-more-fuiorite1223. A flask is charged with 1.500 atm of N₂O4(g) and 1.00 atm NO₂(g) at 25°C, and the followingequilibrium is established.2 NO₂(g) N₂O4(g)At equilibrium, the partial pressure of NO₂(g) is 0.512 atm. Calculate the equilibrium constantKp for this reaction.A. 9.45B. 5.72C. 7.58D. 3.81E. 6.652N02= N₂0 uI 1.5сE

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Answered: -mare-foiorite 12 23. A flask is…

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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Consider the reaction SbH5 (g) SbH3 (g) + H2 (g) If 0.500 atm of SbH5 is introduced into an empty, closed container at 248oC and the system is allowed to reach equilibrium, 0.397 atm of SbH5 remains. Find Kp and Kc.
4. The vapor pressure of ethanol is 400 mmHg at 63.5 °C. Its molar heat of vaporization is 41.7 kJ/mol. Calculate the vapor pressure of ethanol at 34.9 °C. Use 3 sig figs; don't forget the units. [Ans: around 100] 17. Kp for the decomposition of ammonium chloride at 427 °C NH4Cl (s) NH3 (g) + HCI (g) Kp = 4.8 Calculate Ke for the reaction.
When 1.24 moles of N2O4(g) is introduced into a 2.00 L container at 45 °C and allowed to reach equilibrium, 4.22% of the N2O4 is dissociated into NO2(g). Find Ko and Kp.
following equilibrium reaction at 160.00 °C. If 0.420 atm of H2O2(g) is initially present, calculate the equilibrium partial pressures of H2(g), O2(g), and H2O2(g).
A flask is charged with 1.5 atm of N2O4 (g) and 1 atm NO2 (g) at 20°C and the following equilibrium is achieved: N204 (g) 2 NO2 (g). After equilibrium is reached, the partial pressure of NO2 is 0.512 atm. a. What is the equilibrium partial pressure of N2O4 b. Calculate the value Kp for the reaction. c. Calculate Kc for the reaction.
Carbon monoxide reacts with water according to the following equilibrium reaction: CO (g) H2O (g) CO2 (g) + H2 (g) For this reaction, K = 0.810 at a temperature of 1000.°C. Calculate the value of AG for this reaction at 1000.ºC. %3D
12. Consider the chemical reaction 2HCl(g) H2(g) + Cl2(g). It contains 8.0 mol HCI, 0.20 mol H₂ and 0.40 mol Cl₂ in a 1.00 L flask at equilibrium. Calculate Kc and Kp at 300. °C. for the reaction.
The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K.CO(g) + Cl2(g) COCl2(g)If ΔH° for this reaction is -108 kJ, what is the value of Kp at 699 K?Kp =
For the equilibrium system below, which of the following would result in an increase in the quantity of H₂(g)? H₂(g) + 12(g) 2HI(g) + 65 kJ ос removing some I₂(g) and removing some HI(g) removing some HI(g) removing some 1₂(g) decreasing temperature removing some HI(g) and decreasing temperature
Given this reaction at equilibrium, C(s) + CO2(g) D 2CO(g) (∆H° = 119kJ), explain the changes that would occur when the following stresses are applied: a.CO is removed. b.Heat is removed. c.CO2 is added.
8. Consider the following reaction at 1600°C. Br2(g) = 2Br(g) When 1.05 moles of Br2 are put in a 0.980-L flask, 1.20 percent of the Br2 undergoes dissociation. Calculate the equilibrium constant Ke for the reaction
Please help please.. *The equilibrium constant for the reaction of chlorine gas with phosphorus trichloride to form phosphorus pentachloride is 33 at 250°C. If an experiment is initiated with concentrations of 0.035 M PCl3 and 0.035 M Cl2, determine the equilibrium concentration of PCl5. *A reaction at 25⁰C has an equilibrium constant measured as 1113. Calculate the free energy change. *Determine the equilibrium concentration of Cl2.

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