At `46^@C, K_p` for the reaction `N_2O_4(g) iff 2NO_2(g)` is 0.66. Calculate the partial pressure of `N_2O_4` and `NO_2` at equilibrium and at a total pressure of 0.5 atm.

Calculate the partial pressure of SO_2 in a mixture with 60% CO_2 and total pressure being 4 atm.

For the reaction, N_(2)O_(4)(g)hArr2NO_(2)(g) occurring in a closed vessel at 300K, the partial pressures of N_(2)O_(4)(g) and NO_(2)(g) at equilibrium are 0.28 atm and 1.1 atm respectively. What will be the partial pressures of these gases if the volume of the reaction system is doubled keeping the temperature constnt ?

For the reaction, 2NH_3(g) iff N_2(g) + 3H_2(g) the units of K_p will be

For the reaction H_2O(s) iff H_2O(l) at 0^@C and normal pressure

The value of K_p for the reaction 2H_2O(g) +2Cl_2(g) iff 4HCl(g) +O_2(g), is 0.035 atm at 400^@C , when the partial pressure are expressed in atmosphere. Calculate the value of K_c for the same reaction.

At a particular temperature, the value of K_(p) is 100 for the reaction, 2NO(g)hArrN_(2)(g)+O_(2)(g) occurring in a closed container. If the iniital pressure of NO(g) be 25 atm then calculate the partial pressures of NO, N_(2) and O_(2) at equilibrium.

Determine K_p for the given reaction reaction : N_2O_4(g) iff 2NO_2(g), K_c = 4.62 xx 10^-3 M at 298 K

At a given temperature, K_(p) is 0.36 for the reaction, 2SO_(2)(g)+O_(2)(g)hArr2SO_(3)(g) occurring in a closed vessel. If at equilibrium, the partial pressures of SO_(2)(g)&O_(2)(g) be 0.15 atm & 0.8 atm respectively, then calculate the partial pressure of SO_(3)(g) .