Magnitude and temperature dependence of K

The second step converts nitrogen monoxide to nitrogen dioxide. $\ce{2NO(g) + O2(g) <=> 2NO2(g)}$ $\Delta H^\ominus = -114\ \mathrm{kJ\,mol^{-1}}$ (i) Identify the oxidation state of nitrogen in $\ce{NO}$ and in $\ce{NO2}$. (ii) State the equilibrium constant…

What can be deduced about this equilibrium reaction from these data? $\ce{A(g) + B(g) <=> 2C(g)}$ Temperature / K Equilibrium constant, K 280 400 340 40.0 A. It is an exothermic reaction and [products] < [reactants] at equilibrium. B. It is an endothermic…

When potassium thiocyanate solution is added to a pale yellow solution containing iron(III) ions, the following equilibrium is established. $\ce{[Fe(H2O)6]^3+(aq) + SCN^-(aq) <=> [Fe(SCN)(H2O)5]^2+(aq) + H2O(l)}$ $\ce{[Fe(H2O)6]^3+(aq)}$ is pale yellow and…

The following system is at equilibrium. $\ce{H2(g) + I2(g) <=> 2HI(g)}$ $K = 54$ What is the value of the equilibrium constant, K, for the reaction $\ce{2HI(g) <=> H2(g) + I2(g)}$? A. $-54$ B. $\dfrac{1}{54}$ C. $\sqrt{54}$ D. $\dfrac{1}{\sqrt{54}}$

The container holding the equilibrium mixture below is compressed to half its volume while the temperature is kept constant. Which row gives the change in the amount of $\ce{PCl5}$ and the effect on the equilibrium constant, $K$?…