3. A sealed vessel contains 0.25 M COC12, 0.11 M CO, and 0.11 M Cl, at 668 K, which is an equilibrium mixture at this temperature. COCI2(g) = CO(g) + Cl2(g) a. When the temperature is increased and equilibrium is re-established, [CoCl2] = 0.18 M. Is the reaction endothermic or exothermic? How do you know? b. To the equilibrium mixture at 668 K, 0.25 M CO is added. Calculate the concentration of each gas at equilibrium.
3. A sealed vessel contains 0.25 M COC12, 0.11 M CO, and 0.11 M Cl, at 668 K, which is an equilibrium mixture at this temperature. COCI2(g) = CO(g) + Cl2(g) a. When the temperature is increased and equilibrium is re-established, [CoCl2] = 0.18 M. Is the reaction endothermic or exothermic? How do you know? b. To the equilibrium mixture at 668 K, 0.25 M CO is added. Calculate the concentration of each gas at equilibrium.
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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Please help with 3a and 3b
![**3.** A sealed vessel contains 0.25 M COCl₂, 0.11 M CO, and 0.11 M Cl₂ at 668 K, which is an equilibrium mixture at this temperature.
\[ \text{COCl}_2(g) \rightleftharpoons \text{CO}(g) + \text{Cl}_2(g) \]
a. When the temperature is increased and equilibrium is re-established, \([ \text{COCl}_2 ] = 0.18 \, \text{M}\). Is the reaction endothermic or exothermic? How do you know?
b. To the equilibrium mixture at 668 K, 0.25 M CO is added. Calculate the concentration of each gas at equilibrium.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4def24a8-7444-40ec-98ab-79f3007e3ea4%2F15a5a316-96d0-4fe3-8039-4c909bf14184%2F7zoz1o_processed.png&w=3840&q=75)
Transcribed Image Text:**3.** A sealed vessel contains 0.25 M COCl₂, 0.11 M CO, and 0.11 M Cl₂ at 668 K, which is an equilibrium mixture at this temperature.
\[ \text{COCl}_2(g) \rightleftharpoons \text{CO}(g) + \text{Cl}_2(g) \]
a. When the temperature is increased and equilibrium is re-established, \([ \text{COCl}_2 ] = 0.18 \, \text{M}\). Is the reaction endothermic or exothermic? How do you know?
b. To the equilibrium mixture at 668 K, 0.25 M CO is added. Calculate the concentration of each gas at equilibrium.
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![em1.png Part 3: Q9 Average absorbance Flask 8 Flask 9 Flask 10 1:1 Ratio so, Flask 11 Part 3: Q Flask 8 Flask 9 Flask 10 Flask 11 Part 3: Q10 Flask 8 Flask 9 Flask 10 Flask 11 Part 3 0.146 0.166 [Fe] -0.002mol/L 0.215 0.294 [FESCN³mol/L) 4.59% 10 5.18*10* 6.64*10* 9.08*10* [FXmol/L) 5.00 *10* 5.00*10* Y=3362x-0.0083 R² = 0.9993 5.00*10* 5.00*10* (Amounts of flask 8 (9 - 11's values are in the spreadsheet) 71% volume 5.00mL Molarity of Fe(NO3))3 = 0.2M Volume of Fe(NO3))3 = 5.00mL Moles of Fe³= Molarity x volume(L) Moles of Fe¹ = 0.2M X 0.005L = 1x10-³mole x [SCN][mol/ 4x10 5×10-4 7x10 1×10 1 Concentration of Fe³ = mole of Fe³ Volume mole of Fe³1x10³ mole G.O05L 8, Average absorbance for solution 8 (same for 9 - 11) Average absorbance for flask 8 = sum of all absorbances / number of readings (0.145 +0.147 +0.148) 3 Using equation of calibration curve's line(slope) of best fit, the average absorbances of the unknown concentrations to determine [FeSCN-Jat equilibrium in solution 8:…](/questions-and-answers/em1.png-...-part-3-q-average-absorbance-flask-and-11-ratio-so-flash-d-flask-10-flask-11-part-3-q-fla/c9657571-599f-4ed4-a5e6-fabcbd26b888){kind=link}
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