Consider a reaction mixture with the given partial pressures and equilibrium constant:2 SO2 (g)4.00 atm+O2 (g)0.45 atm1L2 SO3 (g)7.20 atmK=5.00Is the reaction mixture at equilibrium? If it is not, which way will it shift in order to get to equilibrium?A) it is at equilibriumB) it is not at equilibrium and it will shift to the right until it reaches equilibriumC) it is not at equilibrium and it will shift to the left until it reaches equilibrium

To determine if the reaction mixture is at equilibrium, we need to compare the given partial…

Answered: Consider a reaction mixture with the…

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...

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Consider the equilibrium system described by the chemical reaction below. A mixture of gas containing only N₂ and H₂ is reacted in a vessel at high temperature. At equilibrium, the 5.0 M H₂, 8.0 M N₂, and 4.0 M NH 3 are present. Determine the initial concentrations of H₂ and N₂ that were present in the vessel. N₂(g) + 3 H₂(g) = 2 NH3(g) Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -2.0 0 2.0 5.0 -5.0 N₂(g) 8.0 1 6.0 + 4.0 -6.0 3 H₂(g) -4.0 10.0 2 NH3(g) RESET 11.0
For the equilibrium system below, which action will cause an equilibrium shift to the left? 2 NOCI (g) + energy 2 NO (g) + Cl₂ (g) An increase in temperature A decrease in pressure A decrease in volume Removal of Cl₂ (g) All of the above will cause a shift to the left
The equilibrium constant for the reaction given below can be determined experimentally when known amounts of hydrogen iodide in a sealed tube are heated until equilibrium is attained. 2HI(g) ➡ H2(g) + I2(g) ΔH= -63KJ/mol State the equilibrium law Write the equilibrium constant expression for the reaction.
Suppose a 250. mL flask is filled with 1.1 mol of Cl2, 0.20 mol of CHCl3 and 2.0 mol of HCl. The following reaction becomes possible: Cl2(g) + CHCl3(g) HCl(g) +CCI4(g) The equilibrium constant K for this reaction is 0.652 at the temperature of the flask. Calculate the equilibrium molarity of HCI. Round your answer to two decimal places. Ом X G
Consider the following reaction. 2 NO, (g) = N,0,(g) When the system is at equilibrium, it contains NO, at a pressure of 0.858 atm, and N,O, at a pressure of 0.0736 atm. The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished? PNO, = 1.716 atm Incorrect PN,0, .1472 %3D atm Incorrect
Can you please answer question 3
Consider the following equilibrium system: 2 NOCI(g) 2 2 NO(g) + Cl2(g) Kc = 57.0 Initially, only NOCI gas is placed in a flask. After equilibrium has been reached it is found that the concentration of the nitrogen monoxide gas in the flask is 1.14 mol/L. What is the initial molar concentration of the NOCI gas? Answer to three decimal places.
Consider the combustion of methane (as represented by the following equation). This is the reaction that occurs for a Bunsen burner, which is a source of heat for chemical reactions in the laboratory. CH 4(9) +20 2(g) =CO2(g) + 2H 20(g) For the system at chemical equilibrium, which of the following explains what happens if the temperature is reduced? O a. The equilibrium position is shifted to the left and the value for K increases. O b. The equilibrium position is shifted to the right and the value for K increases. O c. The equilibrium position is shifted to the right and the value for K decreases. O d. The equilibrium position is shifted but the value for K stays constant. Oe. The equilibrium position is shifted to the left and the value for K decreases.
Can you please answer question 2
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N2(g) + 2H2O(g) 2 NO(g) + 2 H2(g) K=2.x 10 -10 He fills a reaction vessel at this temperature with 6.0 atm of nitrogen gas and 11. atm of water vapor. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of H2, using only the tools available to you within ALEKS? ○ yes x10 O no If you said yes, then enter the equilibrium pressure of H₂ at right. Round your answer to 1 significant digit. atm 5
Consider the following reaction at equilibrium. What effect will removing some SO2 have on the system? SO2(g) + NO2(g) = SO3(g) + NO(g) The pressure of SO3 will increase The equilibrium constant will decrease. No change will occur since SO2 is not included in the equilibrium expression. The pressure of NO2 will increase. The reaction will shift to decrease the pressure.
Consider the following equilibrium If the equilibrium concentration of chlorine and phosphorous trichloride are 0.80 mol/L and 0.70 mol/L, respectively,find the equilibrium concentration of phosphorous pentachloride.

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