`4NH_3(g)+50_2(g) rarr4NO(g)+6H_2O(g)` express instant reaction rate in terms of change of concentration of reactants and products.

For the reaction 4NH_(3)(g)+5O_(2)(g)rarr4NO(g)+6H_(2)O(g) write the instantaneous reaction -rate in terms of decrease in concentration of the reactants and increase in the concentration of the products.

For the reaction A+2Brarr3C , express the rate in terms of change in concentration of reactants and product.

Consider the following reaction for 2NO_(2)(g)+F_(2)(g)rarr2NO_(2)F(g) The expression for the rate of reaction in terms of the rate of change of partial pressure of partial pressure of reactant and product is/ are —

For the reaction, N_(2)(g)+3H_(2)(g)rarr2NH_(3)(g) express the rate of the reaction with respect to the reactants and the product formed.

At a constant temperature, the equilibrium constant of the reaction N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) is K and that of the reaction (1)/(2)N_(2)(g)+(3)/(2)H_(2)(g)hArrNH_(3)(g) is sqrt(K) . Explain this difference of K values in spite of the fact that the reactants and products in both the reactions are same.

For the reaction , 4NH_(3)(g)+5O_(2)(g)rarr4NO(g)+6H_(2)O(g) the concentration of NO increases to 0.18"mol.L"^(-1) in 5s. Calculate rate of formation of water

N_2(g) + 3H_2(g) → 2 NH_3(g) . For the above reaction the correct statement is

Express the rate of following reaction in terms of different reactants and products of 4NH_3(g)+5O_2(g)rarr4NO(g)+6H_2O(g) If the rate of formation of NO is 3.6xx10^-3 mole/lit sec^-1 Calculate: The rate of disappearance of NH_3