Consider the following equilibrium. A + 2B C + 4D If the change in concentration for C is 0.640 M, what will be the corresponding change in concentration (in units of molarity) for D? • Round the answer to three significant figures. Provide your answer below:

MOving to anotrie question will save this response. Question 7 A state of dynamic equilibrium, Ag2CO3(s) +→ 2Ag*(aq) + CO32(aqg), exists in solutida. Which direction will the equilibrium shift if Ca(NO3)2(aq) is added to the system? O To the left. O To the right. O It will not shift left or right. A Moving to another question will save this response. MacBook Pro 80 888 FS F6 F7 FA esc F2 %23 2$ 8. 2 3 4. Q K A D 5

Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO₂(9)+H₂O(1)→2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 4.4 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO₂ 10.6 g H₂O 138.4 g HNO3 21.8 g NO 19.6 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. с K = [] x10 ×

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Consider the equilibrium system described by the chemical reaction below. Determine the concentration of O, at equilibrium by writing the equilibrium constant expression and solving it. Complete Parts 1-2 before submitting your answer. = 2 H₂O(g) 2 H2(g) + O̟₂(g) 1 2 NEXT At this temperature, the Kc = 2.4 × 103 and the equilibrium concentrations of H2O and H2 are 0.11 M and 0.019 M, respectively. If [x] represents the equilibrium concentration of O2, set up the equilibrium expression for Kc to solve for the concentration. Each reaction participant must be represented by one tile. Do not combine terms. Кс = 2' = 2.4 × 103 > RESET [0.11] [0.019] 2[0.11] 2[0.019] [0.11]² [0.019]² [x] [x]² [2x] [2x]²

O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 1.9 mol of NO,, 0.10 mol of N0 and 1.7 mol of CO,. The following reaction becomes possible: 2' NO,(g)+CO(g) -NO(g)+CO,(g The equilibrium constant K for this reaction is 4.70 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M TRADIS Explanation Check 2020 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy | Acces NOV 242 PAGES étv 4 MacBook Air II

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N₂(g) + 2 H₂O(g) 2 H₂(g) + 2NO(g) = -9 K₂=3.x 107 He fills a reaction vessel at this temperature with 15. atm of nitrogen gas and 7.8 atm of water vapor. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NO, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NO at right. Round your answer to 1 significant digit. O yes O no 0 atm 0 10 X