`N_(2)+3H_(2)hArr 2NH_(3)`. This is gaseous phase reaction taking place in 1L flask at `127^(@)C`. Starting with 1 mole `N_(2)` and 3 moles `H_(2)`, equilibrium required 500mL of 1M HCl. Hence `K_(c)` is approximately

N_2(g)+3H_2(g) hArr 2 NH_3(g) .This is a gaseous phase reaction taking place in 1 L flask at 127^@C .Starting with 1 mole of N_2 and 3 mole of H_2 , the equilibrium mixture obtanied is such that if it is titrated requires 500 mL of 1.0 M H_2SO_4 for neutralisation. Which of the following is the most appropritate K_C ?

N_(2(g)) + 3H_(2(g)) harr 2NH_(3(g)) is a gaseous phase equilibrium reaction taking place at 400K in a 5 L flask. For this

N_(2(g)) + 3H_(2(g)) harr 2NH_(3(g)) is a gaseous phase equilibrium reaction taking place at 400K in a 5 L flask. For this

A gaseous phase reaction taking place in 1 lit at 400K is given N_(2) (g) + 3H_(2) (g) hArr 2NH_(3) (g) starting with 1 mole N_(2) and 3 moles H_(2) equilibrium mixture required 250 ml of 1 M H_(2) SO_(4) . Thus , Ke is

A gaseous phase reaction taking place in 1 lit at 400K is given N_(2) (g) + 3H_(2) (g) hArr 2NH_(3) (g) starting with 1 mole N_(2) and 3 moles H_(2) equilibrium mixture required 250 ml of 1 M H_(2) SO_(4) . Thus , Kc is

For N_(2)+3H_(2)hArr 2NH_(3) , 1 mole N_(2) and 3 mol H_(2) are at 4 atm. Equilibrium pressure is found to be 3 atm. Hence, K_(p) is

N_(2) + 3H_(2)hArr2NH_(3) 1mole N_(2) and 3 moles H_(2) are present at start in 1 L flask. At equilibrium NH_(3) formed required 100 mL of 5 M HC1 for neutralisation hence K_(c) is

For the reaction, N_(2) + 3H_(2) hArr 2NH_(3) in a vessel, equal moles of N_(2) and H_(2) are mixed to attain equilibrium.