A reaction mixture for the production of `NH_3` gas contain 250g of `N_2` gas and 50 g of `H_2` gas under suitable conditions. Identify the limiting reactant, if any and calculate the mass of `NH_3` gas produced.

The density of gas was found to be 2.92 g L^(-1) at 27° C and 2.0 atm . Calculate the molar mass of the gas.

10 dm^3 of N_2 gas and 10 dm^3 of gas x at the same temperature contain the same number of molecules. The gas x is CO , CO_2 , H_2 , NO

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. —

Dinitrogen and dihydrogen react as N_2(g)+3H_2(g) to 2NH_3(g) If yes, calculate the mass of the reactant.

7g of N_2 is allowed to react with 2g H_2 in presence of catalyst to form NH_3 Which is the limiting reagent?

The combination of elements form compounds is governed by the laws of chemical combination 28 g of N_2 is mixed with 12g of H_2 to form ammonia as per the reaction, N_2+3H_2rarr2NH_3. Which is the limiting reagent in this reaction?

The kinetic energy for 14g of N_(2) gas at 127^(@)C is nearly

Assertion : For the reaction 2 NH _(3 (g)) to N _(2 (g)) + 3 H _(2 (g)), Delta H gt Delta U Reason : Enthalpy change is always greater than internal energy change