**Experiment: Determining the Equilibrium Constant (Kc) for the Reaction \( \text{CO(g)} + \text{Cl}_2\text{(g)} \rightleftharpoons \text{COCl}_2\text{(g)} \) at 566 K****Introduction:**In this experiment, a student investigated the reaction between carbon monoxide (CO) and chlorine gas (Cl₂) to form phosgene (COCl₂) in the laboratory at a temperature of 566 K.**Chemical Equation:**\[ \text{CO(g)} + \text{Cl}_2\text{(g)} \rightleftharpoons \text{COCl}_2\text{(g)} \]**Initial Conditions:**- **CO(g):** 0.655 moles- **Cl₂(g):** 0.680 moles- Volume of container: 1.00 liter**Equilibrium Concentration:**- **COCl₂(g):** 0.618 M**Calculation Objective:**Determine the equilibrium constant, \( K_c \), for the reaction.**Detailed Procedure:**1. **Establish Initial and Equilibrium Concentrations:** - Initial concentration of CO(g) = \(\frac{0.655 moles}{1.00 L} = 0.655 M\) - Initial concentration of Cl₂(g) = \(\frac{0.680 moles}{1.00 L} = 0.680 M\) - Equilibrium concentration of COCl₂(g) = 0.618 M2. **Calculate Change in Concentration:** The stoichiometry of the reaction informs us that the change in concentration of COCl₂(g) will be equivalent to the change in concentration for both CO(g) and Cl₂(g), but in the opposite direction. Let \( x \) represent the change in concentration for CO(g) and Cl₂(g): - \([ \text{COCl}_2]\) gained = +x - \([ \text{CO]}\) lost = -x - \([ \text{Cl}_2]\) lost = -x Since 0.618 M of COCl₂ is formed: \[ x = 0.618 M \] Therefore: - Change in CO

Answered: Image /qna-images/answer/aaca0561-1da3-41e3-985d-5f8408258d92.jpg

A student ran the following reaction in the laboratory at 566 K: CO(g) + Cl2(g) = COC2(g) When she introduced 0.655 moles of CO(g) and 0.680 moles of Cl,(g) into a 1.00 liter container, she found the equilibrium concentration of COCI,(g) to be 0.618 M. Calculate the equilibrium constant, K, she obtained for this reaction. Kc

A student ran the following reaction in the laboratory at 566 K: CO(g) + Cl2(g) = COC2(g) When she introduced 0.655 moles of CO(g) and 0.680 moles of Cl,(g) into a 1.00 liter container, she found the equilibrium concentration of COCI,(g) to be 0.618 M. Calculate the equilibrium constant, K, she obtained for this reaction. Kc

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...

See similar textbooks

Similar questions

At 500 °C, hydrogen iodide decomposes according to 2 HI(g) = H,(g) + I,(g) For HI(g) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: = 0.402 M, [I,] = 0.402 M, and [HI] [H,] what are the equilibrium concentrations after the new equilibrium has been reached? = 3.40 M. If an additional 1.00 mol of HI(g) is introduced into the reaction vessel, [HI] = M [H,] M M Quection Sourco McO.uarrie Deck AndCallegly d ConoraLChomcitru Dublichen Uni,versi
The equilibrium constant, K. for the following reaction is 1.20×10-2 at 500 K. PCI3(g)=PCl3(g) + Cl½(2) Calculate the equilibrium concentrations of reactant and products when 0.307 moles of PCI3(g) are introduced into a 1.00 L vessel at 500 K. [PCI3] = M [PC13] =| M [Cl2] M
Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI, (g) + Cl, (g) K. 1.80 at 250 °C A 0.2950 mol sample of PCl, (g) is injected into an empty 4.75 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PCl, (g) at equilibrium. [PCl,] = M [PCI,] = M
A student ran the following reaction in the laboratory at 326 K: 2CH,Cl»(g)=CH,(g) + CCl,(g) When she introduced CH,Cl,(g) at a pressure of 0.468 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of CL(E) to be 0.20s atm. Calculate the equilibrium constant, Kp. she obtained for this reaction. Kp=|
The equilibrium constant, Ke, for the following reaction is 7.00 x 105 at 673 K NH,I(s) NH₂ (9) + HI(g) If an equilibrium mixture of the three compounds in a 4.46 L container at 673 K contains 2.50 mol of NHI(s) and 0.411 mol of NH3, the number of moles of HI mol. present is
Nitrosyl chloride, NOCI, decomposes to NO and Cl, at high temperatures: 2NOCI(g) -> 2NO(g) + Cl2(g) Suppose you place 2.00 mol NOCI in a 1.00-L flask and raise the temperature to 462°C. When equilibrium has been established, 0.66 mol NO is present. Calculate the equilibrium constant Kc for the decomposition reaction from these data.
The equilibrium constant, K, for the following reaction is 83.3 at 500 K. PCI,(2) + Cl,(g)=PCI<(g) Calculate the equilibrium concentrations of reactant and products when 0.352 moles of PCl, and 0.352 moles of Cl, are introduced into a 1.00 L vessel at 500 K. [PCI,] =[ M [C)] M [PC!g] = [ M
A student ran the following reaction in the laboratory at 322 K: 2NO(g) + Br2(g) = 2NOB1(g) When she introduced 0.107 moles of NO(g) and 9.86×102 moles of Br2(g) into a 1.00 liter container, she found the equilibrium concentration of NOBR(g) to be 7.65x102 M. Calculate the equilibrium constant, K, she obtained for this reaction. K. =
A student ran the following reaction in the laboratory at 637 K: 2HI(g) H2(g) + I2(g) When she introduced 0.390 moles of HI(g) into a 1.00 liter container, she found the equilibrium concentration of HI(g) to be 0.313 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. K. =
Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI, (g) + Cl, (g) K. 1.80 at 250 °C A 0.1952 mol sample of PCl, (g) is injected into an empty 2.15 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PCl, (g) at equilibrium. [PCI,] = M [PCI,] = M
A chemical engineer is studying the following reaction: 2 NO(g)+2H,(9) - N2(9)+2H,0(g) At the temperature the engineer picks, the equilibrium constant K, for this reaction is 2.0. The engineer charges ("fills") four reaction vessels with nitrogen monoxide and hydrogen, 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 compound pressure expected change in pressure vessel ΝΟ 6.78 atm O f increase Ot decrease O (no change) H, 2.93 atm ↑ increase OI decrease O (no change) A N2 5.23 atm f increase I decrease (no change) H, O 7.24 atm t increase I decrease (no change) NO 5.29 atm f increase I decrease (no change) H, 1.44 atm f increase OI decrease (no change) В N2 5.98 atm increase I decrease (no change) H, O 8.73 atm f increase O I decrease O (no change)…
The equilibrium constant for the reaction shown below is 61.2 H, (g) + Br, (g) = 2HB1(g) Write an expression for the equilibrium constant, K What is the equilibrium concentration of Br2, if [HBr]=0.48 M and [H2] = 0.26 M at equilibrium?