If rate of production of ammonia from its elements in Haber's process is \(6\times10^{-3}molL^{-1}s^{-1}\) ,the rate of consumption of hydrogen gas will be: "

The rate constant of a reaction is \(2.6\times10^{-2}MolL ^{-1}s^{-1}\) .What is the order of the reaction?

The rate of diffusion of a gas having molecular weight. just double of hydrogengas is 30 mls-1. The rate of diffusion of hydrogen gas will be

The stoichiometric equation for the oxidation of bromide ions by hydrogen peroxide in acid solution is 2Br^(-) + H_2O_2 + 2H^(+) to Br_2+ 2H_2O Since the reaction does not occur in one stage, the rate equation does not correspond to this stoichiometric equation but is rate = k[H_2O_2][H^+][Br^-] If, under certain conditions, the rate of consumption of Br^– ions is 7.2 xx 10^(–3) "mole" "dm"^(–3) s^(–1) , what is the rate of consumption of hydrogen peroxide ? What is the rate of production of bromine

In a catalytic conversion of N_(2) to NH_(3) by Haber's process, the rate of reaction was expressed as change in the concentration of ammonia per time is 40 xx 10^(-3) mol L^(-1) s^(-1) . If there are no side reaction, the rate of the reaction as expressed in terms of hydrogen is (in mol L^(-1) s^(-1) )

For the reaction N_(2)(g)+3H_(2)(g)rarr2NH_(3)(g) , uneder certain conditions of temperature and pressure of the reactants, the rate of formation, of ammonia is 0.001 kg hr ^(-1) . The rate of consumption of hydrogen under the same conditions is ...... kg hr^(-1)