State what effect each of the following procedures will have on the rate of this
reaction, and explain in terms of the collision theory why the procedure has the stated
a). The temperature is decreased.
a) rate – the lower temperature means less kinetic energy means fewer
b) rate – higher pressure means greater concentration of reactants
means increased chance of collisions and more effective collisions
c) no change – SO2(g) is a product. Only changes in reactant
concentrations will effect the rate of a forward reaction.
d) rate – grinding up the sulfur increases it’s surface area, increasing
the chance of collisions
e) rate – increasing the volume lowers the pressure which effectively
lowers the concentration O2(g) (a reactant) meaning decreased chance of
collisions and fewer effective collisions
Content will be erased after question is completed.
Enter the email address associated with your account, and we will email you a link to reset your password.
Forgot your password?