d.he following system establishes an equilibrium at 545 K:NH₂HS (s)-NH₂ (8) + H₂S (8)AND >OBriefly explain the effect in terms of the expected shift (toward reactant, toward product or nochange) of each of the following:ab.The volume of the container is doubled.The temperature of the system is raised to 825 KC. Some additional solid NH4HS is added.The reaction flask has 1.25 atm of the inert gas argon added to it.5. (10 points) At 355 K, a 10.00 L reaction flask is charged with 1.44 atm each of hydrogenand fluorine gas. The following reaction takes place:H2 (8) + F2 (g) = 2 HF (g)Kp = 176Based on building an ICE table, determine the partial pressure of H2, F2 and HF once equilibriumhas been established.

Dear student , since you have posted multiple parts questions we are allowed to solve only first…

he following system establishes an equilibrium at 545 K: NH₂HS (s) - NH₂ (8) + H₂S (8) AND >O Briefly explain the effect in terms of the expected shift (toward reactant, toward product or no change) of each of the following: a. The volume of the container is doubled. C. b. The temperature of the system is raised to 825 K Some additional solid NH4HS is added.

he following system establishes an equilibrium at 545 K: NH₂HS (s) - NH₂ (8) + H₂S (8) AND >O Briefly explain the effect in terms of the expected shift (toward reactant, toward product or no change) of each of the following: a. The volume of the container is doubled. C. b. The temperature of the system is raised to 825 K Some additional solid NH4HS is added.

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

A student artificially pumped 1 mole of each substance seen below in a piston with a moveable lid (this lid can increase or decrease thereby changing the volume and pressure): 2 C3H7OH (g) + 902 (g) 6 CO2 (g) +8 H2O(g) If the student increased the volume of the piston, how will the reaction shift to reach a new equilibrium? No conclusion can be made since more information is needed The reaction will shift to the left The reaction will shift to the right The reaction will not shift because Q = K
Choose the process that will not disturb the following equilibrium. Co(g) + H20(g) CO2(g) + H2(g) O A. Adding co B. Increasing the temperature O C. Increasing the volume D. Removing H2
O O Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 0.0074: N,(g) + 0,(g) = 2NO(g) Use this information to complete the following table. Suppose a 22. L reaction vessel is filled with 0.89 mol of N, and 0.89 mol of O2. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little N2 and 02. There will be very little NO. O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = ] 2 NO(g) N2(9)+O2(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K =] 2N2(9)+202(g) 4 NO(g) 1. Explanation Check 02021 McGraw-Hill Education All Rights Reserved Terms of U
A 3.00-liter flask initially contains 3.00 mol of gas A and 1.50 mol of gas B. Gas A decomposes according to the following reaction: 3A 2B+C The equilibrium concentration of gas C is 0.134 mol/L. Determine the value of the equilibrium constant, K O a. 0.172 O b. 0.132 OC. 3.19 10-3 O d. 0.370 X e. none of these
12. The following gases are added to a 1.00 L container: 2.0 mole of A; 4.0 mole of B. The gases react as follows: A (g) + 3B (g) = C (g) + 2D (g) a. Create an ICE table to indicate the initial concentrations, the change in concentrations with respect to x, and the equilibrium concentrations al all the reactants and produces with respect to x. b. If the container contains 0.4 moles of D at equilibrium, calculate the equilibrium concentrations of A, B, C, and D. c. Calculate the value for the equilibrium constant at this temperature.
Consider the following system at equilibrium at 698 K: 2 HI (g)=H2 (g) + I2 (g) When some H2 (g) is added to the equilibrium system at constant temperature: 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 concentration of I, will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Retry Entire Group 9 more group attempts remaining
4
Please don't provide handwriting solutions...
only d
+O2 (8) 2 SO, (8) A,2.000 Lflask was initially filled with,0.0400 mol SO and 0.0200 mol O, and was allowed to reach equilibrium. If the flask contained, 0.0296 mol SO, at equilibrium: Consider the following: 2 SO, (e) 2 (g) 32 3. al Calculate the moles of each substance present at equilibrium. b| Calculate the equilibrium constant, K. + O2 (3) = 2SO, (8) 3 (g) c Calculate the equilibrium constant, K, for the following: 2 SO, +2O2(8) = 4 SO, (3) 2 (g) d| Calculate the equilibrium constant, K, for the following: 4 SO, (e) of HCN CHEMISTRY 1516L