**Title:** Industrial Production of Ethanol**Introduction:**Ethanol (C₂H₅OH), a significant industrial chemical, is generally produced through the reaction between steam and ethylene (C₂H₄), which is derived from oil.**Chemical Reaction:**\[ \text{C}_2\text{H}_4 (g) + \text{H}_2\text{O} (g) \rightleftharpoons \text{C}_2\text{H}_5\text{OH} (g) \]- **ΔH** = (Negative value not specified, indicating an exothermic reaction)- **Kₚ** = 181**Questions:**a. **What is the value of Kₚ at 600 K?**b. **At equilibrium, if the concentration of the product (C₂H₅OH) is 0.987 M and the concentration of water (H₂O) is 0.0562 M, what is the equilibrium concentration of C₂H₄?**(Note: A file attachment feature was mentioned, but specifics were not detailed here)

Answered: Image /qna-images/answer/8a9e4857-b5e4-4a57-bff1-126cba43de82.jpg

An important industrial source of ethanol, C2H5OH, is the reaction of steam with ethylene (C2H4) derived from oil. C2H4 (g) + H20 (g) C2H5OH (g) AH (-) Kp = 181 a. What is the value of K, at 600.K? b. At equilibrium, the concentration of the product, C2H5OH is .987M and the concentration of water is 0.0562M. What is the equilibrium concentration of C2H4? Attach File Browse Local Files

An important industrial source of ethanol, C2H5OH, is the reaction of steam with ethylene (C2H4) derived from oil. C2H4 (g) + H20 (g) C2H5OH (g) AH (-) Kp = 181 a. What is the value of K, at 600.K? b. At equilibrium, the concentration of the product, C2H5OH is .987M and the concentration of water is 0.0562M. What is the equilibrium concentration of C2H4? Attach File Browse Local Files

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

35 Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 3.01 × 10³ at 900 K. If an initial mixture of 0.0216 mol SO2 and 0.0148 mol O2 reacts in a 1.0 L vessel, what will be the concentration of SO3 at equilibrium? 2 SO:(g) + O2(g)= 2 SO:(g) 1 3 NEXT Based on the given values, set up ICE table in order to determine the unknown. 2 SO:(g) O:(g) + 2 SO:(g) Initial (M) 0.0216 0.0148 Change (M) 0.0216 - 2x 0.0148 - x Equilibrium (M) 5 RESET 0.0216 0.0148 1.0 +x +2x -2x 0.0216 + x 0.0216 + 2x 0.0216 - x 0.0216 - 2x 0.0148 + x 0.0148 + 2x 0.0148 - x 0.0148 - 2x
A sample of ammonia gas was allowed to come to equilibrium at 400 K. 2NH3(g) --------> N2(g) + 3H2(g) At equilibrium, it was found that the concentration of H2 was 0.0352 M, the concentration of N2 was 0.0117 M, and the concentration of NH3 was 0.157 M. What is Kc for this equilibrium?
A sample of HI was placed in a container and the following reaction was allowed to come equilibrium. H₂(g) + 1₂(g) = 2 HI(g) The equilibrium concentrations were found to be [HI] = 3.88 M and [H₂] = [1₂] = 0.556. Calculate the equilibrium const Kc, for the reaction. Note Kc is often called K.
An equilibrium reaction has a K = 3.2 x 10-4. What can be said about the reaction? [Reactants] [Products] [Reactants]> [Products] [Reactants] [Products] < =
Consider the equilibrium between SbCl5, SbCl3 and Cl₂. SbCl5(g) SbCl3(g) + Cl₂(g) K = 2.46x10-² at 530 K The reaction is allowed to reach equilibrium in a 7.30-L flask. At equilibrium, [SbCl5] = 0.430 M, [SbCl3] = 0.103 M and [Cl₂] = 0.103 M. (a) The equilibrium mixture is transferred to a 14.6-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 14.6-L flask. [SbCl5] = [SbCl3] = [Cl₂] |||| ΣΣΣ
SC At a certain temperature, the equilibrium constant K for the following reaction is 506.: Br₂(g) + OC1₂(g) BrOCI(g) + BrCl(g) Use this information to complete the following table. Suppose a 46. L reaction vessel is filled with 0.62 mol of Br₂ and 0.62 mol of OCI₂. What can you say about the composition of the mixture in the vessel at equilibrium? ! 1 What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. BrOCI(g)+BrCl(g) Q A What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 Br₂(9)+20C1₂(9) P 2 BrOCI(g)+2BrCl(9) Explanation NO 2 W S Check *3 # E Br₂(9)+OCL₂(9) D D DS 4 C R F % LO 5 O There will be very little Br₂ and OCl₂. O There will be very little BrOCI and BrCl. ONeither of the above is true. K = 0 K = 0 T MacBook Pro 20 ^ 6 G Y C & 7 H 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy C U 00 8 J X I ( 9 K 0 0 < F
Consider the following equilibrium: CO (g) + Br2 (g) = COBr2 (g) K=12.0 at 85C Initially, the concentration of CO is 0.10M and Br2 is 0.40M. What are all the equilibrium concentrations?
The equilibrium constant Kp for the reaction,2 SO3(g) <-------> 2 SO2(g) + O2(g)is 7.880 at 759 °C. If a vessel at this temperature initially contains pure SO3 and if the partial pressure of SO3 at equilibrium is 0.109 atm, what is the partial pressure of O2 in the flask at equilibrium? What was the initial pressure of SO3 in the flask?
12.) A sample of ammonia gas was allowed to come to equilibrium at 400 K.2NH3(g) = N2(g) + 3H2(g) At equilibrium, the mixture contained to following concentrations: [H2] = 0.0283 M, [N2] = 0.00944 M,[NH3] = 0.101 M. What is Kp at this temperature?
Consider the reaction: 2 HI(g) yields H2(g) + I2(g) where K=46.5. In an experiment, 0.5 moles of HI, 0.75 moles of H2 and 0.75 moles of I2 are mixed in a 1 liter flask and allowed to reach equilibrium. The equilibrium concentration of H2 is?
An important industrial source of ethanol, C₂H5OH, is the reaction of steam with ethylene (C2H4) derived from oil. C2H4 (g) + H2O (g) C2H5OH (g) AH (-) Kp = 181 a. What is the value of Kc at 600.K? b. At equilibrium, the concentration of the product, C₂H5OH is .987M and the concentration of water is 0.0562M. What is the equilibrium concentration of C₂H4?
At a certain temperature, the equilibrium constant, K., is 0.00572 for the reaction Cl,(g) = 2 Cl(g) A. If 2.77 g Cl, is placed in a 2.50 L flask at this temperature, what are the equilibrium concentrations of Cl, and Cl? [CI,] = M [CI] = M B. Following the establishment of equilibrium in part A, the volume of the flask is suddenly increased to 5.00 L while the temperature is held constant. What are the new equilibrium concentrations of Cl, and Cl? [Cl,] = M [CI] = M C. Following the establishment of equilibrium in part A, the volume of the flask is instead suddenly decreased to 1.0 L while the temperature is held constant. What are the new equilibrium concentrations of Cl, and CI? [Cl,] = M [CI] = M