Under S.T.P. 1 mol of `N_(2)` and 3 mol of `H_(2)` will form on complete reaction

At S.T.P. 0.50 mol of H_(2) gas and 1.-0 mol of He gas

At 1400 K, K_( c) = 2.5 xx 10^(-3) for the reaction CH_(4)(g)+2H_(2)S(g)hArrCS_(2)(g)+4H_(2)(g) A 10 L reaction vessel at 1400 K contains 2.0 mol of CH_(4) , 4.0 mol of H_(2)S , 3.0 mol of CS_(2) , 3.0 mol of H_(2) . In which direction does the reaction proceed to reach equilibrium?

A mixture of 1.57 mol of N_(2) , 1.92 mol of H_(2) and 8.13 mol of NH_(3) is introduced into a 20L reaction vessel at 500K . At this temperature, the equilibrium constant, K_(c) for the reaction N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) is 1.7xx10^(2) . Is the reaction mixture at equilibrium ? If not, what is the direction of the net reaction ?

1 mol of N_2 and 4 mol of H_2 are allowed to react in a vessel and after reaction, H_2O is added. Aqueous solution required 1 mol of HCI for neutralization. Mol fraction of H_2 in the mixture after reaction is :

1 mol of N_2 and 4 mol of H_2 are allowed to react in a vessel and after reaction, H_2O is added. Aqueous solution required 1 mol of HCI for neutralization. Mol fraction of H_2 in the mixture after reaction is :

A mixture of 1.57 mol of N_(2), 1.92 mol of H_(2) and 8.13 mol of NH_(3) is introduced into a 20 L reaction vessel at 500 K . At this temperature, the equilibrium constant K_(c ) for the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) is 1.7xx10^(2) . Is the reaction mixture at equilibrium? If not, what is the direction of the net reaction?

A mixture of 1.57 mol of N_(2), 1.92 mol of H_(2) and 8.13 mol of NH_(3) is introduced into a 20 L reaction vessel at 500 K . At this temperature, the equilibrium constant K_(c ) for the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) is 1.7xx10^(2) . Is the reaction mixture at equilibrium? If not, what is the direction of the net reaction?

A mixture of 1.57 mol of N_(2), 1.92 mol of H_(2) and 8.13 mol of NH_(3) is introduced into a 20 L reaction vessel at 500 K . At this temperature, the equilibrium constant K_(c ) for the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) is 1.7xx10^(2) . Is the reaction mixture at equilibrium? If not, what is the direction of the net reaction?

A mixture of 1.57 mol of N_(2) ,1.92 mol of H_(2) and 8.17 mol of NH_(3) is introduced in a 20 L reaction vessel at 500 K. At this temperature, the equilibrium constant K_(c) for the reaction is 1.7 xx 10^(-2) . Is the reaction at equilibrium? The reaction is N_(2)(g)+3H_(2)(g) rarr 2NH_(3)(g)