Reversible Reaction Lab Report

Q1 A reversible reaction is one which can go both ways. Reactants react to form products and products can form the reactants again. Under different conditions the reactants and products can still react but may just become a oneway reaction, however a reversible reaction will eventually reach a point of equilibrium where the products are reactant are produced at the same rate. ( AS and A level Chemistry book) Dynamic equilibrium occurs in a closed system where the amounts of products and reactants are not changing anymore and even though there is no visible change the chemical reaction is continually happening known term being equilibrium, where both forwards and backwards reactions are produced at the same rate. The Haber process is the

If more product is added (eg. NH3) then the equilibrium shifts to the left in order to produce more reactants to overcome the change. In the harbour process if the reactant N2(g) or 3H2(g) concentration increases then the position of equilibrium will shift to the right to reduce the amount of reactant and overcome the change which produces more ammonia.

An increase in pressure (less volume) causes the equilibrium to shift to whichever side has least concentration (number of moles) to counteract the change and decrease the pressure again, in ammonia production it would shift to the right creating more ammonia. Decrease in pressure means the equilibrium will shift in order to increase pressure again so in the haber process the equilibrium will shift to the left making more nitrogen and hydrogen. If the concentration of the gases on either side of the reaction are equal, then there will be no effect when there is a change in pressure. But, increase in pressure shifts the position of equilibrium to the side with the least amount of concentration and decrease in pressure shifts it to the side with the higher concentration.

A strong acid will have a weak conjugate base and a weak acid will have a strong conjugate base because strong acids will dissociate fully, giving up protons, so the conjugate base must be weak and a poor acceptor of protons. (chemed.chem.purdue.edu,n.d.)

A acid fully dissociates in solution and the equilibrium will lie more to the right as the acid fully splits up into ions Eg. HCl→H+(aq) + Cl-(aq). HCl splits into hydrogen ions and chlorine ions. In weak acids the equilibrium lies much closer to left as they do not fully dissociate in solution. So, there are going to be less H+ ions available in solution.

ll) Bases are proton acceptors. They neutralise acids, because when in solution they release hydroxides (OH-ions) which mop up excess H+. An alkali is a soluble base which has a PH between 7 and 14. Including ammonia, they release oh- ions in solution. (chemteam.info,n.d.)
Every base has a conjugate acid. The hydroxides released from bases accept protons released from