At -8.15 °C the pressure equilibrium constant K, =3.8 for a certain reaction.d.Here are some facts about the reaction:• If the reaction is run at constant pressure, the volume increases by 14.%.-1.- 1• The constant pressure molar heat capacity C = 2.98 J•mol 'K '.d.• The reaction is exothermic.O Yes.x10Using these facts, can you calculate K, at 5.3 °C?O No.If you said yes, then enter your answer at right. Round it to2 significant digits.Yes, and K,will bebigger.If you said no, can you at least decide whether K,atYes, and K,will be5.3 °C will be bigger or smaller than K, at -8.15 °C?smaller.рNo.

We could have used the Van't Hoff isotherm equation to predict the Kp of the reaction at different…

At -8.15 °C the pressure equilibrium constant K, =3.8 for a certain reaction. Here are some facts about the reaction: • If the reaction is run at constant pressure, the volume increases by 14.%. 1 • The constant pressure molar heat capacity C = 2.98 J•mol. K'. • The reaction is exothermic. O Yes. Using these facts, can you calculate K, at 5.3 °C? O No. ? If you said yes, then enter your answer at right. Round it to 2 significant digits,

At -8.15 °C the pressure equilibrium constant K, =3.8 for a certain reaction. Here are some facts about the reaction: • If the reaction is run at constant pressure, the volume increases by 14.%. 1 • The constant pressure molar heat capacity C = 2.98 J•mol. K'. • The reaction is exothermic. O Yes. Using these facts, can you calculate K, at 5.3 °C? O No. ? If you said yes, then enter your answer at right. Round it to 2 significant digits,

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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For the system, 2 NO2(g) --> N2O4(g), ?Grxn° = 17.3 kJ/mol at 1000 K. If the system was initialized using enough NO2 to create a partial pressure of 0.750 atm and enough N2O4 to create partial pressure of 0.450 atm, calculate the value of ?G in kJ/mol at this temperature using these initial values after chemical equilibrium is established. Report answer to nearest whole number.
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Phosphoryl chloride, POCl3(g), is used in the manufacturing of flame retardants. It is manufactured in an equilibrium process in which phosphorus trichloride reacts with nitrogen dioxide to form POCl3(g)and NO(g) according to the following equation: PCI3 (g) + NO₂ (g) POCI3 (g) + NO (g) + 228.93kJ At 298K, the equilibrium concentration of POCI3 was 0.68 mol/L, the concentration of NO was 0.72mol/L, the concentration of PC13 was 0.62 mol/L, and the concentration of NO₂ was 0.56 mol/L. a. 6.25 moles of POCI3 (g) is added to the 5.0 L reaction chamber. What is the new concentration of POCI 3 (g) when equilibrium is re-established? PCI 3 (g) NO2 (g) E' - C E + 11 POCI 3 (g) + NO(g)
3.) Consider the reaction below. Reaction: AH°r (kJ/mole) 2 ICI (£) 17.78 L. (g) 247.551 l16.135 223.066 (/mole K) Which explains the outcome when 0.45 mol ½, 0.45 mol Cl2, and 2.42 mol ICl are added to a 2.0L flask at 25°C? A. [ICI] decreases B. [ICI] increases C. both [b] and [CL] increase D. at equilibrium Keywords: reaction quotient (Q), initial concentration(s), equilibrium concentration(s), equilibrium constant, forward reaction, reverse reaction, Q K. Q= K Concepts: Reaction Quotient, Chemical equilibrium
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N8.
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At -5.92 °C the pressure equilibrium constant K = 5.9 for a certain reaction. P Here are some facts about the reaction: • If the reaction is run at constant pressure, 127. kJ/mol of heat are released. • The constant pressure molar heat capacity C • The net change in moles of gases is -1. = 2.41 J mol -1. K¹. -1 р Yes. ☐ x10 Using these facts, can you calculate K at -27. °C? ○ No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Р If you said no, can you at least decide whether K at -27. °C will be bigger or smaller than K, at −5.92 °C? П Yes, and K, will be р bigger. Yes, and K smaller. will be No. ☑