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Questions and Answers
What is the equilibrium constant for the reaction PCl5(g) ⇌ PCl3(g) + Cl2(g) if the flask at equilibrium contains 0.1 mol PCl5, 0.20 mol PCl3, and 0.20 mol Cl2?
What is the equilibrium constant for the reaction PCl5(g) ⇌ PCl3(g) + Cl2(g) if the flask at equilibrium contains 0.1 mol PCl5, 0.20 mol PCl3, and 0.20 mol Cl2?
- 0.4
- 0.004
- 0.045
- 0.02 (correct)
Which compound is NOT a Brønsted-Lowry acid?
Which compound is NOT a Brønsted-Lowry acid?
- CH3COOH
- NH3 (correct)
- (CH3)NH+
- HNO2
In the reaction 2 CO2(g) ⇌ 2 CO(g) + O2(g), how can the equilibrium partial pressure of CO (g) be maximized according to Le Châtelier's principle?
In the reaction 2 CO2(g) ⇌ 2 CO(g) + O2(g), how can the equilibrium partial pressure of CO (g) be maximized according to Le Châtelier's principle?
- At high temperature and high pressure
- At low temperature and high pressure
- At low temperature and low pressure
- At high temperature and low pressure (correct)
A 0.045 M aqueous solution with a pOH of 5.33 is classified as:
A 0.045 M aqueous solution with a pOH of 5.33 is classified as:
For a system that absorbs 60 J of heat while 40 J of work are performed on it, then releases 30 J of heat while doing 70 J of work, what is the change in internal energy (ΔU)?
For a system that absorbs 60 J of heat while 40 J of work are performed on it, then releases 30 J of heat while doing 70 J of work, what is the change in internal energy (ΔU)?
Which statement is TRUE about enthalpy?
Which statement is TRUE about enthalpy?
What is the heat capacity of the water in the bomb calorimeter?
What is the heat capacity of the water in the bomb calorimeter?
Which substance has the highest standard enthalpy of formation among NH3(g), HCl(g), and NH4Cl(s)?
Which substance has the highest standard enthalpy of formation among NH3(g), HCl(g), and NH4Cl(s)?
What is the equilibrium constant for the reaction NH3(g) + HCl(g) ⇌ NH4Cl(s) at 25oC?
What is the equilibrium constant for the reaction NH3(g) + HCl(g) ⇌ NH4Cl(s) at 25oC?
In Le Chatelier's principle, what happens when a stress is applied to a system at equilibrium?
In Le Chatelier's principle, what happens when a stress is applied to a system at equilibrium?
Which concept involves ions that do not participate in a chemical reaction but are present in the solution?
Which concept involves ions that do not participate in a chemical reaction but are present in the solution?
What is the rest mass of a neutron?
What is the rest mass of a neutron?
Which of the following statements about enthalpy is correct?
Which of the following statements about enthalpy is correct?
For the reaction N2O4(g) + Cl2(g) → 2 NOCl(g) + O2(g), what is ΔHo?
For the reaction N2O4(g) + Cl2(g) → 2 NOCl(g) + O2(g), what is ΔHo?
In the reaction 2 KCl(aq) + O2(g) → 2 KClO3(aq), which species acts as a spectator ion?
In the reaction 2 KCl(aq) + O2(g) → 2 KClO3(aq), which species acts as a spectator ion?
Which of the following reactions has ΔH equal to ΔH°f?
Which of the following reactions has ΔH equal to ΔH°f?
If a human needs 11300 kJ of energy per day, and ΔHcombustion of glucose is -5650 kJ mol–1, how many grams of glucose must be consumed per day?
If a human needs 11300 kJ of energy per day, and ΔHcombustion of glucose is -5650 kJ mol–1, how many grams of glucose must be consumed per day?
What is the specific heat capacity of lead if 52 J of heat raises the temperature of a block of lead from 22°C to 32°C?
What is the specific heat capacity of lead if 52 J of heat raises the temperature of a block of lead from 22°C to 32°C?
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Study Notes
Le Châtelier's Principle
- Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximised under different conditions:
- Low temperature and low pressure
- High temperature and low pressure
- High temperature and high pressure
- Low temperature and high pressure
- In the presence of solid carbon
Equilibrium Constant
- The equilibrium constant (Kc) can be calculated from the concentrations of reactants and products at equilibrium:
- Kc = [PCl3]^2 [Cl2]^2 / [PCl5]^2
Thermodynamics
- ΔU (change in internal energy) can be calculated from the heat absorbed and work done on the system:
- ΔU = Q - W
- Enthalpy (H) is a state function, and ΔH is independent of the state of the reactants and products:
- ΔH = ΔH°f (enthalpy of formation)
Calorimetry
- The heat of combustion of octane (C8H18) can be calculated from the temperature change in a bomb calorimeter:
- ΔHcombustion = -5650 kJ mol-1 (for glucose)
Reaction Equilibria
- The equilibrium constant (Kc) can be calculated from the concentrations of reactants and products at equilibrium:
- Kc = [NH4Cl] / [NH3] [HCl]
- The reaction quotient (Q) can be calculated from the concentrations of reactants and products at any time:
- Q = [NH4Cl] / [NH3] [HCl]
Thermodynamic Properties
- Standard enthalpy of formation (ΔH°f) is the enthalpy change for the formation of one mole of a substance from its constituent elements:
- ΔH°f (NH3) = -46.19 kJ mol-1
- ΔH°f (HCl) = -92.30 kJ mol-1
- ΔH°f (NH4Cl) = -314.4 kJ mol-1
Energy Requirements
- A human being requires 11300 kJ of energy per day:
- To satisfy this energy requirement, a person needs to consume a certain amount of glucose:
- Amount of glucose = 11300 kJ / -5650 kJ mol-1 = 2 mol (approx.)
- To satisfy this energy requirement, a person needs to consume a certain amount of glucose:
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