Question

Which of the following reactions should be fast at room temperature? Which would be slow? Explain

A. KCl+AgNO3->KNO3+AgCl
B. H2(g)+Cl2(g)->2 HCL(g)

I would assume that B would react faster because it has all gases.??

Answer 1

I think your assumption is not right. A is almost instantaneous since the aqueous solutions mix instantaneously. B reacts slower because those gases must mix before they react. In addition, Ag^+ and Cl^- are ready to form AgCl as soon as they come in contact with each other. In B, H2 must break the H-H bond, Cl2 must break the Cl-Cl bond, then H atom must collide with a Cl atom to form HCl.

Answer 2

so the temperature doesnt have a whole lot to do with this reaction?

Answer 3

Actually it does. But room temperature doesn't provide the energy to break the H-H and Cl-Cl bonds and that is the primary reason (at least one of the reasons) for the slow reaction. At higher temperatures you have a few individual atoms present and the higher the temperature the more of those individual atoms you have.

Answer 4

thank you

Answer 5

B b/c A is ionic solid so they so hard then required much more activation energy that is not available early but B is in gas phase which is fast at room temperature but it's decreased by increase temperature