Group Assignment-4 Chemistry 1110 1. Methanol, CH3OH, is prepared industrially from the following reaction: ΔΗΡ-21.7 Kj Predict the direction of the reaction for the following and EXPLAIN WHY a. Hydrogen gas is added to the equilibrium mixture. b. Carbon monoxide is removed from the equilibrium mixture. c. The pressure is increased. d. The temperature is increased. e. A catalyst is added. f. Methanol is removed from the equilibrium mixture. 2. The reaction: 2 NO(g) +2 H2(g) -N2 +2 H20(g) was studied at 1100K and the following data was collected. Initial Rate, mol/L-min 3.0 x 10-3 9.0 x 10-3 3.6 x 10-2 a. What is the order with respect to NO? with respect to H2? 5.00x10-3 15.0x10-3 15.0x10-3 2.50x103 2.50x103 10.0x103 2 3 b. Determine the overall order of the reaction. C. Write the rate law. 3. State Le Chatelier's Principle and how you will test it in next week's experiment. Is the lab qualitative or quantitative? Explain

Group Assignment-4 Chemistry 1110 1. Methanol, CH3OH, is prepared industrially from the following reaction: ΔΗΡ-21.7 Kj Predict the direction of the reaction for the following and EXPLAIN WHY a. Hydrogen gas is added to the equilibrium mixture. b. Carbon monoxide is removed from the equilibrium mixture. c. The pressure is increased. d. The temperature is increased. e. A catalyst is added. f. Methanol is removed from the equilibrium mixture. 2. The reaction: 2 NO(g) +2 H2(g) -N2 +2 H20(g) was studied at 1100K and the following data was collected. Initial Rate, mol/L-min 3.0 x 10-3 9.0 x 10-3 3.6 x 10-2 a. What is the order with respect to NO? with respect to H2? 5.00x10-3 15.0x10-3 15.0x10-3 2.50x103 2.50x103 10.0x103 2 3 b. Determine the overall order of the reaction. C. Write the rate law. 3. State Le Chatelier's Principle and how you will test it in next week's experiment. Is the lab qualitative or quantitative? Explain

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

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.
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
For the following reaction, which of changes listed below would cause more reactants to form when equilibrium is re- established? 2NO(g) + Cl₂(g) 2NOCI(g) + 75 kJ a. Add a catalyst. b. Increase the volume. C. Increase the temperature. d. Decrease the [NO] e. Increase the pressure.
Given that Kp - 3.0 x 10 for the reaction: 2 CO(g) C(graphite) + CO2(g). what is the partial pressure of CO2(g) at equilibrium if initially 4.00 atm of CO(g) is in contact with graphite? MA. 0.0024.atm B. 0.0060 atm C.0.0048 atm D.0.0012 atm E. 0.0096 atm
Consider the following reaction and its equilibrium constant: 12(g) 2 I(g) Kp = 0.209 A reaction mixture contains 0.89 atm 12 and 1.88 atm I. Which of the following statements is TRUE concerning this system? OA. The reaction quotient will decrease. OB. The reaction will shift in the direction of reactants. OC. The system is at equilibrium. D. The reaction will shift in the direction of products. OE. The equilibrium constant will decrease.
14
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.
Explain deeply
Consider the reaction: 2 NO₂ (g) = N₂O4 (g) At equilibrium, the partial pressures of N₂O4 and NO₂ are 0.35 atm and 4.3 atm, respectively. What is Kp? h O a. 0.16 O b. 0.081 O c. 0.019 O d. 12.28 O e. 52.83 Previous page hp
please answer all parts!
5. Consider the reaction A+B=C+ D. A friend asks the fol- lowing: "I know we have been told that if a mixture of A, B, C, and D is in equilibrium and more A is added, more C and D will form. But how can more C and D form if we do not add more B?" What do you tell your friend? Consider the following statements: "Consider the reaction