The equilibrium constant for the generic reaction : A(g) + 3B(g) ⇄ 2C(g) is Keq=1.5x103 At equilibrium the reaction mixture contains: hard to answer: need to know the equilibrium concentrations comparable amounts of reactants and products mostly products mostly reactants only reactants
The equilibrium constant for the generic reaction : A(g) + 3B(g) ⇄ 2C(g) is Keq=1.5x103
At equilibrium the reaction mixture contains:
- hard to answer: need to know the equilibrium concentrations
- comparable amounts of reactants and products
- mostly products
- mostly reactants
- only reactants
Consider the following reaction at 200oC: CO(g) + 2 H2(g)⇌ CH3OH(g); Kc=10.5.
If the concentrations in the reaction mixture at some moment of time are: [CO] = 0.200 M, [H2] = 0.100 M and [CH3OH] = 0.0400M , then
- the system is at equilibrium and no net change will occur
- the system is not at equilibrium and the reaction will proceed to the right
- the system is not at equilibrium and the reaction will proceed to the left
- the system is at equilibrium and the reaction will proceed to the right
- the system is at equilibrium and the reaction will proceed to the left
Consider the following reaction: SO2(g) + O2(g) ⇌ SO3(g)
When the initial amounts of the components of the reaction system were mixed, the pressure in the system started to increase. What statement is correct?
- not enough information to answer
- Kc < Q
- Kc =Q
- Kc >Q
Consider the following reactions. In which cases is the product formation favored by decreased pressure?
1) CO2(g) + C(s)⇌2CO(g)
2) N2(g) + 3 H2(g)⇌ 2 NH3(g)
3) CO(g) + 2H2(g) ⇌CH3OH(g)
4) N2(g) + O2(g) ⇌2 NO(g)
5) 2 H2O(g) ⇌2 H2(g) + O2(g)
- 2, 3
- 3, 4
- 1, 5
- 3, 5
- 2, 4
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