An equilibrium mixture in a vessel of capacity 100 litre contain 1 mol `N_(2)`, 2 mol `O_(2)` and 3 mol NO. Find number of moles of `O_(2)` to be added, so that at new equilibrium the concentration of No is 0.04 mol/lit.

An equilibrium mixture in a vessel of capacity 100 litre contain 1 "mol" N_(2).2"mol"O_(2) "and" 3 "mol" NO . Number of moles of O_(2) to be added so that at new equilibrium the conc. Of NO is found to be 0.04 mol//lt.

In a closed vessel of 1 dm^(3) capacity, 1 mol N_(2)(g) and 2 mol H_(2)(g) interact to produce 0.8 mol NH_(3)(g) in the equilibrium mixture. What is the concentration of H_(2)(g) in the equilibrium mixture?

The reaction : CO(g)+3H_2(g)hArr CH_4(g) +H_2O(g) is at equilibrium at 1300 K in a one litre flask. The gaseous equilibrium mixture contains 0.30 mol of CO, 0.10 mol of H_2 and 0.020 mol of H_2O and an unknown amount of CH_4 in the flask. Determine the concentration of CH_4 in the mixture . The equilibrium consant K_c for the reaction at given temperature is 3.90

For the reaction of XO with O_(2) to form XO_(2) the equilibrium constant at 398 K is 1.0 xx 10^(-4) mol^(-1) . If 1.0 mol of XO and 2,0 mol of O_(2) are placed in a 1.0 L flask and allowed to come to equilibrium, the equilibrium concentration of XO_(2) will be

A reaction system in equilibrium according to reaction 2SO_(2)(g)+O_(2)(g)hArr2SO_(3)(g) in one litre vessel at a given temperature was found to be 0.12 mole each of SO_(2) and SO_(3) and 5 mole of O_(2) In another vessel of one litre contains 32 g of SO_(2) at the same temperature. What mass of O_(2) must be added to this vessel in order that at equilibrium 20% of SO_(2) is oxidized to SO_(3) ?

An equilibrium mixture CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g) present in a vessel of one litre capacity at 815^(@)C was found by analysis to contain 0.4 mol of CO, 0.3 mol of H_(2)O, 0.2 mol of CO_(2) and 0.6 mol of H_(2) . a. Calculate K_(c) b. If it is derived to increase the concentration of CO to 0.6 mol by adding CO_(2) to the vessel, how many moles must be addes into equilibrium mixture at constant temperature in order to get this change?

An equilibrium mixture CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g) present in a vessel of one litre capacity at 815^(@)C was found by analysis to contain 0.4 mol of CO, 0.3 mol of H_(2)O, 0.2 mol of CO_(2) and 0.6 mol of H_(2) . a. Calculate K_(c) b. If it is derived to increase the concentration of CO to 0.6 mol by adding CO_(2) to the vessel, how many moles must be addes into equilibrium mixture at constant temperature in order to get this change?

1 mol of N_(2) and 2 mol of H_(2) are allowed to react in a 1 dm^(3) vessel. At equilibrium, 0.8 mol of NH_(3) is formed. The concentration of H_(2) in the vessel is