Consider a reaction with a large negative Gibbs energy change, as shown below: YZ, AG/ - 42.6 kJ mol The reaction is initiated by adding 16 mmol of compound Y into the flask, in the absence of compound Z is present. After 48 hours, analysis reveals the presence of 4 mmol of Z and 12 mmol of Y. Which is the most likely explanation? Y and Z have reached equilibrium concentrations. An enzyme has shifted the equilibrium toward Y. Formation of Z is kinetically slow; equilibrium has not been reached by 48 hours. Formation of Z is thermodynamically unfavorable. OTwo of the above explanations are reasonable.

Hydrogen chloride and oxygen react to form chlorine and water, like this: 4 HCl(g) + O,(g) 2 Cl,(g) + 2 H,0(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen chloride, oxygen, chlorine, and water has the following composition: compound concentration at equilibrium HCl 0.46 M O2 1.1M Cl2 1.2 M H20 0.21 M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = 0 Check Explanation O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy | Accessibility

A student ran the following reaction in the laboratory at 1101 K:2SO2(g) + O2(g)      2SO3(g)When she introduced 0.104 moles of SO2(g) and 0.101 moles of O2(g) into a 1.00 liter container, she found the equilibrium concentration of SO3(g) to be 7.28×10-2 M.Calculate the equilibrium constant, Kc, she obtained for this reaction.

Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O2(g)→2 HgO(s) At a certain temperature, a chemist finds that a 7.0 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound amount Hg 7.0 g O2 5.8 g HgO 16.5 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = | x10

Chapter 12 part 1 #12

Select the correct equilibrium constant expression for each of the following chemical equations.

Consider the quilibrium reaction between X and Y, as shown below: X=Y AG The reaction is started with 10 mmol of X; no Y is initially present. After 48 hours, analysis reveals the presence of 10 mmol of X and 0 mmol of Y. Which is the most likely explanation? = −1 - 45 kJ mol X and Y have reached equilibrium concentrations. An enzyme has shifted the equilibrium toward X. Formation of Y is kinetically slow; equilibrium has not been reached by 48 hours. Formation of Y is thermodynamically unfavorable. Two of the above explanations are reasonable.

A student ran the following reaction in the laboratory at 543 K: CoCl₂(g) CO(g) + Cl₂(g) When she introduced 1.10 moles of COCI₂(g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂(g) to be 3.94-102 M. Calculate the equilibrium constant, K, she obtained for this reaction.

Write the equilibrium expression for the following: I2(s) + 3XeF2(s) ↔↔ 2IF3(s) + 3Xe(g)

Ammonia and oxygen react to form nitrogen monoxide and water, like this: 4 NH3(9) + 5O2(g) → 4NO(g) + 6H,O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, oxygen, nitrogen monoxide, and water has the following composition: compound concentration at equilibrium NH, 1.8M 1.6M NO 1.7M AH,0 1.9M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. C. K x10