5. Predict the effect of the change described in the first column of the followi
ID: 855444 • Letter: 5
Question
5. Predict the effect of the change described in the first column of the following table upon the
quantity appearing in the second column of the table for the following equilibrium system:
O3(g) + Mn+2(aq) + H2O(l) = O2(g) + MnO2(s) + 2H+(aq) DeltaH? = -157 kJ/mol (exothermic)
Change
Quantity
Answer
(a) add some O3
Amount of H2O
(b) add He(g) at constant V
Amount of O2
(c) increase the volume
K
(d) add He(g) at constant V
Ptot
(e) decrease the temperature
K
(f) add a catalyst
Amount of O2
(g) add He(g) at constant Ptot
Amount of Mn+2
Change
Quantity
Answer
(a) add some O3
Amount of H2O
(b) add He(g) at constant V
Amount of O2
(c) increase the volume
K
(d) add He(g) at constant V
Ptot
(e) decrease the temperature
K
(f) add a catalyst
Amount of O2
(g) add He(g) at constant Ptot
Amount of Mn+2
Explanation / Answer
please find the extra explanation asked further in the comment
1. addition of reactant favours forward reaction increasing amount of products hence decreasing amount of reactants
2 This is because the addition of a non-reactive gas does not change the partial pressures of the other gases in the container.
3.Rate constatn is independant of other factors apart from temperature
4.addition of inert gas increases the number of molecules hence inrease the pressure
5.An increase in temperature will always increase the rate of a reaction since the particles will have more kinetic energy and there would be more productive collisions.
6. catalyst inreases rate of reaction and hence amount of oxygen
7. When both sides of the equation have the same number of moles, pressure changes will not influence the amounts of the various substances present at equilibrium. This is because there is no way for the system to counteract pressure changes.
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