Answered

IDNStudy.com, kung saan ang mga eksperto at komunidad ay nagtutulungan para sagutin ang iyong mga tanong. Makakuha ng mabilis at eksaktong sagot sa iyong mga tanong mula sa aming mga eksperto na laging handang tumulong.

A student ran the following reaction in the laboratory at 288 K:

2NO(g) + Br2(g) 2NOBr(g)

When she introduced 0.164 moles of NO(g) and 0.131 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBr(g) to be 0.128 M.

Calculate the equilibrium constant, Kc, she obtained for this reaction.

Sagot :

SOLUTION:

Step 1: Calculate the initial concentration of each species.

[tex]\begin{aligned} & [\text{NO}]_i = \frac{\text{0.164 mol}}{\text{1.00 L}} = 0.164 \: M \\ & [\text{Br}_2]_i = \frac{\text{0.131 mol}}{\text{1.00 L}} = 0.131 \: M \\ & [\text{NOBr}]_i = 0 \end{aligned}[/tex]

Step 2: Summarize the concentrations of each species by using ICE table.

[tex]\begin{array}{lccccc} & 2\text{NO}(g) & + & \text{Br}_2 & \rightleftharpoons & 2\text{NOBr}(g) \\ \text{Initial} \: (M): & 0.164 & & 0.131 & & 0 \\ \text{Change} \: (M): & -2(0.064) & & -0.064 & & +2(0.064) \\ \hline \text{Equilibrium} \: (M): & 0.036 & & 0.067 & & 0.128 \\ \end{array}[/tex]

Step 3: Calculate the equilibrium constant.

[tex]\begin{aligned} K_{\text{c}} & = \frac{[\text{NOBr}]^2}{[\text{NO}]^2[\text{Br}_2]} \\ & = \frac{0.128^2}{(0.036)^2(0.067)} \\ & = 188.6862 \\ & \approx \boxed{189} \end{aligned}[/tex]

Hence, the equilibrium constant obtained by the student for the reaction is 189.

[tex]\\[/tex]

#CarryOnLearning

Ang iyong presensya ay mahalaga sa amin. Magpatuloy sa pagtatanong at pagbahagi ng iyong nalalaman. Sama-sama tayong magtutulungan upang makamit ang mas mataas na antas ng karunungan. Bawat tanong ay may sagot sa IDNStudy.com. Salamat at sa muling pagkikita para sa mas maraming solusyon.