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
General, Organic, and Biological Chemistry
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- hi Tester 8 Chem 1110 Johnson/Lippert Q 9 - Carrie Fletcher For the reaction a) adding a catalyst b) decreasing the temperature C C6H6 (g) + 3 H₂ (g) C6H12 (g) + heat Determine which of the following will shift the equilibrium to the left. Chi Tester g) more than one correct response h) no correct response c) increasing the pressure by decreasing the volume of the container d) decreasing the concentration of H₂ e) increasing the concentration of C6H6 f) decreasing the concentration of C6H12 For whicharrow_forwardThe reaction below has an equilibrium constant of K₂ = 2.26 x 10¹ at 298 K. CO(g) + 2H₂(g) = CH₂OH(g) Calculate K₂ for the reaction below. CH₂OH(g) = CO(g) + 2H₂(g) IVE ΑΣΦ K= Submit X Incorrect; Try Again; 3 attempts remaining Part B Previous Answers Request Answer Predict whether reactants or products will be favored at equilibrium in the reaction above. Reactants will be favored at equilibrium. O Products will be favored at equilibrium. Submit Part C ✓ Correct Previous Answers K= Calculate Kp for the reaction below. CO(g) + H₂(g) =CH₂OH(g) IVE ΑΣΦ ? ?arrow_forwardThe equilibrium constant, K, for the following reaction is 7.00×10-5 at 673 K. NH,I(s) NH3(g) + HI(g) This reaction is favored at equilibrium. Enter PRODUCT or REACTANT. The concentrations of NH3 and HI will be at equilibrium. Enter HIGH or LOW. Submit Answer Try Another Version 2 item attempts remainingarrow_forward
- 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
- If an equilibrium for a reaction is said to lie to the RIGHT then the equilibrium constant ____. Select one: A. is a negative value B. is a positive value less than one C. is a positive value greater than one D. is equal to onearrow_forwardH2(g) + 12(g) = 2HI(g) (= is equilibrium sign) At particular temperature, The equilibrium constant (K) = 100 If 1.0 mole of H2, 1.0 mol of I2 and 1.79 mol of HI are introduced into 1.00 L container. The concentration of HI when equilibrium is reached is Write your answer to 1 d.p e.g 7.6 Answer:arrow_forwardWhich side of the equilibrium shown in the following figure is favored? Select the favored set of compounds from the choices given. -NH₂ + -NH₂ + ONH₂ + OH OH NH3 + O At equilibrium, essentially equal amounts of reactants and products will exist. Submit Request Answerarrow_forward
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