The synthesis of CH3OH(g) from CO(g) and H2(g) is represented by the equation above. A sample of each of the three gases is put in a previously evacuated rigid container. The initial concentrations of the gases are shown in the table below. Gas Initial Concentration (M) CO 1.0 H2 0.1 CH3OH 2.0 The temperature of the reaction mixture is held constant at 450 K. In which direction, if any, will the reaction proceed?

The synthesis of CH3OH(g) from CO(g) and H2(g) is represented by the equation above. A sample of each of the three gases is put in a previously evacuated rigid container. The initial concentrations of the gases are shown in the table below. Gas Initial Concentration (M) CO 1.0 H2 0.1 CH3OH 2.0 The temperature of the reaction mixture is held constant at 450 K. In which direction, if any, will the reaction proceed?

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

61
Sulfur trioxide decomposes according to the following reaction. 2 SO3 (g) 2 SO, (g) + O, (g) 0.0437 mol of SO3 was placed in an evacuated 1.00L flask at 100.0 °C. At equilibrium 43.8% of the SO3 had decomposed. Calculate the following: (write answers to three significant figures) 1. [SO3] decomposed M %3D 2. [SO3] at equilibrium %3D 3. [SO2] at equilibrium %3D YouTube 4. [O2] at equilibrium M 5. Determine Kc for the equilibrium reaction.
1. The diagrams below represent the following reversible chemical reaction: H2(g) + 12 (g) =2 HI (g) At 448 °C, the equilibrium constant, K, for this reaction is 51 Initial Conditions: Temperature = 448 °C Volume of the container = 2.0 L 0 = 1 mole H2 (g) = 1 mole I2 (g) 00 00 .. 00 00 •. What is the initial molar concentration of hydrogen. [H:]? What is the initial molar concentration of iodide, [I2]? M This system will reach equilibrium when rate of the forward reaction is equal to the rate of the reverse reaction. Write the equilibrium constant expression, Kc, for this reaction: Calculate the equilibrium concentrations for H;(g), I (g) and HI (g) H2(g}_ + l2 (g) 2 HI (g) [H2] [L2] [HI Initial Change Equilibrium +2x -X-
For the reaction of NO2 to form NO and O2, which reaction vessel (all at different temperatures) would yield the smallest equilibrium constant? 2 NO2(g) +2 NO(g) + O2(g) → is supposed to be an equilibrium arrow
Consider the following reaction where Kc = 1.20×10-2 at 500 K:PCl5 (g) PCl3 (g) + Cl2 (g)A reaction mixture was found to contain 0.115 moles of PCl5 (g), 4.47×10-2 moles of PCl3 (g), and 4.16×10-2 moles of Cl2 (g), in a 1.00 liter container.Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium PCl5(g) must be consumed . 2. In order to reach equilibrium Kc must increase . 3. In order to reach equilibrium PCl3 must be consumed . 4. Qc is less than Kc. 5. The reaction is at equilibrium. No further reaction will occur.
Phosphorus pentachloride decomposes according to the chemical equation: PCIs(g) → PCl3(g) + Cl₂(g) Kc = 1.80 at 250.0 °C A 45.0 gram sample of PCI-(g) is injected into an empty 5.00-liter reaction vessel held at 250.0 °C. Calculate the pressure, in atm, of the vessel when equilibrium is reached.
3.) For the following equilibrium reaction2NO2(g) ↔N2O4(g) + Δlook in the Tro text to see what LeChatelier's principle states about gases. Assume that the reaction occurs in an enclosed movable piston. [Hint: remember that PV=nRT] a.) The pressure of the reaction is increased. b.) The volume of the reaction is decreased. c.) The volume of the reaction is increased.
4. For the reaction CH4(g) + 2 H2S(g) = CS2(g) + 4 H₂(g) Kc = 3.59 at 900 °C. For each of the following measured concentrations determine whether the reaction is at equilibrium. If not, in which direction will the reaction proceed to get to equilibrium? [CH] [H₂S] [CS₂] [H2] Expt 1 Expt 2 Expt 3 1.15 1.07 1.10 1.20 1.20 1.49 1.51 0.90 1.10 1.08 1.78 1.68
Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO₂(g) + H₂O(1)→2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 3.4 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound NO₂ H₂O HNO3 NO amount 5.9 g 142.0 g 15.1 g 12.0 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. с K = D 0 C x10 X Ś
Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 200. mL flask with 4.6 atm of ammonia gas, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 4.8 atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits.
*****
Indicate whether either an increase or a decrease of pressure obtained by changing the volume would increase the amount of product in each of the following reactions.