Consider the following system at equilibrium where \( \Delta H^\circ = 92.7 \, \text{kJ} \), and \( K_c = 1.80 \times 10^{-4} \), at 298 K.\[ \text{NH}_4\text{HS} (s) \rightarrow \text{NH}_3 (g) + \text{H}_2\text{S} (g) \]When some moles of \( \text{NH}_4\text{HS} (s) \) are removed from the equilibrium system at constant temperature:1. The value of \( K_c \) - \( \circ \) increases - \( \phantom{\circ} \) decreases - \( \phantom{\circ} \) remains the same2. The value of \( Q_c \) - \( \phantom{\circ} \) is greater than \( K_c \) - \( \circ \) is equal to \( K_c \) - \( \phantom{\circ} \) is less than \( K_c \)3. The reaction must - \( \circ \) run in the forward direction to reestablish equilibrium. - \( \phantom{\circ} \) run in the reverse direction to reestablish equilibrium. - \( \phantom{\circ} \) remain the same. It is already at equilibrium.4. The number of moles of \( \text{NH}_3 \) will - \( \circ \) increase - \( \phantom{\circ} \) decrease - \( \phantom{\circ} \) remain the same ```markdownConsider the following system at equilibrium where \( \Delta H^\circ = -87.9 \, \text{kJ} \), and \( K_c = 83.3 \), at 500 K:\[ \text{PCl}_3(g) + \text{Cl}_2(g) \rightleftharpoons \text{PCl}_5(g) \]When 0.36 moles of \( \text{PCl}_5(g) \) are added to the equilibrium system at constant temperature:The value of \( K_c \)- ( ) increases- ( ) decreases- (O) remains the sameThe value of \( Q_c \)- (O) is greater than \( K_c \)- ( ) is equal to \( K_c \)- ( ) is less than \( K_c \)The reaction must- ( ) run in the forward direction to reestablish equilibrium- (O) run in the reverse direction to reestablish equilibrium- ( ) remain in the current position, since it is already at equilibriumThe concentration of \( \text{PCl}_3 \) will- (O) increase- ( ) decrease- ( ) remain the same```This text is designed to help students understand how changes in concentration affect equilibrium conditions in a chemical reaction, using \( \Delta H \), \( K_c \), and \( Q_c \) as guiding parameters. The use of checkboxes indicates choices for hypothetical scenarios regarding changes in equilibrium and concentration. There are no graphs or diagrams in this content.

The objective of the question is to solve the problems related to equilibrium.

Consider the following system at equilibrium where AHO NH4HS(s) → NH3 (9) + H₂S(9) When some moles of NH4HS(s) are removed from the equilibrium system at constant temperature: The value of Kc O increases O decreases O remains the same The value of Qc O is greater than Kc O is equal to Kec O is less than KC = 92.7 kJ, and Kc = 1.80 × 10-4, at 298 K. The reaction must Orun in the forward direction to reestablish equilibrium. Orun in the reverse direction to reestablish equilibrium. O remain the same. It is already at equilibrium. The number of moles of NH3 will O increase O decrease O remain the same Click to reveal a list of eBook readings and review topics associated with this item.

Consider the following system at equilibrium where AHO NH4HS(s) → NH3 (9) + H₂S(9) When some moles of NH4HS(s) are removed from the equilibrium system at constant temperature: The value of Kc O increases O decreases O remains the same The value of Qc O is greater than Kc O is equal to Kec O is less than KC = 92.7 kJ, and Kc = 1.80 × 10-4, at 298 K. The reaction must Orun in the forward direction to reestablish equilibrium. Orun in the reverse direction to reestablish equilibrium. O remain the same. It is already at equilibrium. The number of moles of NH3 will O increase O decrease O remain the same Click to reveal a list of eBook readings and review topics associated with this item.

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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