`1.7g` of `NH_3(g)` is present in a `2-L` flask. The active mass of `NH_3(g)` is

4g of hydrogen and 128 g of hydrogen iodide are present in a 2litre flask. What are their active masses?

2g of H_2 and 17g of NH_3 are placed in a 8.21 litre flask at 27^@C . The total pressure of the gas mixture is?

20.0 kg of N_2(g) and 3.0 kg of H_2(g) are mixed to produce NH_3(g) . The amount of NH_3 (g) formed is

Average molar kinetic energy of NH_3 (g) is

Some solid NH_(4)HS is placed in flask containing 0.5 atm of NH_(3) . What would be the pressure of NH_(3) and H_(2)S when equilibrium is reached. NH_(4)HS(g) hArr NH_(3)(g)+H_(2)S(g), K_(p)=0.11

1 mole N_2 and 3 moles of H_2 are taken in a 4 litre flask. If 0.25% of N_2 is converted to NH_3 at equilibrium and the reaction is N_2(g)+3H_2(g)iff2NH_3(g) . Then calculate the value of K_c under that condition. Prove that for the reaction aA_2(g)+bB_2(g)iffcAB(g) the value of the ratio K_p/K_c is 1 when a+b=c.

50.0 kg of N_2 (g) and 10.0 kg of Hydrogen (g) are mixed to produce NH_3 (g). Calculate the amount of NH_3 (g) formed. Identify the limiting reagent in the production Of NH_3 in this situation. —