1 mole of nitrogen is mixed with 3 moles of hydrogen in a `sqrt3` litre container where 66.67% of nitrogen is converted into ammonia by the following reaction : `N_2(g)+3H_2(g) hArr 2NH_3(g)`,Then the value of `K_C` for the reaction
`NH_3(g) hArr 1/2N_2(g) + 3/2H_2` will be :

For a reaction N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g))

One mole of nitrogen is mixed with three moles of hydrogen in a 4 litre container. If 0.25 per cent of nitrogen is converted into ammonia by the following reaction N_2(g) +3H_2 hArr 2NH_3(g) calculate the equilibrium constant of the reaction in concentration units. What will be the value of K for the following reaction? (1)/(2) N_2 (g) + (3)/(2) H_2 hArr NH_3 (g)

1 mol of nitrogen is mixed with 3 mol of hydrogen in a 4 L container. If 0.25% of nitrogen is converted to ammonia by the following reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) then calculate the equilibrium constant K_(c) in concentration units. What will be the value of K_(c) for the following equilibrium? 1/2 N_(2)(g)+3/2 H_(2)(g) hArr NH_(3)(g)

One mole of nitrogen is mixed with three moles of hydrogen in a four litre container. If 0.25 per cent of nitrogen is converted to ammonia by the following reaction N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) , then calculate the equilibrium constant, K_(c) in concentration, units. What will be the value of K_(c) for the following equilibrium? 1/2 N_(2)(g)+3/2H_(2)(g)hArrNH_(3)(g)

One mole of nitrogen is mixed with 3 mole of hydrogen in a closed 3 litre vessel. 20% of nitrogen is converted into NH_(3) . Then K_(C) for the (1)/(2)N_(2)(g)+(3)/(2)H_(2)(g)hArr NH_(3) is

One mole of nitrogen is mixed with 3 mole of hydrogen in a closed 3 litre vessel. 20% of nitrogen is converted into NH_(3) . Then K_(C) for the (1)/(2)N_(2)(g)+(3)/(2)H_(2)(g)hArr NH_(3) is

1 mol of N_(2) is mixed with 3 mol of H_(2) in a litre container. If 50% of N_(2) is converted into ammonia by the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) , then the total number of moles of gas at the equilibrium are

1 mol of N_(2) is mixed with 3 mol of H_(2) in a litre container. If 50% of N_(2) is converted into ammonia by the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) , then the total number of moles of gas at the equilibrium are