The Reaction below has an equilibrium constant of Kp = 2.26 x 104 at 298 K. For Reactions a, b and c, PREDICT whether REACTANTS or PRODUCTS will be favored at equilibrium. CO(g) + 2 H₂(g) = CH3OH(g) a. CH₂OH(g) = CO(g) + 2 H₂(g) b. CO(g) + H₂(g) = CH3OH(8) c. 2 CH3OH(g) = 2 CO(g) + 4H₂(g) Reaction c Reaction a Reaction b Favors REACTANTS Favors PRODUCTS

The Reaction below has an equilibrium constant of Kp = 2.26 x 104 at 298 K. For Reactions a, b and c, PREDICT whether REACTANTS or PRODUCTS will be favored at equilibrium. CO(g) + 2 H₂(g) = CH3OH(g) a. CH₂OH(g) = CO(g) + 2 H₂(g) b. CO(g) + H₂(g) = CH3OH(8) c. 2 CH3OH(g) = 2 CO(g) + 4H₂(g) Reaction c Reaction a Reaction b Favors REACTANTS Favors PRODUCTS

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 equilibrium: CO(g) + 3 H2(g)⇄CH4(g) + H2O(g). If Kp = 5.25 x 10-5 at 1468.0 K, calculate Kc.
True or False: For the reaction, A(g) + 2B(g) <-> 4 C(g) the value of Kp, at a given temperature, equal the value of Kc
The equilibrium reaction below has the Kc = 4.00. If the volume of the system at equilibrium is decreased from 4.00 liters to 2.00 liters, how and for what reason will the equilibrium shift. Be sure to calculate the value of the reaction quotient, Q, and use this to confirm your answer. 2 SO 3 (g) 2 SO2 (g) + O2 (g)
Calculate Kc for each reaction.N2(g)+3H2(g)⇌2NH3(g),Kp=6.2×105 (at 298 K)
Using any data you can find in the ALEKS Data resource, calculate the equilibrium constant k at 25.0 °C for the following reaction. TiC14(g) + 2 H₂O(g) TiO₂ (s) + 4 HC1 (g) Round your answer to 2 significant digits. K = 0 0 X
The Keg for the equilibrium below is 7.82 · 10-2 at 510.0 °C. 2Cl, (g) + 2H20 (g) =4HCI (g) + 02 (g) What is the value of Keg at this temperature for the following reaction? Cl2 (g) + H20 (g) = 2HCI (g) + 02 (g) O 0.280 O 0.0376 O 6.12 - 10-3 O 0.150 O 0.0782
Do not give handwriting solution. Given the following equilibrium reaction and equilibrium constant at 300 K: 2 SO3 (g) ⇌ O2 (g) + 2 SO2 (g) Kp = 0.049 calculate the equilibrium constant (Kp) for the following reaction at the same temperature. Enter your answer with no units. 3 O2 (g) + 6 SO2 (g) ⇌ 6 SO3 (g) Kp = ?
Ethyl acetate is synthesized in a nonreacting solvent (not water) according to the following reaction: CH; CO,H+ C,H; OH = CH;CO,C,Hs + H20 K = 2.2 Acetic acid Ethanol Ethyl acetate For the following mixtures (a-d), will the concentration of H30 increase, decrease, or remain the same as equilibrium is established? c. [CH; CO, C, H5] = 0.88 M, [H2O] = 0.12 M, [CH; CO,H] = 0.044 M, [C,H; OH] = 6.0 M %3D O increase O decrease Oremain the same d. [CH; CO, C,Hs] = 4.4 M, [H2O] = 4.4 M, [CH3CO,H] = 0.88 M , [C,H; OH] = 10.0 M O increase O decrease remain the same e. What must the concentration of water be for a mixture with [CH3 CO2 C,Hs] = 1.0 M, [CH; CO,H] = 0.10 M , and [C,H; OH] = 6.0 M to be at equilibrium? %3D Concentration M
Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample of gas from the system is collected into 5.00 L flask. The flask is found to contain 8.62 g of CO, 2.60 g of H2, 43.0 g of CH4, and 48.4 g of H:O at 320.0 °C. What are the values of Kc and Kp for this reaction? CH:(g) + H2O(g) = CO(g) + 3 H2(g) 1 2 NEXT > Based on the given data, set up the expression for Kc and then evaluate it. Do not combine or simplify terms.
1.If Kp = 845 for the reaction below at 310.0 K, then what is the value of Kc?(R = 0.0821 L･atm/mol･K.) 2 A (g) + B (s) ⇌ 2 C (s) + D (g) 2.A reaction vessel initially contains only 3.5 atm of N₂O₄. When the system reaches equilibrium according to the reaction below, there is 1.7 atm of NO₂ in the vessel. What is Kp for this reaction? 2 NO₂ (g) ⇌ N₂O₄ (g) 3.A solution is made initially with 0.440 M HIO₃ (Kc = 0.170). Once the equilibrium below is established, what is the equilibrium concentration of H⁺ ions? HIO₃ (aq) ⇌ H+ (aq) + IO₃⁻ (aq) 4.An empty steel container is filled with 0.0580 atm of HF. The system is allowed to reach equilibrium. If Kp = 2.76 for the reaction below, what is the equilibrium partial pressure of H₂? 2 HF (g) ⇌ H₂ (g) + F₂ (g)
3. Phosphoryl chloride, POCI3(g), is used in the manufacturing of flame retardants. It is manufactured in an equilibrium process in which phosphorus trichloride reacts with nitrogen dioxide to form POCI3(8)and NO(g) according to the following equation: PCI3 (g) + NO2 (g) = POCI3 (g) + NO (g) The Keg for this reaction at 800 K is 6.90. If 1.25 mol PCI3 (g) and 1.94 mol NO2 (g) are placed into a 2.0 L container, what is the concentration of each gas at equilibrium at 800 K? PCI3 (g) NO2 (g) POCI3 (g) NO(g) Keq = 6.90 + + E
Nitrogen dioxide reacts to form dinitrogen tetroxide as follows: 2 NO2 N₂04 (g) At 150 °C, Kp = 4.51. If one starts with 10.0 atm NO2 (g), what is the equilibrium pressure (in atm) of N₂O4 (g)?