At 1000°C, the reaction NO2(3) + SO23) mia NO(g) + SO318) has Ke- 4.57. Suppose 0.160 mol of NO2 and 0.160 mol of SO2 are placed in a 5.00 L container and allowed to react. Record all your answers to three (3) significant figures. What are the following concentrations at equilibrium? INO:) - M (SO2) - [NO] - (SO3) - e Textbook and Media What will the new equilibrium concentrations be if 0.016 mol NO and 0.016 mol SO3 are added to the original equilibrium mixture? (NO2) - M [SO2) = 1 (NO) = (SO3) -

At 1000°C, the reaction NO2(3) + SO23) mia NO(g) + SO318) has Ke- 4.57. Suppose 0.160 mol of NO2 and 0.160 mol of SO2 are placed in a 5.00 L container and allowed to react. Record all your answers to three (3) significant figures. What are the following concentrations at equilibrium? INO:) - M (SO2) - [NO] - (SO3) - e Textbook and Media What will the new equilibrium concentrations be if 0.016 mol NO and 0.016 mol SO3 are added to the original equilibrium mixture? (NO2) - M [SO2) = 1 (NO) = (SO3) -

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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Question 2, part c: please see attached Part a answer: if an initial concentration before equilibrium of c2h4o2 is 0.080 M, what are the equilibrium conc of the three species in the equilibrium: [H3O+]=[C2H3O2-]=1.20x10^-3M Part b answer: a solution in which this reaction takes place is analyzed and found to have [C2H4O2]=0.073M and [C2H3O2-]=0.251M and pH 2.131. Is the system and equilibrium? Calculate Q Qc=2543.0 x 10^-5 Kc=1.81 x 10^-5 not at equilibrium
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-7 At a certain temperature, the equilibrium constant K for the following reaction is 2.25 × 10 ': H,(g) + L(g) =2 HI(g) Use this information to complete the following table. Suppose a 40. L reaction vessel is filled with 0.22 mol of HI. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little H2 and I2. x10 There will be very little HI. ? do O Neither of the above is true. 18 Ar What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 0 K = 2 HI(g) H2(9)+I½(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K = | 3 H,(9)+31,(9) 6 HI(g) Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility
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A student artificially pumped 1 mole of each substance seen below in a piston with a moveable lid (this lid can increase or decrease thereby changing the volume and pressure): 2 C3H7OH (g) + 902 (g) 6 CO2 (g) +8 H2O(g) If the student increased the volume of the piston, how will the reaction shift to reach a new equilibrium? No conclusion can be made since more information is needed The reaction will shift to the left The reaction will shift to the right The reaction will not shift because Q = K
A chem gineer is studying the following reaclon! HCN(aq)+NH,(aq) - CN (aq)+NH,(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.99. The engineer charges ("fills") four reaction vessels with hydrogen cyanide and ammonia, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel compound concentration expected change in concentration HCN 0.84 M O t increase OI decrease O (no change) NH, 1.00 M O t increase O, decrease O (no change) CN 0.42 M O 1 increase O. decrease O (no change) NH, 0.33 M O t increase O, decrease O (no change) HCN 1.01 M O t increase O. decrease O (no change) NH, 1.17 M O t increase O. decrease O (no change) CN 0.25 NM M t increase O. decrease O (no change) NH. 0.16 MM O t increase O.…
Consider the reaction, 2AB2(g) = A2(g) + 2B2(g), Kc = 0.263 at 25°C. The reaction begins with an unknown concentration of AB2 in the reaction flask. At equilibrium, the concentration of AB2 is found to be 0.00545 M. a) Complete the ICEE table below, b) Write the equilibrium expression and equation for this reaction (pay close attention to coefficients!), c) Calculate the equilibrium concentration of both products, and d) Calculate the initial concentration of AB2. You should confirm that your equilibrium concentrations will give the correct equilibrium constant when plugged into the expression. ICEE table I C E 2 AB₂(g) A₂(g) + 2 B₂(g)
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If this reaction is taking place in a 1.0L container, and 1.5 mol of SO2 were added to the reaction, whatwill the new concentrations of all fours gases be when equilibrium is reestablished?