Consider the following system at equilibrium where Kc
= 1.80×10-2and delta H° =
10.4 kJ/mol at 698 K.
2 HI (g) goes to
H2(g) +
I2(g)
The production of H2(g) is favored
by:
Indicate True (T) or False (F)
for each of the following:
___TF 1. increasing the
temperature.
___TF 2. increasing the pressure
(by changing the volume).
___TF 3. increasing the
volume.
___TF 4. removing
HI .
___TF 5. removing
I2.
1)
Increasing Temperature will shift the reaction in a direction which
absorbs heat as per Le chatelier Principle
Forward reaction is endothermic in nature
hence, forward reaction will be favoured
So, Equilibrium moves to product side
Answer: True
2)
Increasing pressure will shift the reaction in a direction which
have lesser gaseous molecules as per Le chatelier Principle
Here, number of gaseous molecules is same on both side
So equilibrium will not be effected
So, No effect on equilibrium
Answer: False
3)
Increasing volume will decrease the pressure which in turn shift
the reaction in a direction which have greater gaseous molecules as
per Le chatelier Principle
Here, number of gaseous molecules is same on both side
So equilibrium will not be effected
So, No effect on equilibrium
Answer: False
4)
Removing reactant will shift the reaction in the direction of
reactant as per Le chatelier Principle
So, Equilibrium moves to reactant side
Answer: False
5)
Removing product will shift the reaction in the direction of
product as per Le chatelier Principle
So, Equilibrium moves to product side
Answer: True
Consider the following system at equilibrium where Kc = 1.80×10-2and delta H° = 10.4 kJ/mol at...
Consider the following system at equilibrium where Kc = 1.80×10-2and H° = 10.4 kJ/mol at 698 K. 2 HI (g) -->H2(g) + I2(g) The production of H2(g) is favored by: Indicate True (T) or False (F) for each of the following: ___TF 1. increasing the temperature. ___TF 2. increasing the pressure (by changing the volume). ___TF 3. increasing the volume. ___TF 4. removing HI . ___TF 5. adding I2. Consider the following system at equilibrium where Kc = 55.6 and...
Consider the following system at equilibrium where Kc = 7.00×10-5and delta H° = 182 kJ/mol at 673 K. NH4I (s) = NH3(g) + HI (g) The production of NH3(g) is favored by: Indicate True (T) or False (F) for each of the following: ___TF 1. decreasing the temperature. ___TF 2. decreasing the pressure (by changing the volume). ___TF 3. decreasing the volume. ___TF 4. adding NH4I . ___TF 5. removing HI . Submit Answer
Consider the following system at equilibrium where Kc = 7.00×10-5and H° = 182 kJ/mol at 673 K. NH4I (s) - NH3(g) + HI (g) The production of NH3(g) is favored by: Indicate True (T) or False (F) for each of the following: ___TF 1. increasing the temperature. ___TF 2. decreasing the pressure (by changing the volume). ___TF 3. increasing the volume. ___TF 4. adding NH4I . ___TF 5. removing HI
Consider the following system at equilibrium where K. = 1.80x10-2 and AH° = 10.4 kJ/mol at 698 K. 2 HI (g) – H2 (g) +12 (g) The production of H2 (g) is favored by: Indicate True (T) or False (F) for each of the following: - - - 1. increasing the temperature. 2. increasing the pressure (by changing the volume). 3. increasing the volume. 4. adding HI 5. removing 12 . -
Consider the following system at equilibrium where Kc = 9.52×10-2 and H° = 18.8 kJ/mol at 350 K. CH4 (g) + CCl4 (g) goes to 2 CH2Cl2 (g) The production of CH2Cl2 (g) is favored by: Indicate True (T) or False (F) for each of the following: 1. decreasing the temperature. 2. decreasing the pressure (by changing the volume). 3. increasing the volume. 4. removing CH2Cl2 . 5. removing CCl4 .
Consider the following system at equilibrium where H° = 10.4 kJ, and Kc = 1.80×10-2, at 698 K: 2HI(g) =H2(g) + I2(g) If the TEMPERATURE on the equilibrium system is suddenly decreased: The value of Kc A. Increases B. Decreases C. Remains the same The value of Qc A. Is greater than Kc B. Is equal to Kc C. Is less than Kc The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction...
Consider the following system at equilibrium where Kc = 6.50×10-3 and H° = 16.1 kJ/mol at 298 K. 2 NOBr (g) 2 NO (g) + Br2 (g) The production of NO (g) is favored by: Indicate True (T) or False (F) for each of the following: 1. increasing the temperature. 2. increasing the pressure (by changing the volume). 3. increasing the volume. 4. adding NOBr . 5. removing Br2 .
Consider the following system at equilibrium where Kc = 77.5 and H° = -108 kJ/mol at 600 K. CO (g) + Cl2 (g) COCl2 (g) The production of COCl2 (g) is favored by: Indicate True (T) or False (F) for each of the following: 1. decreasing the temperature. 2. increasing the pressure (by changing the volume). 3. increasing the volume. 4. adding COCl2 . 5. removing Cl2 .
Consider the following system at equilibrium where Kc = 34.5 and H° = -198 kJ/mol at 1150 K. 2 SO2 (g) + O2 (g) 2 SO3 (g) The production of SO3 (g) is favored by: Indicate True (T) or False (F) for each of the following: 1. decreasing the temperature. 2. decreasing the pressure (by changing the volume). 3. decreasing the volume. 4. removing SO3 . 5. adding O2 .
Consider the following system at equilibrium where K - 1.29x10- and AH = 108 kJ/mol at 600 K. COC12() CO(g) + Cl2 ) The production of CO (g) is favored by: Indicate True (T) or False (F) for each of the following: 1. increasing the temperature. 2. increasing the pressure (by changing the volume). 3. increasing the volume. 4. removing COCI2. 5. removing Cl2 Submit Answer Retry Entire Group 1 more group attempt remaining Consider the following system at equilibrium...