+Br_(2)(g)hArr2NOBr(g)` is

The following data were obtained for the reaction: 2NO(g)+Br_2(g) rarr 2NOBr(g) Determine rate constant.

The following data were obtained for the reaction: 2NO(g)+Br_2(g) rarr 2NOBr(g) Determine the rate law?

For, 2NOBr(g)iff 2NO(g)+Br_2(g) , at equilibrium P_(Br_2)=P/9 and p is the total pressure, the ratio K_p/P will be

k_(P) & k_(C) are ….. for reaction at equilibrium of type H_(2)(g) + Br_(2)(g) hArr 2HBr(g) .

NO and Br_(2) at initial pressures of 98.4 and 41.3 torr respectively were allowed react at 300 K . At equilibrium the total pressure was 110.5 torr. Calculate the value of equilibrium constant, K_(p) and the standard free energy change at 300 K for the reaction: 2NO(g)+Br_(2)(g) hArr 2NOBr(g)

NO and Br_(2) at initial pressures of 98.4 and 41.3 torr respectively were allowed react at 300 K . At equilibrium the total pressure was 110.5 torr. Calculate the value of equilibrium constant, K_(p) and the standard free energy change at 300 K for the reaction: 2NO(g)+Br_(2)(g) hArr 2NOBr(g)

At 1000K , the pressure of iodine gas is found to be 0.1 atm due to partial dissociation of I_(2)(g) into I(g) . Had there been no dissociation, the pressure would have been 0.07 atm . Calculate the value of K_(p) for the reaction: I_(2)(g)hArr2I(g) .

At 1000K, the pressure of iodine gas is found to be 0.112 atm due to partial dissociation of I_(2)(g) into I(g). Had there been no dissociation, the pressure would have been 0.074 atm. Calculate the value of K_(p) for the reaction: I_(2)(g) hArr 2I(g) .