How far? The extent of chemical change

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

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…

The cyanide ion acts as a ligand in many complex ions, for example hexacyanoferrate(III), $\ce{[Fe(CN)6]^3-}$. (i) State the type of bond, as precisely as possible, that joins each cyanide ion to the iron ion. (ii) Deduce the oxidation state of iron in…

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, 0.00860 mol of $\ce{NO2}$ remained in the vessel. Using the expression below, determine $K$ for…

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…

Cresolphthalein is a weak acid that can be represented as HIn. Using an equation, explain why the colour of a solution containing cresolphthalein depends on its pH.

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…

State, in terms of equilibrium concentrations, the expression for $K$, the equilibrium constant of this reaction.

By the time equilibrium was reached, the vessel held 1.7 mol of $\ce{H2(g)}$. Calculate the equilibrium amounts, in mol, of the three remaining gases, then use them to calculate $K$.