I need guidance on tackling this assignment.

My professor has stated that she does not expect us to design an experiment from scratch, instead she wants us to think critically. I have read the background document and I am at a loss of what to do. Can you help? The instructor posted the following in response to a confused classmates question;: When you think about determining order, if you double the concentration of a reactant and the rate doubles, what is the order of the reaction? What if the rate remained the same, or what if the rate quadrupled? That is all we are doing in this reaction, determining rate, order, k, and looking at Arrhenius equation. I am not asking you to design an experiment from scratch, I have given you all... click for more

zero and second order reaction

The second order reaction for the decomposition of nitrosyl bromide has a half life of 12.5seconds at a concentration of 0.100M. NOBr(g)-->NO(g) + 1/2Br2(g) I need help finding k for the reaction, and how would I find how long it will take to decompose 80 % of a 0.0500M solution of nitrosyl bromide, and how fast 0.200M solution of nitrosyl bromide will decompose.

Zero order reaction

For the zero order decomposistion of HI on a gold surface it takes 1.0 seconds for the concentration of HI to drop from 0.335M to 0.285M. HI(g)---> 1/2H2(g)+1/2I2 I need to know what is the rate constant for the reaction, how long will it take for the concentration of a 0.650M solution to drop to 0.0100M, and what is the half life of a 0.400M solution

activation energy

I am trying to find deltaH. The activation energy is 128kJ for this reaction. The activation energy for the reverse reaction is 95kJ. In the presence of a catalyst Eacat is 110kJ.

calorimetry

I just need to know the formula for this problem I cannot find it in my book. If you have 2.40 mol of Au at 100 degrees C and is added to 10.mol of water at 25 degrees what will be the final temp...cpAu=25 J/Km and cp of water=75.3J/Km. Thanks