How far? The extent of chemical change

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…

Which change would shift the position of this equilibrium towards the products? $\ce{H2(g) + I2(g) <=> 2HI(g)}$ $\Delta H = -9\ \mathrm{kJ\,mol^{-1}}$ A. Increase pressure B. Decrease pressure C. Increase temperature D. Decrease temperature

A related nitrile, ethanenitrile, $\ce{CH3CN}$, reacts with hydrogen according to the equilibrium: $\ce{CH3CN(g) + 2H2(g) <=> CH3CH2NH2(g)}$ (i) Write the expression for the equilibrium constant, $K$, for this reaction. (ii) Determine the oxidation states that…

A sample of 0.0120 mol of $\ce{NO2}$ was placed in a sealed vessel of volume 1.00 $\mathrm{dm^3}$, which was kept at a constant temperature of 35 °C. (i) Suggest a simple way of keeping the vessel at a constant temperature in a school laboratory. (ii) The…

A sample of 0.0120 mol of $\ce{NO2}$ was sealed in a vessel of volume 1.00 $\mathrm{dm^3}$ and kept at 10.0 °C until equilibrium was established. At equilibrium, the vessel contained 0.00860 mol of $\ce{NO2}$ and 0.00170 mol of $\ce{N2O4}$.…

The amount of $\ce{NO2}$ prepared was checked by titration. The gas was first absorbed in water: $\ce{2NO2(g) + H2O(l) -> HNO3(aq) + HNO2(aq)}$ The resulting solution was made up to 200.0 $\mathrm{cm^3}$ in a volumetric flask, and 20.0 $\mathrm{cm^3}$ portions…

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…

An equilibrium mixture in a 25.0 $\mathrm{dm^3}$ reactor at 500 °C contains 15.0 mol $\ce{N2}$, 22.5 mol $\ce{H2}$ and 5.25 mol $\ce{NH3}$. Calculate the equilibrium constant, $K$, for the reaction.

The volume of the reactor containing the equilibrium mixture described in 3a is suddenly increased at constant temperature. Sketch, on the axes below, how the concentration of hydrogen changes with time until the new equilibrium is established.