Sorry for the late reply guys, I'm a real menace with technology sometimes! Also, I bought some really engrossing books in London... back to topic!
1. Add the same concentration of (reactant A) to a conical flask and then add a volume of (reactant B) which will react to give a precipitate.
2. Measure the amount of time between adding B to A and a precipitate being formed, and record this as the rate of reaction.
3. Repeat at different concentrations of B and record results, whilst keeping [A] constant.
4. If the reaction is first order with respect to B, doubling
will effect a twofold increase in the reaction rate.
How's that?
Q: Explain why transition metals often yield coloured compounds.
Sorry for the late reply sir, I hope I've not ruined your revision session with Otrivine!
Well... if the ionic charge is larger, then the ions will experience a greater attraction to each other and the lattice enthalpy will be larger as more energy will be released when they become a solid compound. If the ionic radius is larger, the lattice enthalpy will be smaller as the attractive force of the ionic charges will have to act over a larger radius? I haven't looked at this in a while if I'm honest, you can probably tell!
Q: Describe the graphs for rate vs. time for first, second and zero order reactions.