7. The equilibrium constant for the reac- tion N2(8) + O2(g) 2NO(g) at 2130°C is 2.5 × 10-3. Why is it un- necessary to be told whether the value is for K, or K.? The reaction absorbs heat. For the following conditions, determine whether the reaction is spontaneous for- ward or in reverse, or whether it is at equilibrium: a) A 1-liter box contains 0.02 mole of NO, 0.01 mole of O2, and 0.02 mole of N, at 2130°C. b) A 20-liter box contains 0.01 mole of N,, 0.001 mole of O,, and 0.02 mole of NO at 2130°C. c) A 1-liter box contains 1.00 mole of N2, 16 moles of O,, and 0.2 mole of NO at 2500°C.

7. The equilibrium constant for the reac- tion N2(8) + O2(g) 2NO(g) at 2130°C is 2.5 × 10-3. Why is it un- necessary to be told whether the value is for K, or K.? The reaction absorbs heat. For the following conditions, determine whether the reaction is spontaneous for- ward or in reverse, or whether it is at equilibrium: a) A 1-liter box contains 0.02 mole of NO, 0.01 mole of O2, and 0.02 mole of N, at 2130°C. b) A 20-liter box contains 0.01 mole of N,, 0.001 mole of O,, and 0.02 mole of NO at 2130°C. c) A 1-liter box contains 1.00 mole of N2, 16 moles of O,, and 0.2 mole of NO at 2500°C.

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

Given the following information below, determine AGxn at equilibrium. 12(g) + Cl2(g) 2 ICI(g) 11 K, = 81.9 (at 298 K) O 1 O +10.9 kJ O -10.9 kJ
A2(g) + 3B2(g) -> 2AB3(g) where the ΔGorxn is -140 kJ and equilibrium constant at standard conditions is 3.5x1024. a) If we place 0.100 atm of AB3, 0.050 atm of B2, and 0.500 atm of A2 in a container at 25oC, which direction will the reaction go (if any) to reach equilibrium? b) What is the value of ΔGrxn assuming the temperature is maintained at 25oC?
The vapor pressure of water at 25oC is 0.0313 atm. Calculate the value of Kc at 25oC for the following reaction. H2O(l) ⇆ H2O(g) Your answer should have 3 sig figs.
A] HgS occurs in two crystalline forms called "red" and "black". For the conversion of 8. L- the red form to the black form at 525 °C, 4Gº = -0.157 kJ mol-¹ and AH = 4.184 kJ mol-¹. Assuming the AH is temperature independent, find the temperature at which the two forms can coexist at equilibrium at 1.000 bar. Which is more stable above this temperature?
Calcualte the change in Gibbs free energy (AG°) for the reaction below given the change in enthalpy (AH°) is CO (g) + H,O (g) – CO2 (g) + H2 (B) DH° = -41.2 kJ and Ds° = -135 J/mol K at 298 K -0.97 kļ/mol a 40188.8 kļ/mol -81.43 kJ/mol -0.77 kļ/mol
Kp for the following reaction is 0.16 at 25 0C. 2NOBr(g)=2NO (g)+ Br2 (l) the enthalpy change for the reaction at standard conditions is +16.1 kJ. State which way the equilibrium will shift (left, right or no change) when each of the following changes is made. Breifly explain credit for result. (a) adding more Br2 (l) (b) removing some NOBr (g) (c) Decreasing the temperature (d) increasing the container volume (e) increasing the total pressure by adding an inert gas.
6
ient/takeCovalentActivity.do?locator-assignment-take Consider the following system at equilibrium where AH° = 198 kJ, and K. = 2.90x102, at 1.15x10° K. 2S03(g) 2S02(g) + O2(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value ofK. A. increases. B. decreases. C. remains the same. The value of Q. A. is greater than K.. B. is equal to K. C. is less than K. The reaction must: A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The number of moles of O, will: A. increase. B. decrease. C. remain the same. Submit Answer Retry Entire Group 8 more group attempts remaining Prev
We start with a sample of pure A(g). The following equilibrium is established 2 A(g) <---> B(g) + C(g) The total pressure is 8.33 atm and the temperature is 25.0oC. The partial pressure of A(g) is 5.26 atm. Calculate the value of the standard free enthalpy change (in kJ) of this reaction at 25.0oC.
( do all with explanation with clear handwritting )
Consider the following system at equilibrium where ΔΗ° - 111 kJ, and == Kc = 0.159, at 7.23 × 10² K: N₂(g) + 3H₂ (g) — 2NH3 (g) If the temperature on the equilibrium system is suddenly decreased: The value of Kc Oincreases Odecreases Oremains the same The value of Qc is less than Ke Ois greater than Kc Ois equal to Ke The reaction must Orun in the forward direction to reestablish equilibrium Orun in the reverse direction to reestablish equilibrium Oremain in the current position, since it is already at equilibrium The concentration of H₂ will Oincrease Odecrease Oremain the same
Give detailed Solution with explanation..don't give Handwritten answer