Suppose a 500. mL flask is filled with 1.6 mol of I, and 1.0 mol of HI. The following reaction becomes possible:H,(g)+L,(g) – 2HI(g)The equilibrium constant K for this reaction is 0.452 at the temperature of the flask.Calculate the equilibrium molarity of I,. Round your answer to two decimal places.MExplanationCheckO2022 McGraw Hill LLC. All Rights Reserved. Mercury(II) oxide decomposes to form mercury and oxygen, like this:2 HgO(s)→2 Hg(l1)+O,(g)At a certain temperature, a chemist finds that a 8.6 L reaction vessel containing a mixture of mercury(II) oxide, mercury, and oxygen at equilibrium has thefollowing composition:compound amountHgO20.3 gHg10.1 gO220.3 gCalculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.K_ = Dx10CCheckExplanation2022 McGraw Hill LLC. AIl Rights Reserved. Terms of Use Privacy Center AccessibilityMacBook Proesc

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Jupp0se a J00. IL IldSk IS filled with 1.6 mol of I, and 1.0 mol of HI. The following reacti H, (g) +I,(g) – 2HI(g) The equilibrium constant K for this reaction is 0.452 at the temperature of the flask. Calculate the equilibrium molarity of I,. Round your answer to two decimal places. OM

Jupp0se a J00. IL IldSk IS filled with 1.6 mol of I, and 1.0 mol of HI. The following reacti H, (g) +I,(g) – 2HI(g) The equilibrium constant K for this reaction is 0.452 at the temperature of the flask. Calculate the equilibrium molarity of I,. Round your answer to two decimal places. OM

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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|For the equilibrium system H2 (g) + CO2 (g) H2O (g) + CO (g), predict the effect that the indicated stress will have on the specified quantity. a) The effect of adding CO on [H2] b) The effect of adding CO2 on [H2] c) The effect of increasing the volume on amount of H2 (g) Do any of the stresses affect the value of K?
Consider the following equilibrium: N,0, )-2NO, () AG-S4 J Now suppose a reaction vessel is filled with 7.35 atm of dinitrogen tetroxide (N,o) at 374. C. Answer the following questions about this system: Under these conditions, will the pressure of N,0, tend to rise er fal? rise O fall Is it possible to reverse this tendency by adding NO,? In other words, if you said the presture of N,O, will tend to rise, can that be changed to a tendency to fall by adding NO, Similarly, if you said the yes pressure of N,O, will tend to fal, can that be changed to a tendency to no e by adding NO,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO, needed to reverse it 0- Round your answer to 2 signficant digits
Consider the following system at equilibrium where AH° = -108 kJ, and K. = 77.5, at 600 K. CO(g) + Cl2(g) COC,(g) When 0.27 moles of Cl(g) are removed from the equilibrium system at constant temperature: The value of K. The value of Q. |K. The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. Oremain the same. It is already at equilibrium. The concentration of CO will increase. decrease. remain the same. Submit Answer Retry more group attempts remain
Suppose a 500. mL flask is filled with 1.2 mol of H, and 1.6 mol of I,. The following reaction becomes possible: H2 (g)+ I½ (g) – 2HI (g) The equilibrium constant K for this reaction is 9.90 at the temperature of the flask. Calculate the equilibrium molarity of I,. Round your answer to two decimal places. M
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 30, (g) = 20, (g) K, = 4. × 10-6 He fills a reaction vessel at this temperature with 9.0 atm of oxygen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of O3, using only the tools Oyes available to you within ALEKS? O no O atm If you said yes, then enter the equilibrium pressure of O, at right. Round your answer to 1 significant digit.
Consider the following system at equilibrium where AH° = 16.1 k), and Ke = 6.50×103, at 298 K. 2NOBr(g) =2N0(g) + Br2(g) When 0.34 moles of NO(g) are added to the equilibrium system at constant temperature: The value of Kel The value of Qc( | Kc. The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. remain the same. It is already at equilibrium. The concentration of Br2 will|
Suppose a 500. mL flask is filled with 0.80 mol of NO, and 1.8 mol of NO,. The following reaction becomes possible: NO,(g) + NO(g) - 2NO,(g) The equilibrium constant K for this reaction is 4.18 at the te perature of the flask. Calculate the equilibrium molarity of NO,. Round your answer to two decimal places. Fducation AR Rights Re
Suppose a 500. mL flask is filled with 1.6 mol of N, and 0.10 mol of O,. The following reaction becomes possible: N,(g) +0,(g) 2NO(g) The equilibrium constant K for this reaction is 2.74 at the temperature of the flask. Calculate the equilibrium molarity of N,. Round your answer to two decimal places. 2:
At a certain temperature, 0.347 mol CH, and 0.619 mol H,S are placed in a 2.50 L container. CH,(g) + 2 H, S(g)= CS, (g) + 4 H,(g) At equilibrium, 11.8 g CS, is present. Calculate K.. K. =
O KINETICS AND EQUILIBRIUM 1/5 Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 1.1 mol of Cl,, 0.20 mol of HCl and 0.80 mol of CCl,. The following reaction becomes possible: Cl,(g) +CHCI, (g) = HCl(g)+CCl, (g) The equilibrium constant K for this reaction is 9.65 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. | M II
Calculating equilibrium composition from an equilibrium... 0/5 Suppose 500. mL flask is filled with 1.9 mol of H, and o0.50 mol of C1,. The following reaction becomes possible: H, (g) + Cl,(g) – 2HC1(g) The equilibrium constant K for this reaction is 3.61 at the temperature of the flask. Calculate the equilibrium molarity of H,. Round your answer to two decimal places. OM