`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

In a one litre containder 1 mole of N_(2) and 3 moles of H_(2) were introduced. After some time at equilibrium, ammonia formed requires 100 ml of 1 M H_(2)SO_(4) for complete neutralisation. Then K_(c) for reaction will be

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

Consider the following reaction equilibrium N_(2)(g) + 3H_(2)(g) hArr 2NH_(3)(g) Initially, 1 mole of N_(2) and 3 moles of H_(2) are taken in a 2 flask. At equilibrium state if, the number of moles of N_(2) is 0.6, what is the total number of moles of all gases present in the flask ?

For the reaction, N_(2)+3H_(2)hArr2NH_(3) , in a vessel equal moles of N_(2) and H_(2) are mixed to attain equilibrium. At equilibrium:

N_(2)+3H_(2)rarr2NH_(3) . 1 mol N_(2) and 4 mol H_(2) are taken in 15L flask at 27^(@)C After cmomplete conversion of N_(2) into NH_(3),5L of H_(2)O is added pressure set up in the flask is:

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 ?

1 "mole of" N_(2) "and" 3 "moles of " H_(2) are placed in 1L vessel. Find the concentration of NH_(3) at equilibrium, if the equilibrium constant (K_(c)) at 400K "is" (4)/(27)