21-2. Consider the following equilibrium. Which way will the system shift, if at all? How would thefollowing changes affect the partial pressures of each gas at the new equilibrium, if at all?How will the equilibrium constant change, if at all?a.PC13(g) +Cl2(g) + PCI5(g) AH = -56 kJShift(pPc13)(pcı2)(ppcis)KAddition of PCI3Removal of PC33Removal of Cl2Addition of Cl2Removal of PCI5Addition of PCI5Addition of He(g)Decrease container volumeIncrease container volumeIncrease temperatureDecrease temperature

Given reaction is: PCl3 (g) + Cl2 (g) → PCl5 (g) - 56.0 kJ So, the above reaction edothermic from…

2. Consider the following equilibrium. Which way will the system shift, if at all? How would the following changes affect the partial pressures of each gas at the new equilibrium, if at all? How will the equilibrium constant change, if at all? a. PCl3(8) Cl2(g) + PCI5(g) AH = -56 kJ Shift (prc13) (раз) (prcis) K Addition of PCl3 Removal of PCla Removal of Cl2 Addition of Cl2 Removal of PCI5 Addition of PCls Addition of He(g) Decrease container volume Increase container volume Increase temperature Decrease temperature

2. Consider the following equilibrium. Which way will the system shift, if at all? How would the following changes affect the partial pressures of each gas at the new equilibrium, if at all? How will the equilibrium constant change, if at all? a. PCl3(8) Cl2(g) + PCI5(g) AH = -56 kJ Shift (prc13) (раз) (prcis) K Addition of PCl3 Removal of PCla Removal of Cl2 Addition of Cl2 Removal of PCI5 Addition of PCls Addition of He(g) Decrease container volume Increase container volume Increase temperature Decrease temperature

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

Br2 (g) + Cl2 (g) = 2 BrCl (g) Initially, 3.4 atm each of bromine gas and chlorine gas are added to a steel cylinder and the reaction comes to equilibrium. At equilibrium, there is 1.0 atm of BrCl. What is the equilibrium pressure of chlorine gas? O A. 2.9 atm O B. 2.4 atm OC.0 atm O D. 1.0 atm O E. 3.9 atm O F. 0.1 atm O G.0.5 atm O H. Cannot be determined from the information given O1. 0.05 atm OJ. 3.4 atm
1. Please don't write on a paper. I can't understand handwritten.
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature. If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?
1C. Please don't write on a paper. I can't understand handwritten.
4. A. An important reaction in the commercial production of hydrogen is CO(g) + H2O(g) --><-- H2(g) + CO2(g) How will the system at equilibrium shift in each of the five following cases? (Use arrows or write "right" , "left" , or "no shift"). a. Gaseous carbon monoxide is removed b. In rigid reaction container, a catalyst is added. c. The temperature is decreased (the reaction is exothermic). d. The reaction container volume is doubled. e. Hydrogen gas is added. B. The equation above has a Kc value of 7.5 x 102. If 2.0 moles of each reactant and product are put into the same sealed 4.0 L container, determine the concentrations of all species present at equilibrium. Please answer A with sub parts and B.
Consider the following system at equilibrium at 600 K:COCl2(g) =CO(g) + Cl2(g)When some COCl2(g) is added to the equilibrium system at constant temperature: The reaction must: fill in the blank 1 A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of CO will: fill in the blank 2 A. Increase. B. Decrease. C. Remain the same.
d. Suppose you add compound E to the equilibrium mixture. Compound E reacts with compound D which is a component of the equilibrium to form compound F as described in the equation below. E + D Which compound is removed from the equilibrium mixture when you add compound E to the mixture? (Enter "correct" for ALL correct answers.) • B D e. What shift in the equilibrium will occur as a result of the addition of compound E? (Enter "correct" for the correct shift.) A + B C + D (shift to the right) A + B C + D (shift to the left)
23 and 24 please
3. Predict the shift in the following equilibrium system resulting from each of the following changes: 4 HCI (g) + O, (g) = 2 H,O(g) + 2 Cl, (g) + 113 kJ c. an increase in the concentration of oxygen d. the addition of a catalyst
Choose the equilibrium expression for the following reaction. a. CH4 (9) + 2H₂S(9) ⇒ CS₂ (9) + 4H₂ (9) OK: = K= OK= K= b. 4NH3(g) + 5O2(g) — 4NO(g) + 6H₂O(g) [NO] 4 [H₂0]6 [NH,][0₂]5 [NO] [H₂ O] 2 [NH3][0₂] [NO]¹ [H₂O]6 [NH₂] 4 [NO] ¹ [H₂O]6 [NH₂] 4 [0₂]5 c. CO₂(g) + MgO(s) = MgCO3(s) OK: OK= OK: OK= K: K= OK= [CS₂] [H₂]4 [CH₂] [H₂S] [CS₂] [CH][H₂S]² [CS₂] [H₂] [CH₂] [H₂S]² [CS₂] [H₂] 4 [CH₂] [H₂S]² K= 1 [CO₂] [MgCO₂]² [CO₂][MgO] [MgCO3] [CO₂]²[MgO]² [MgO] [CO₂][MgCO3]
The equation represents a chemical reaction at equilibrium. HCI (aq) + Mg (s) + Heat MgCl2 (aq) + H2 (g) What happens to the system when the temperature is decreased? O A. The reaction shifts toward the left, and the amount of hydrogen gas decreases. B. The reaction shifts toward the right, and the amount of hydrogen gas decreases. C. The reaction shifts toward the left, and the amount of hydrogen gas increases. D. The reaction shifts toward the right, and the amount of hydrogen gas increases.
Concerning the following reaction at equilibrium: 3Fe(s) + 4H2O(g) ⇋ Fe3O4(s) + 4H2(g), increasing the volume of the container would: a. Cause no change b. Decrease the value of the equilibrium constant, K c. Increase the value of the equilibrium constant, K d. Shift the equilibrium to the right e. Shift the equilibrium to the left