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Ch.15 - Chemical Equilibrium
McMurry - Chemistry 8th Edition
McMurry8th EditionChemistryISBN: 9781292336145당신이 사용하는 게 아니라요?교과서 변경
모든 교과서McMurry 8th EditionCh.15 - Chemical Equilibrium문제 115
15장, 문제 115

The reaction of fumarate with water to form L-malate is catalyzed by the enzyme fumarase; Kc = 3.3 at 37°C. When a reaction mixture with [fumarate] = 1.56 * 10-3 M and [l -malate] = 2.27 * 10-3 M comes to equilibrium in the presence of fumarase at 37 °C, what are the equilibrium concentrations of fumarate and L-malate? (Water can be omit- ted from the equilibrium equation because its concentration in dilute solutions is essentially the same as that in pure water.)

검증된 단계별 안내
1
Step 1: Write down the equilibrium expression for the reaction. Since water is not included in the equilibrium expression, the equilibrium constant Kc for the reaction is given by [L-malate]/[fumarate].
Step 2: Set up the ICE (Initial, Change, Equilibrium) table. Initially, [fumarate] = 1.56 * 10^-3 M and [L-malate] = 2.27 * 10^-3 M. Let x be the change in concentration of fumarate and L-malate as the reaction proceeds to equilibrium.
Step 3: Write the equilibrium concentrations in terms of x. The equilibrium concentration of fumarate will be (1.56 * 10^-3 - x) M and the equilibrium concentration of L-malate will be (2.27 * 10^-3 + x) M.
Step 4: Substitute the equilibrium concentrations into the equilibrium expression and set it equal to the given Kc value of 3.3. Solve the resulting equation for x.
Step 5: Substitute the value of x back into the expressions for the equilibrium concentrations of fumarate and L-malate to find their values at equilibrium.

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이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Equilibrium Constant (Kc)

The equilibrium constant (Kc) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. In this case, Kc = 3.3 indicates that at equilibrium, the concentration of L-malate is 3.3 times greater than that of fumarate. Understanding Kc is essential for calculating the equilibrium concentrations of reactants and products.
추천 영상:
가이드 코스
03:20
Equilibrium Constant Expressions

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. This principle helps predict how changes in concentration, temperature, or pressure will affect the position of equilibrium, which is crucial for understanding how the concentrations of fumarate and L-malate will shift in response to their initial concentrations.
추천 영상:
가이드 코스
07:32
Le Chatelier's Principle

Reaction Quotient (Q)

The reaction quotient (Q) is a measure of the relative concentrations of products and reactants at any point in time during a reaction. It is calculated using the same formula as Kc but with the current concentrations. By comparing Q to Kc, one can determine the direction in which the reaction will proceed to reach equilibrium, which is vital for solving the problem of finding the equilibrium concentrations of fumarate and L-malate.
추천 영상:
가이드 코스
00:49
Reaction Quotient Q
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교과서 질문

Consider the following equilibrium: Ag+ (aq) + Cl-(aq) → AgCl(s) Use Le Châtelier's principle to predict how the amount of solid silver chloride will change when the equilibrium is disturbed by: (a) Adding NaCl (b) Adding AgNO3

교과서 질문
The equilibrium constant Kc for the reaction N21g2 + 3 H21g2 ∆ 2 NH31g2 is 4.20 at 600 K. When a quantity of gaseous NH3 was placed in a 1.00-L reaction vessel at 600 K and the reaction was allowed to reach equilibrium, the vessel was found to contain 0.200 mol of N2. How many moles of NH3 were placed in the vessel?
432
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