Given a gas phase reaction `2A(g)+B(g)hArr C(g)+D(g)`. Which one of the following changes will affect the value of `K_(c)`?

Consider the reaction, A(g)+2B(g)hArr 2D(g)+3E(g)+ heat and state how the following changes at equilibrium will affect the yield of the product. D(g)- pressure is increased at constant temperature.

Consider the reaction, A(g)+2B(g)hArr 2D(g)+3E(g)+ heat and state how the following changes at equilibrium will affect the yield of the product. D(g)- temperature is increased.

For the given reaction 2A(g)+ B(g) hArr C(g) , Delta H = x kJ which of the following favour the reactants ?

For the given reaction 2A(g)+ B(g) hArr C(g) , Delta H = x kJ which of the following favour the reactants ?

For reaction H_(2)(g) +I_(2)(g) hArr 2HI (g) The value of K_(p) changes with

For the reversible reaction : A_(s) + B_(g) hArr C_(g) + D_(g) : Delta G^(@) = - 350 kJ Which one of the following statements is true ?

For the gas-phase reaction, 2NO hArr N_(2) + O_(2) : Delta H = -43.5 keal. Which one of the following is false for the reaction N_(2) (g) + O_(2) (g) hArr 2NO(g)