Consider the reactions and their respective equilibrium
constants:
NO(g) + 1/2 Br (g) ⇌ NOBr(g) K_p = 5.3
2 NO(g) ⇌ N₂(g) + O₂(g) K_p = 2.1⨉10³⁰
Use these reactions and their equilibrium constants to predict
the equilibrium constant for the following reaction: N₂(g) + O₂(g) + Br₂(g) ⇌ 2 NOBr(g)

검증된 단계별 안내

Identify the target reaction: \( \text{N}_2(g) + \text{O}_2(g) + \text{Br}_2(g) \rightleftharpoons 2\text{NOBr}(g) \).

Recognize that the target reaction can be obtained by manipulating the given reactions.

Reverse the second reaction: \( \text{N}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{NO}(g) \), which changes its equilibrium constant to \( K' = \frac{1}{K_p} = \frac{1}{2.1 \times 10^{30}} \).

Multiply the first reaction by 2: \( 2\text{NO}(g) + \text{Br}_2(g) \rightleftharpoons 2\text{NOBr}(g) \), which squares its equilibrium constant to \( K'' = (5.3)^2 \).

Combine the modified reactions to match the target reaction and multiply their equilibrium constants: \( K_{\text{target}} = K' \times K'' \).

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

주요 개념

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

Equilibrium Constant (K)

The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given chemical reaction. It provides insight into the extent to which a reaction proceeds; a large K indicates a reaction that favors products, while a small K suggests a preference for reactants. Understanding K is essential for predicting the behavior of chemical systems at equilibrium.

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, pressure, or temperature will affect the position of equilibrium, which is crucial when manipulating reactions to achieve desired outcomes.

Manipulating Equilibrium Reactions

To find the equilibrium constant for a new reaction based on known reactions, one can manipulate the given reactions by reversing them or multiplying them to derive the desired equation. The equilibrium constants for these manipulated reactions can then be combined using multiplication or inversion rules. This concept is vital for predicting the equilibrium constant of complex reactions from simpler, known reactions.

Consider the reactions and their respective equilibriumconstants:NO(g) + 1/2 Br (g) ⇌ NOBr(g) Kp = 5.32 NO(g) ⇌ N2(g) + O2(g) Kp = 2.1⨉1030Use these reactions and their equilibrium constants to predictthe equilibrium constant for the following reaction: N2(g) + O2(g) + Br2(g) ⇌ 2 NOBr(g)

비슷한 문제에 대한 검증된 영상 답변:

주요 개념

Equilibrium Constant (K)

Le Chatelier's Principle

Manipulating Equilibrium Reactions