The equation below represents the reaction between nitrogen gas and hydrogen gas to form ammonia. The reaction occurs within a closed container and comes to equilibrium: N, + 3H, 2 2NH, What expression represents the equilibrium expression for this reaction? [NH,7 A K. [N,TH,] [N,TH,] [NH,] B Keg = [N,TH,] Keg [NH,] [N,][H,] [NH,1 ASED D eq

The equation below represents the reaction between nitrogen gas and hydrogen gas to form ammonia. The reaction occurs within a closed container and comes to equilibrium: N, + 3H, 2 2NH, What expression represents the equilibrium expression for this reaction? [NH,7 A K. [N,TH,] [N,TH,] [NH,] B Keg = [N,TH,] Keg [NH,] [N,][H,] [NH,1 ASED D eq

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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Suppose a 250. mL flask is filled with 0.90 mol of N, and 1.2 mol of NH2. This reaction becomes possible: ME N,(g) +3H,(g) – 2NH, (g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N,. You can leave out the M symbol for molarity. H, NH, initial change equilibrium Continue Submit As O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center 43,203 FEB 19 CH.9 PE ASSESS MacBook Air D00 FI0 吕口 F3 F9 esc F5 F7 F2 ロ口 X
00 II O KINETICS AND EQUILIBRIUM Using the van't Hoff equation to predict K at a different... At -18.7 °C the pressure equilibrium constant K, =7.2 for a certain reaction. d. Here are some facts about the reaction: -1 -1 • The initial rate of the reaction is 13. mol·L s . • Some of the reactants are liquids and solids. • If the reaction is run at constant pressure, 79.0 kJ/mol of heat are absorbed. O Yes. x10 Using these facts, can you calculate K, at -5.6 °C? No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Yes, and K. will be d. bigger. If you said no, can you at least decide whether K, at Yes, and K, will be d. smaller. - 5.6 °C will be bigger or smaller than K, at – 18.7 °C? No. Explanation Check Terms of Use I Privacy Center A O 2021 McGraw Hill LLC. All Rights Reserved. DD F10 O00 F5 F4 esc F1 24 41 %23 6 7. 3.
Methanol and oxygen react to form carbon dioxide and water, like this: 2 CH,OH(I)+30,(g)-2 Co,(g)+4H,0(g) At a certain temperature, a chemist finds that a 6.3 L reaction vessel containing a mixture of methanol, oxygen, carbon dioxide, and water at equilibrium has the following composition: olo Ar compound amount CH;OH 2.06 g O2 2.63 g CO2 3.06 g H,O 4.20 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0
A given amount of HI is placed inside a reaction vessel and is allowed to reach the equilibrium. The following concentrations are measured at the equilibrium: [HI] = 0.60 M, [H2] = 0.20 M, [I2] = 0.55 M. What is the value of Keq for this reaction?
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 50 L tank with 3.5 mol of carbon monoxide gas and 14. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 1.4 mol of carbon monoxide gas, 11.9 mol of water vapor and 2.1 mol of hydrogen gas. The engineer then adds another 0.90 mol of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the moles of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. mol
O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 2.0 mol of NO, and 1.3 mol of NO. The following reaction becomes possible: NO, (g) + NO(g) → 2NO, (g) The equilibrium constant K for this reaction is 6.91 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. Explanation Check 02022 McGraw Hill LLC. All Rights Reserved. Terms of Use |P 21
At a certain temperature, the equilibrium constant, ?c, for this reaction is 53.3. H2(g)+I2(g)↽−−⇀2HI(g)?c=53.3 At this temperature, 0.400 mol H2 and 0.400 mol I2 were placed in a 1.00 L container to react. What concentration of HI is present at equilibrium? [HI]= M At a certain temperature, the equilibrium constant for the chemical reaction shown is 1.13×10−3. At equilibrium, the concentration of AB is 2.725 M, the concentration of BC is 2.225 M, and the concentration of AC is 0.220 M. Calculate the concentration of B at equilibrium. AB(aq)+BC(aq)↽−−⇀AC(aq)+2B(aq) [B]= M
Consider the reaction. NaC2O2H3(s) <--- H2O ------> NaC2O2H3(aq), which is at equilibrium in an open flask in the lab at room temperature. You add more water to the equilibrium mixture. When the system reestablishes equilibrium, what has changed? a. the concentration of NaC2H3O2(aq) does not change b. heat is produced c. the concentration of NaC2H3O2(aq) decreases d. the concentration of the water increases
. Consider the equilibrium 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H₂O(g). Predict the effect on the equilibrium concentration by the addition of N₂. A The equilibrium will shift to produce more nitrogen. B The equilibrium will shift to produce more reactants. C The equilibrium will shift to produce more products. D The reaction is already at equilibrium. E None of the above Given: 2P(g) + 3Cl2(g) → 2PC13(g) K Calculate the equilibrium constant for the following reaction. P(g) + 3/2Cl2(g) → PCI(g) AK BK¹ C 2K D 0.5K EK¹/2
Consider the equilibrium system described by the chemical reaction below. For this reaction, Kc = 2.4 x 103 at a particular temperature. If the equilibrium concentrations of H,0 and H, are 0.11 M and 0.019 M, respectively, determine the concentration of O, at equilibrium.. 2 2 H,O(g) = 2 H,(g) + 0,(g) 2 NEXT > If [x] represents the equilibrium concentration of O, set up the equilibrium expression for Kc to solve for the concentration. Do not combine or simplify terms.. 2' K. = = 2.4 x 103 5 RESET [О.11] [0.019] 2[0.11] 2[0.019] [0.11]? [0.019]? [x] [x]? [2x] [2x]?
Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction below is K = 6.0 x 10-2, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 104M. N2(g) + 3H2(g) = 2NH3(g) 3. BI U T O Word(s) 4. If the concentration of the reactant H2 was decreased from 1.0 x 10-² M to 2.7 x 10-4 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. BI U T O Word(s)