Deriving concentrations from dataIn Part A, you were given the equilibrium pressures, which could be plugged directly into the formula for K. In Part B however, you will be given initialconcentrations and only one equilibrium concentration. You must use this data to find all three equilibrium concentrations before you can apply the formula for K.Part BThe following reaction was performed in a sealed vessel at 734 °C :H2 (g) + I2(g) = 2HI(g)Initially, only H, and I2 were present at concentrations of [H2] = 3.65 M and [I2] = 2.75M. The equilibrium concentration of I, is 0.0600 M. What is theequilibrium constant, Ke, for the reaction at this temperature?Express your answer numerically.> View Availlable Hint(s)?Ke =SubmitNext>ovide FeedbackMacBook Air

Given: Initial concentration of H2 = 3.65 M Initial concentration of I2 = 2.75 M Equilibrium…

Answered: The following reaction was performed in…

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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Booking.com: Chea.. TripAdvisor Facebook [References] The reaction 2 NO2(s) N20.(g) has an equilibrium constant, K. of 170 at 25 °C. If 4.5 x 10 mol of NO2 is present in 10.-L flask along with 3.5 x 10 mol of N204, is the system at equilibrium? If it is not at equilibrium, does the concentration of NO2 increase or decrease as the system proceeds to equilibrium? The system is V. The concentration of NO2 will Vas the system proceeds to equilibrium. Submit Answer Try Another Version 2 Item attempts remalning Previous Email Instructor Save and Exit ment Ceneare Learning Ceneae A
Nickel and carbon monoxide react to form nickel carbonyl, like this: Ni(s)+4 CO(g)→Ni(CO),(9) At a certain temperature, a chemist finds that a 3.4 L reaction vessel containing a mixture of nickel, carbon monoxide, and nickel carbonyl at equilibrium has the following composition: compound amount Ni 88.8 g CO 1.63 g Ni(CO), 0.813 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 %3D Check Explanation Privacy Accessibility 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use MacBook Air
A 2.50 mole quantity of NOCl was initially in a 1.50 L reaction chamber at 400°C. After equilibrium was established, it was found that 32.0 percent of the NOCl had dissociated: 2NOCl(g) 2NO(g) + Cl2(g) Calculate the equilibrium constant Kc for the reaction.
A 2.20 mole quantity of NOCl was initially in a 1.50 L reaction chamber at 400°C. After equilibrium was established, it was found that 32.0 percent of the NOCl had dissociated: 2NOCl(g) 2NO(g) + Cl2(g) Calculate the equilibrium constant Kc for the reaction.
At 15 degrees Celcius, the following concentrations were found for the gases in an equilibrium mixture for the reaction N2O(g) + NO2 (g) <-----> 3NO (g) (NO2) = 0.42 M (NO) = 4.1 X 10^-8 M N2O = 0.022 M
Consider the equilibrium reaction. 3A +B= 2C After multiplying the reaction by a factor of 2, what is the new equilibrium equation? new equilibrium equation: 6A + 2B = 4C Create the equilibrium-constant expression, K, for the new equilibrium reaction. Answer Bank IAP Ke = [B) [B) LA Answer Bank [C] [AP K = [B] (B] [B] (A) If the initial reaction contains 1.79 M A, 1.53 M B, and 2.39 M C, calculate K, for the new equilibrium reaction. K = Incorrect
The equilibrium constant, K,, for the following reaction is 0.636 at 600 K: COCl,(E) CO(g) + Cl(g) Calculate the equilibrium partial pressures of all species when COC1,(g) is introduced into an evacuated flask at a pressure of 1.33 atm at 600 K. Рсос, - atm Рсо atm atm
2. Please don't write on a paper. I can't understand handwritten.
For the following reaction at a certain temperature H2(g) + F2(g) = 2HF(g) the equilibrium concentrations in a 10.00-L rigid container are [H2] = 0.0600 M, [F2] = 0.0200 M, and [HF] = 0.620 M. If 0.220 moles of F2 is added to the equilibrium mixture, calculate the concentration of H2 after equilibrium is reestablished.
A student ran the following reaction in the laboratory at 1080 K: 2SO3(g) 2S02(g) + O₂(g) When he introduced SO3(g) at a pressure of 0.886 atm Into a 1.00 L evacuated container, he found the equilibrium partial pressure of SO3(g) to be 0.340 atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = Submit Answer 44 $ T R F V/ % 5 Retry Entire Group 9 more group attempts remaining T Cengage Learning Cengage Technical Support F5 G ^ 6 MacBook Air Y H & 7 RN U * 0 J ► 11 F8 M ( 9 ►► K F9 O 1 F11 + { Save and Exit = F12 11
A sample of HI was placed in a container and the following reaction was allowed to come equilibrium. H₂(g) + 1₂(g) = 2 HI(g) The equilibrium concentrations were found to be [HI] = 3.88 M and [H₂] = [1₂] = 0.556. Calculate the equilibrium const Kc, for the reaction. Note Kc is often called K.
Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 3.0 L reaction vessel contained a mixture of 1.37 x 10-2 M HI, 6.47 × 10-3 M H2, and 5.94 × 10-4 M I, at 740 K. What are the values of Kc and Kp for the reaction at this temperature? H2(g) + 12(g) = 2 HI(g) 1 NEXT > Based on the given data, set up the expression for Kc and then evaluate it. Do not combine or simplify terms. K. = 2 RESET [1.37 x 10-2] [6.47 x 10-3] [5.94 × 10-4] [4.57 × 10-3] [2.16 х 10-3] [2.31 x 10-4] 2[1.37 x 10-2] 2[6.47 x 10-3] 2[5.94 x 10-4] [1.37 х 10-7)2 [6.47 x 10-312 [5.94 x 10-4]2 3.56 x 103 2.81 × 10-4 48.8 2.05 x 10-2

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