On an educational website, this image would be presented to teach concepts related to chemical equilibria and the effects of temperature changes on such systems. Below is a detailed transcription and explanation:---### Understanding Chemical Equilibria: Temperature Effects**Question:**What is correct when temperature increases in this reaction at equilibrium?\[ \text{2NOCI(g) ↔ 2 NO(g) + Cl}_2\text{(g)} \quad \Delta H^\circ = +75.5 \text{kJ} \]**Options:**| Position of Equilibrium | Equilibrium Constant, \( K_c \) ||--------------------------|-------------------------------|| **A.** Shifts left | Unchanged || **B.** Shifts left | Decreases || **C.** Shifts right | Unchanged || **D.** Shifts right | Increases |**Explanation:**This reaction has a positive enthalpy change (\( \Delta H^\circ = +75.5 \text{kJ} \)), indicating it is an endothermic reaction. According to Le Chatelier's Principle, if the temperature is increased, the equilibrium will shift to favor the direction that absorbs heat. In this endothermic reaction, heat is absorbed when the reactants (2NOCls) are converted into products (2 NOs and Cl₂). Therefore, the position of equilibrium will shift to the right (towards the products).Additionally, an increase in temperature of an endothermic reaction increases the value of the equilibrium constant (\( K_c \)) since the equilibrium position favors the products more.**Correct Option:**| **D.** Shifts right | Increases |

From the enthalpy change if reaction it is well known that reaction is endothermic reaction so heat…

What is correct when temperature increases in this reaction at equilibrium? 2 NOCI(g)= 2 NO(g)+Cl2 (g) AHº = +75. 5 kJ Position of equilibrium Equilibrium constant, K, A. Shifts left Unchanged B. Shifts left Decreases C. Shifts right Unchanged D. Shifts right Increases

What is correct when temperature increases in this reaction at equilibrium? 2 NOCI(g)= 2 NO(g)+Cl2 (g) AHº = +75. 5 kJ Position of equilibrium Equilibrium constant, K, A. Shifts left Unchanged B. Shifts left Decreases C. Shifts right Unchanged D. Shifts right Increases

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Ammonia and oxygen react to form nitrogen monoxide and water, like this: 4 NH3(g) + 502(g) → 4 NO(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 pressure at equilibrium NH3 23.4 atm O2 40.2 atm NO 87.8 atm H,0 63.4 atm Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.
Question 4
Consider the following reaction at equilibrium: 2CO2 (g) 2CO (g) + 02 (g) AH° = -514 kJ Le Châtelier's principle predicts that adding additional O2 (g) from the reaction container will A) The reaction will shift to decrease the pressure. B) The reaction will shift in the direction of the reactants. . C) The reaction will shift in the direction of the products. D) The equilibrium constant will decrease. E) No change in the reaction
Consider the following system at equilibrium where H° = -18.8 kJ, and Kc = 10.5, at 350 K:2CH2Cl2(g) CH4(g) + CCl4(g)If the TEMPERATURE on the equilibrium system is suddenly increased: The value of Kc fill in the blank 1 A. Increases B. Decreases C. Remains the same The value of Qc fill in the blank 2 A. Is greater than Kc B. Is equal to Kc C. Is less than Kc The reaction must: fill in the blank 3 A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of CCl4 will: fill in the blank 4 A. Increase. B. Decrease. C. Remain the same.
4. A. An important reaction in the commercial production of hydrogen is CO(g) + H2O(g) --><-- H2(g) + CO2(g) How will the system at equilibrium shift in each of the five following cases? (Use arrows or write "right" , "left" , or "no shift"). a. Gaseous carbon monoxide is removed b. In rigid reaction container, a catalyst is added. c. The temperature is decreased (the reaction is exothermic). d. The reaction container volume is doubled. e. Hydrogen gas is added. B. The equation above has a Kc value of 7.5 x 102. If 2.0 moles of each reactant and product are put into the same sealed 4.0 L container, determine the concentrations of all species present at equilibrium. Please answer A with sub parts and B.
The decomposition of PCl5 occurs by the equilibrium process PCl5(g) = PCl3(g) + Cl2(g) DH, = 92.5 kJ mol–1 If the reaction is initially at equilibrium, explain what happens when the temperature is lowered. Select one: a. The equilibrium shifts left b. The concentration of Cl2(g) will increase c. No change d. The equilibrium shifts right
The chemical equation represents a reversible reaction. 3H2(9) + N2(9) # 2NH3(g) At equilibrium, 1 liter of a mixture of gases at 450°C contains 1.83 mol of hydrogen (H2), 0.793 mol of nitrogen (N2), and 1.72 mol of ammonia (NH3).What is the equilibrium constant for the reaction under these conditions? O A. 0.718 B. 0.609 O C. 1.39 O D. 0.159 96 5 6
23 and 24 please
Bromine and water react to form hydrogen bromide and oxygen, like this: 2 Br, (g) + 2 H,0(g) - 4 HBr(g) + 0,(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of bromine, water, hydrogen bromide, and oxygen has the following composition: compound pressure at equilibrium Br, 49.2 atm H,0 80.9 atm HBr 94.3 atm O2 62.5 atm Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. * = 0
Which reaction, when at equilibrium, would be unaffected by a change in pressure? A. N2(g) + O2 (g) = 2NO(g) B. 2CO(g) + O2 = 2CO2(g) C. COBr2(g) = CO(g) + Br2(g) D. N2O4(g) = 2NO2 (g)
Consider the following system at equilibrium where H° = -18.8 kJ, and Kc = 10.5, at 350 K:2CH2Cl2(g) CH4(g) + CCl4(g)If the TEMPERATURE on the equilibrium system is suddenly increased: The value of Kc fill in the blank 1 A. Increases B. Decreases C. Remains the same The value of Qc fill in the blank 2 A. Is greater than Kc B. Is equal to Kc C. Is less than Kc The reaction must: fill in the blank 3 A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of CCl4 will: fill in the blank 4 A. Increase. B. Decrease. C. Remain the same.
5. Consider the following reaction: N2(g) + 3 H₂(g) 2 NH3(g) At equilibrium, the pressure values of the substances were 0.62 atm N2, 0.50 atm H2, and 0.24 atm NH3. What is Keq for the reaction? a. 0.74 b. 2.7 c. 1.3 d. 0.60 e. 0.37