Aluminum metal and bromine liquid (red) react violently to make aluminum bromide (white powder). One way to represent this equilibrium is: 2 Al(s) +3 Br2(1) 2 AIBR3(s) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) Al(s) + 3/2 Br2) AIBr3(s) K, %3D 2) 2 AIBr3(s) =2 Al(s) + 3 Br2(1) K, = 3) AIB33(s) e Al(s) + 3/2 Br2(1) K3 =

Aluminum metal and bromine liquid (red) react violently to make aluminum bromide (white powder). One way to represent this equilibrium is: 2 Al(s) +3 Br2(1) 2 AIBR3(s) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) Al(s) + 3/2 Br2) AIBr3(s) K, %3D 2) 2 AIBr3(s) =2 Al(s) + 3 Br2(1) K, = 3) AIB33(s) e Al(s) + 3/2 Br2(1) K3 =

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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Aluminum metal and bromine liquid (red) react violently to make aluminum bromide (white powder). One way to represent this equilibrium is: 2 Al(s) + 3 Br2(1)=2 AIBR3(s) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) 2 AIBR3(s) =2 Al(s) + 3 Br2(1) K1 = 2) Al(s) + 3/2 Br2(1)=AIBR3(s) 3) AIBR3(s) K2 = 2 Al(s) + 3/2 Br2(1) K3 = Drag and drop your selection from the following list to complete the answer: 1/K (1/K)12 K12
Consider the following fictional reaction: 2AB(aq) = 2A(aq) + B2(aq) K = 9.8 x 101 %3D If you start out with a 5.0 M solution of AB, A, and B2, what is the concentration of each species when the reaction reaches equilibrium. when solving this problem (more specifically, you are not allowed to put the algebra equation in your calculator to solve for x)
A student ran the following reaction in the laboratory at 316 K:2CH2Cl2(g) CH4(g) + CCl4(g)When he introduced CH2Cl2(g) at a pressure of 0.487 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of CCl4(g) to be 0.219 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction.
Dinitrogen tetraoxide, a colorless gas, exists in equilibrium with nitrogen dioxide, a reddish brown gas. One way to represent this equilibrium is: N₂04(g) 2NO₂(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1) NO₂(g) 1/2 N₂O4(g) K₁ 2) 1/2 N₂O4(9) NO₂(g) 3) 2NO₂(g) N₂O4(9) Drag and drop your selection from the following list to complete the answer: K¹/2 (1/K)¹/2 = = K₂ K3 = 1/K
Dinitrogen tetraoxide, a colorless gas, exists in equilibrium with nitrogen dioxide, a reddish brown gas. One way to represent this equilibrium is: 2NO2(g)N,04(g) We could also write this reaction three other ways, listed below. The equilibrium constants for all of the reactions are related. Write the equilibrium constant for each new reaction in terms of K, the equilibrium constant for the reaction above. 1/2 K1 1) N,O4(2) (5)-ON = K2 1/2 2) NO2(g) N204(g) K3 3) N204(g) = 2NO2(g) Drag and drop your selection from the following list to complete the answer: (1К)12 K12 1/K
A student ran the following reaction in the laboratory at 682 K:2HI(g) H2(g) + I2(g)When she introduced HI(g) at a pressure of 5.24 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of HI(g) to be 4.15 atm.Calculate the equilibrium constant, Kp, she obtained for this reaction.Kp =
A student ran the following reaction in the laboratory at 697 K:2HI(g) H2(g) + I2(g)When he introduced HI(g) at a pressure of 4.46 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of HI(g) to be 3.52 atm.Calculate the equilibrium constant, Kp, he obtained for this reaction.Kp =
3 H2(g) + N2 (g) the equilibrium For the reaction 2NH3(g) ---- 3H2(g) +N2(g) 2 NH 3 (g) - concentrations were found to be [NH3] = 0.250 M, [H2] = 0.330 M and [N2] = 0.750 M. What is the equilibrium constant for this reaction?
At a particular temperature, the equilibrium amounts of hydrogen, iodine and hydrogen iodide present in a 4.00 L flask are found to be: 0.25 moles of hydrogen gas, 0.15 moles of iodine gas and 1.37 moles of hydrogen iodide gas. H2(g) + I2(g) ↔ 2 HI(g) Calculate the equilibrium constant, Kc, value for the reaction.
The reaction listed below is currently at equilibrium. If you were to suddenly halve the volume of the reaction chamber, what effect would that have on the system? Kr (g) + 2 F2 (3) = KrF4 (s) The reaction will shift to the left in the direction of reactants. O Cannot be determined - The equilibrium concentrations of all species must be provided. The reaction will shift to the right in the direction of products. O The equilibrium constant will increase. O The equilibrium constant will decrease.
2 A reaction quotient, Q, is calculated to be 3.2 x 10. The equilibrium constant for the same reaction is 5.4 x 10³. Which statement is correct? a The system is at equilibrium. b The concentrations of the products are greater than their concentrations at equilibrium. The system will attain equilibrium by moving to the right. The system will attain equilibrium by moving to the left. More information is needed to determine which statement is correct. C d e
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 NO(g) + Cl₂(g) = 2 NOC1 (g) K₁₂=4.×100 He fills a reaction vessel at this temperature with 8.0 atm of nitrogen monoxide gas and 7.5 atm of chlorine gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NOC1, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NOC1 at right. Round your answer to 1 significant digit. O yes O no 0 atm X