For the reaction `3H_2(g) + N_2(g) rarr 2NH_3(g)`. Compute and equate the reaction rates.

For the reaction : 2Cl(g)-.Cl_2(g) .

For the reaction, N_2(g)+3H_2(g)rarr2NH_3(g) , which is true:

Complete the reactions. PH_(3)(g) +O_(2)(g) rarr

For the reaction, N_(2) (g) + 3H_(2) (g) to 2NH_(3) (g) under certain conditions of temperature and partial pressure of the reactants, the rate of formation of NH_(3) is 0.001 kg h^(-1) . What will be the rate of conversion of H_(2) under the same condition?

triangleH for the reaction, H(g)+H(g)rarrH_2(g) will be,

For the reaction N_2+3H_2=2NH_3, triangleH=?

The partial pressure of CH_3OH(g) , CO(g) and H_2(g) in equilibrium mixture for the reaction, CO(g) + 2H_2(g) hArr CH_3OH(g) are 2.0,1.0 and 0.1 atm respectively at 427^Oc. The value of K_p for the decomposition of CH_3OH to CO and H_2 is :

In the reaction, N_2(g) +3H_2(g) hArr2NH_3(g) increase in H_2 concentration equilibrium:

For the reaction N_2 + 3H_2 hArr 2NH_3 in a vessel after the addition of equal number of mole of N_2 and H_2 equilibrium state is formed.Which of the following is correct ?