At - 17.6 °C the pressure equilibrium constant K₁ = 5.1 × 105 for a certain reaction.Here are some facts about the reaction:• The net change in moles of gases is -1.• If the reaction is run at constant pressure, 129. kJ/mol of heat are absorbed.• If the reaction is run at constant pressure, the volume increases by 14.%.Yes.☐ x10Using these facts, can you calculate K, at -41. °C?No.ХIf you said yes, then enter your answer at right. Round it to2 significant digits.atIf you said no, can you at least decide whether Kp-41. °C will be bigger or smaller than K, at − 17.6 °C?PYes, and K, will bebigger.Yes, and K,, will beРsmaller.○ No.

The objective of the question is to answer, the questions related to the equilibrium constant.

At - 17.6 °C the pressure equilibrium constant Kp = 5.1 × 10° for a certain reaction. Here are some facts about the reaction: • The net change in moles of gases is -1. •If the reaction is run at constant pressure, 129. kJ/mol of heat are absorbed. • If the reaction is run at constant pressure, the volume increases by 14.%. Yes. Using these facts, can you calculate K, at-41. °C? No. X If you said yes, then enter your answer at right. Round it to 2 significant digits. P If you said no, can you at least decide whether K, at -41. °C will be bigger or smaller than K, at -17.6 °C? Yes, and K, will be bigger. Yes, and K, will be smaller. No. G

At - 17.6 °C the pressure equilibrium constant Kp = 5.1 × 10° for a certain reaction. Here are some facts about the reaction: • The net change in moles of gases is -1. •If the reaction is run at constant pressure, 129. kJ/mol of heat are absorbed. • If the reaction is run at constant pressure, the volume increases by 14.%. Yes. Using these facts, can you calculate K, at-41. °C? No. X If you said yes, then enter your answer at right. Round it to 2 significant digits. P If you said no, can you at least decide whether K, at -41. °C will be bigger or smaller than K, at -17.6 °C? Yes, and K, will be bigger. Yes, and K, will be smaller. No. G

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

Pp.58. Subject :- Chemistry
Answer the following questions about the system given the chemical reaction below.
Consider the following reaction which produces phosgene, a toxic gas used in WWI. CO (g) + Cl2 (g) ⇌ COCl2 (g) A vessel at 77°C is filled to the following initial partial pressures: PCO = 1.25 atm PCl2 = 1.65 atm PCOCl2 = 0.50 atm The standard Gibb’s Energies of Formation (ΔGf°) for CO is -137.2 kJ/mol and for phosgene (COCl2) is -304 kJ/mol. Compute the ΔG of this reaction mixture which has not yet reached equilibrium. Enter your answer in units kJ/mol.
At -6.33 °C the concentration equilibrium constant K = 1.2 x 10 for a certain reaction. Here are some facts about the reaction: • If the reaction is run at constant pressure, the volume increases by 9.7%. • The net change in moles of gases is -2. • If the reaction is run at constant pressure, 126. kJ/mol of heat are absorbed. Using these facts, can you calculate Kat -26. °C? If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether Kat –26. °℃ will be bigger or smaller than Kat -6.33 °C? Yes. O No. 0 Yes, and K will be bigger. Yes, and K will be smaller. No.
11. The equilibrium constant Kp for the following reaction is 0.403 at 1000 °C. FeO(s) + CO(g) Fe(s) + CO₂(g) Given the following starting conditions, is the system at equilibrium? If not, which direction will it proceed to get to equilibrium? a. 5.00 kg of FeO(s), Pco = 25.0 atm b. 25.0 kg of FeO(s), Pco = 25.1 atm, 14 kg Fe(s), Pco₂ = 15.2 atm c. 2.05 kg of FeO(s), Pco = 8.11 atm, 3.7 kg Fe(s), Pco₂ = 2.78 atm d. 18.0 kg of FeO(s), Pco = 29.8 atm, 6.41 kg Fe(s), P CO₂ = = 12.0 atm
75. Consider the reaction: H2(g) + I½(g) = 2 HI(g) The following data show the equilibrium constant for this reac- tion measured at several different temperatures. Use the data to find AHan and ASan for the reaction. rxn Temperature Kp 150 K 1.4 X 10 6 175 K 4.6 × 104 200 K 3.6 X 10-2 225 K 1.1 250 K 15.5
Given that Kp = 1.39 at 400. PC for the reaction, P4(g) 2 P2(g), which answer best describes the reaction when 1.30 mol of P4(g) and 1.10 mol of P2(g) are mixed in a 25.0 L, closed container at 400. °C? [REMEMBER: it's Kp] A. Qp = 0.0372 the reaction proceeds to the right. O B. Qp = 0.931. the reaction proceeds to the right. OC. Qp = 0.0372, the reaction proceeds to the left D. Qp = 1.39, the reaction is at equilibrium E. Qp = 2.06, the reaction proceeds to the left.
For the following reaction H₂(g) + ₂(g) → 2HI(g) 2 AH° = -10.64 kJ/mol and AS° = 21.48 J/mol K. A closed container in which P_H₂ = P_I₂ = 0.100 atm and P_HI = 0.500 atm is heated to 555 °C at constant pressure. After equilibrium is attained at that temperature, what is the pressure of HI in atm? Assume AH° and AS° are temperature independent.
Consider the following equilibrium: N₂O4 (g) → 2NO₂ (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 0.399 atm of dinitrogen tetroxide (N₂O4) at 588. °C. Answer the following questions about this system: Under these conditions, will the pressure of N₂O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO₂? In other words, if you said the pressure of N₂O4 will tend to rise, can that be changed to a tendency to fall by adding NO₂? Similarly, if you said the pressure of N₂O4 will tend to fall, can that be changed to a tendency to rise by adding NO₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO₂ needed to reverse it. Round your answer to 2 significant digits. O O rise fall yes no atm x10 X 5
Enter your answer in the provided box. The equilibrium constant Kp for the reaction is 159 at a certain temperature. Calculate Po, if PNo = 0.447 atm and PNo, = 0.357 atm. 2NO,(g) 5 2NO(g) + 02(g) Poz atm
The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K.2SO3(g) 2SO2(g) + O2(g)If ΔH° for this reaction is 198 kJ, what is the value of Kp at 1030 K?Kp = --- The equilibrium constant, Kp, for the following reaction is 2.01 at 500 K.PCl3(g) + Cl2(g) PCl5(g)If ΔH° for this reaction is -87.9 kJ, what is the value of Kp at 416 K?Kp =
A sample of PCI5(g) was placed in an otherwise empty flask at an initial pressure of 0.500 atm and a temperature above 500 K. Over time the PCls decomposed to PC13(g) and Cl{g): PCI5(g) 2 PC13(g) + Cl(g) At equilibrium the pressure of PCI, in the flask was found to be 0.260 atm. Calculate the value ofK, for this reaction at this temperature. Kp