Interpretation:
From the given options, the change in position of the equilibrium with very small value for equilibrium constant has to be characterized.
Concept Introduction:
Law of
The equilibrium constant is the product of molar concentrations of the product which is raised to its
Equilibrium Constant:
Consider a reaction,
Forward
Backward reaction rate
At equilibrium, the rate of forward reaction = rate of backward reaction
If the value of the equilibrium constant is larger, then the equilibrium shifts to right. That means the system have more products than reactants.
If the value of the equilibrium constant is smaller, then the equilibrium shifts to left. That is the system will have more reactants than products.
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Chapter 9 Solutions
CHM 104/201 <C>
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- What is the concentration of H2C2O4 at equilibrium if I started with .4 M? (Of course the reaction is with wter) Ka1=7.00E-02) Answer: 2.64E-01 M How do we get to that answer step by step?arrow_forwardWhat will happen to the NO2 concentration at equilibrium if the pressure is decreased NO2(9) N2O3(9) NO(9) + + energy A. increase B. decrease C. stay the samearrow_forwardQUESTION 10 If you know Kb for ammonia, NH 3, you can calculate the equilibrium constant, Ka, for the following reaction: NH4* + H20 =NH3 + HgO* using the equation: O Ka = Kb/ Kyw O Ka = Kw/ Kb O Ka = Kw × Kb O Ka=1/Kb Click Save and Submit to save and submit. Click Save All Answers to save all answers. MacBook Air 000 20 F7 F8 F4 F5 F6 F2 F3 C@ %24 &. %23 2 3 5 8.arrow_forward
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