Consider the following equilibrium system and then indicate whether the followin

Question

Consider the following equilibrium system and then indicate whether the following statements are true or false; be prepared to defend your answers. 2CO_(g) + O_2(g) rightarrow 2CO_2(g); Delta G degree - -51.4 kJ. When equilibrium is reached after both reactants are placed in an empty vessel at standard conditions, P_CO = P_CO2 When both reactants are placed in an empty vessel at standard conditions, CO_2 will from rapidly because Delat G degree is negative and large. When the forward reaction occurs, the entropy of the system, S_sys, increase. This system is reactant-favored at standard conditions. If CO_2 and CO are placed in an empty vessel at standard conditions, more CO_2 will form. Delta H degree for the forward reaction is positive. Delta G for the reaction becomes a more positive number as T increases. If CO_2 at P = 1.0 atm is placed alone in a vessel at 25 degree C, a chemical reaction will occur. When all substances are placed in an empty vessel at standard conditions, equilibrium will be reached only when more CO_2 has formed.

Explanation / Answer

5. a) false, because at equilibrium the partial pressures of reactants=products

b) False, although the delta G of reaction is -ve it may not proceeds rapidly at Standrad conditions

c) False, in products the no. of moles are lower than reactants entropy decreases

d) True, since delta G is -ve it favors at low temp.

e) True, because the delta G is -ve it favors the formation of products

f) False, delta H is -ve because dG is -ve and dS is +ve

g) True, Since it is exothermic high temperature favors backward reaction

h) false

i) True

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