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(a)
Interpretation:
Effect of increase in concentration of
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
(b)
Interpretation:
Effect of increase in concentration of
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
Effect of decrease in concentration of
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
Effect of decrease in volume of reaction vessel in below reaction 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_forwardConsider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the concentration of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N2(g)? (3) adding water? (4) expanding the container? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?arrow_forwardWrite the expression for the equilibrium constant and calculate the partial pressure of CO2(g), given that Kp is 0.25 (at 427 C) for NaHCO3(s) NaOH(s) + CO2(g)arrow_forward
- Write the equilibrium constant expression for each of the following reactions in terms of concentrations. (a) CO2(g) + C(s) 2 CO(g) (b) [Cu(NH3)4)2+(aq) Cu2+(aq) + 4 NH3(aq) (c) CH3CO2H(aq) + H2O() CH3CO2(aq) + H3O+(aq)arrow_forwardDescribe any thermochemical (heat of reaction) evidence for the Arrhenius concept.arrow_forwardFor the reaction C6H6(g)+3H2(g)C6H12(g)+heat determine in what direction the equilibrium will be shifted by each of the following changes. Decreasing the concentration of H2 a. Increasing the concentration of C6H6 b. Decreasing the temperature c. Increasing the pressure by decreasing the volume of the containerarrow_forward
- For the generalized chemical reaction A(g)+B(g)C(g)+D(g) determine whether the concentration of A in an equilibrium mixture will (1) increase, (2) decrease, or (3) not change when each of the following changes is effected. a. concentration of B is increased b. concentration of C is decreased c. concentration of D is increased d. concentration of D is decreasedarrow_forwardWrite the equilibrium constant expression, K, for the following reaction. Please enter the compounds in the order given in the reaction. If either the numerator or denominator is blank, please enter 1 K = (CH3)3N(aq) + H₂O(1) — (CH3)3 NH+ (aq) + OH¯(aq)arrow_forward(a) What does it mean when the reaction quotient, Q, is numerically equal to the equilibrium constant, Kc? (b) What does it mean when it is less than the equilibrium constant? (c) What does it mean when it is less than the equilibrium constant?arrow_forward
- 28. The reaction 2 CO₂(g) 2 CO(g) + O₂(g) is known to be endothermic. According to Le Chatelier's principle, how will this reaction's equilibrium be affected, if the reaction temperature is increased? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will increase and the reaction will shift to the right. (D) The equilibrium constant will be unchanged, but the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.arrow_forwardwrite the equilibrium constant of the following expression: 6Ca(s) + 2NH3 (g) <--> 3CaH2(s) + CaN2(s)arrow_forwardAmmonia is a weak base that reacts with water according to this equation: NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH −(aq) Will any of the following increase the percent of ammonia that is converted to the ammonium ion in water? (a) Addition of NaOH (b) Addition of HCl (c) Addition of NH4Cl.arrow_forward
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