Equilibrium pressure at which 50% of reactant A(g) will be consumed, keeping constant temperature of 300 K inthe given equilibrium is equal

0.924 mole of A (g) is placed in a 1.00 liter container at 700 ° C, where it is 38.8 % dissociatedwhen equilibrium was established.3 A (g) 5 B (g) + 2 C (g)What is the value of the equilibrium constant, Kc, at the same temperature?

Write down the equilibrium values for:AD*=Y*=C*=I*=G*=T*=m=Marginal propensity to consume=using this (1) c=1000+0.4(y-t)(2) i=500(3) G=400(4) t=300

Consider the following economyC=1000+0.4(Y-T)I=500T=400G=300What is the consumption of equilibrium?

For the reaction ⇌+2H2gS2g2H2Sg, determine the equilibrium constant at 700°C if at this temperature, the equilibrium concentrations are as follows: [H2] = 0.208 M, [S2] = 1.13 × 10-6 M, [H2S] = 0.725 M

If equilibrium constant is 2 at 300 K then the standard free energy change at 300 K and 1 atm pressure is