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(a)
Interpretation:
Direction of shift of equilibrium with changes brought in below equation has to be determined.
Concept Introduction:
Le Chatelier’s principle states that changes at equilibrium in system respond to reduce the changes and bring back the system to restore its equilibrium under new conditions. This principle follows certain conditions that are as follows:
1 With increase in concentration of reactants the reaction moves towards forward direction thus this increases the concentration of products. Whereas with increase in concentration of product reaction shifts towards reverse direction. This increases the concentration of reactants.
2 Change in volume affects
3 With increase in temperature reaction rate rises due to rise in kinetic energy. In case of endothermic reaction that is when energy is absorbed then the reaction moves in forward direction. In case of exothermic reaction that is when energy is released then reaction moves in backward direction.
4 Catalyst is a substance that affects rate of
(b)
Interpretation:
Direction of shift of equilibrium with changes brought in below equation has to be determined.
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
Direction of shift of equilibrium with changes brought in below equation has to be determined.
Concept Introduction:
Refer to part (a).
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Chapter 16 Solutions
FOUND.OF COLLEGE CHEMISTRY
- Write an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a productarrow_forwardDescribe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.arrow_forwardThe dehydrogenation of benzyl alcohol to make the fla- voring agent benzaldehyde is an equilibrium process described by the equation C,H;CH,OH(g) 2 C,H;CHO(g) + H2(g) At 523 K, the value of its equilibrium constant is K = 0.558. (a) Suppose 1.20 g of benzyl alcohol is placed in a 2.00-L vessel and heated to 523 K. What is the partial pres- sure of benzaldehyde when equilibrium is attained? (b) What fraction of benzyl alcohol is dissociated into products at equilibrium?arrow_forward
- Write the pressure equilibrium constant expression for this reaction. 2 H₂(g) + O₂(g) → 2 H₂O(1) 0 X Ś 010 ?arrow_forwardWhat is the equilibrium constant for: CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g), Is it Homogenous or Heterogenous?arrow_forwardConsider the equilibrium4NO2(g) + 6H2 O(g) ⇌ 4NH3(g) + 7O2(g)(a) What is the expression for the equilibrium constant (Kc) of the reaction?(b) How must the concentration of NH3 change to reach equilibrium if the reaction quotient is less than the equilibrium constant?(c) If the reaction were at equilibrium, how would a decrease in pressure (from an increase in the volume of the reaction vessel) affect the pressure of NO2?(d) If the change in the pressure of NO2 is 28 torr as a mixture of the four gases reaches equilibrium, how much will the pressure of O2 change?arrow_forward
- What is the symbolic expression for the equilibrium constant for the reaction: 2 C2H6(g) + 7 O2(g) ⇌ 4 CO2(g) + 6 H2O(g)?arrow_forwardConsider the reaction 2 SO2(g) + O2(g) 2 SO3(g) at 1000 K. In a 1.00 L reaction vessel, 0.440 mol SO2, 0.220 mol O₂ and 0.440 mol SO3 are introduced simultaneously. If the Kç is 2.82 x 10², which of the statements below is TRUE? Q > Kc so the reaction will proceed in the reverse direction to attain equilibrium. The reaction is at equilibrium since T is constant. O Kp = Kc since T is constant. O Q< Kc so the reaction will proceed forward and form more SO3 to attain equilibrium.arrow_forwardSuppose a 500. mL flask is filled with 1.9 mol of CO, 0.60 mol of H₂O and 1.7 mol of H₂. The following reaction becomes possible: CO (g) + H₂O(g) → CO₂(g) + H₂ ( (g) 2 The equilibrium constant K for this reaction is 1.81 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. 2 M X Ś ?arrow_forward
- (a) Is the dissociation of fluorine molecules into atomicfluorine, F2(g)⇌ 2 F(g) an exothermic or endothermicprocess? (b) If the temperature is raised by 100 K, doesthe equilibrium constant for this reaction increase or decrease? (c) If the temperature is raised by 100 K, doesthe forward rate constant kf increase by a larger or smalleramount than the reverse rate constant kr?arrow_forwardWhat is the expression for the equilibrium constant for the reaction: 2 C2H6(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)?arrow_forwardWhat is the expression for the equilibrium constant for the reaction: 2 C2H6(g) + 7 O2(g) ⇌ 4 CO2(g) + 6 H2O(g)?arrow_forward
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