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# Review Questions for a Chemistry Final

I'm reviewing for my chemistry final and need stuff explained. Please give very in-depth explanations and answers so I can understand how to do it. Thank you!

Determine the amount of heat (in kJ) given off when 1.26x10^4g of N02 are produced according to the equation;
2NO(g)+O2(g)---->2NO2(g) Change of heat=-114.6 kJmol

A sheet of gold weighing 10.0g and at a temperature of 18.0 degreesC is placed flat on a sheet of iron weighing 20.0g and at a temperature of 55.6 degreesC. What is the final temperature of the combining metals? Assume that no heat is lost to the surroundings.

A quantity of 2.00x10^2 ml of 0.862 M HCl is mixed with 2.00x10^2ml of 0.431 M Ba(OH)2 in a constant-pressure calorimeter of negligible capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.48 degreesC. For the process
H+(aq)+OH-(aq)----->H2O(l)
the heat of neutralization is -56.2 kJmol. What is the final temperature of the mixed solution?

The first step in the industrial recovery of zinc from the zinc sulfide ore is roasting, that is, the conversion of ZnS to ZnO by heating:
2ZnS(s)+3O2(g)---->2ZnO(s)+2SO2(g) Change in heat rxn=-879 kJmol
Calculate the heat evolved (in kJ) per gram of ZnS roasted.

#### Solution Summary

This solution provides answers for the chemistry final exam review questions attached.

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