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Consider a reaction where 2 moles of reactant A decompose to form 1 mole of product B. If the enthalpy change for this reaction is +50 kJ, what is the enthalpy change when 4 moles of reactant A decompose?
Consider a reaction where 2 moles of reactant A decompose to form 1 mole of product B. If the enthalpy change for this reaction is +50 kJ, what is the enthalpy change when 4 moles of reactant A decompose?
- -100 kJ
- +50 kJ
- +100 kJ (correct)
- +25 kJ
Given the following reactions:
Reaction 1: $A \rightarrow B$ $\Delta H_1 = -100 kJ$
Reaction 2: $B \rightarrow C$ $\Delta H_2 = +50 kJ$
According to Hess's Law, what is the enthalpy change for the reaction $A \rightarrow C$?
Given the following reactions:
Reaction 1: $A \rightarrow B$ $\Delta H_1 = -100 kJ$ Reaction 2: $B \rightarrow C$ $\Delta H_2 = +50 kJ$
According to Hess's Law, what is the enthalpy change for the reaction $A \rightarrow C$?
- +50 kJ
- -50 kJ (correct)
- +150 kJ
- -150 kJ
Which of the following statements accurately describes the standard enthalpy of formation ($\Delta H_f^\circ$)?
Which of the following statements accurately describes the standard enthalpy of formation ($\Delta H_f^\circ$)?
- $\Delta H_f^\circ$ of an element in its standard state is always non-zero.
- $\Delta H_f^\circ$ is the enthalpy change when one mole of a compound is formed from its elements in their standard states. (correct)
- $\Delta H_f^\circ$ is always positive for all compounds.
- $\Delta H_f^\circ$ is the enthalpy change when a compound decomposes into its elements.
A system absorbs 50 J of heat and performs 20 J of work. What is the change in internal energy ($\Delta U$) of the system?
A system absorbs 50 J of heat and performs 20 J of work. What is the change in internal energy ($\Delta U$) of the system?
Which of the following processes leads to a decrease in entropy?
Which of the following processes leads to a decrease in entropy?
For a reaction to be spontaneous at all temperatures, which of the following conditions must be met?
For a reaction to be spontaneous at all temperatures, which of the following conditions must be met?
Given the Gibbs free energy change ($\Delta G^\circ$) for a reaction is -100 kJ/mol at 298 K, calculate the equilibrium constant (K) for the reaction. Assume R = 8.314 J/mol·K.
Given the Gibbs free energy change ($\Delta G^\circ$) for a reaction is -100 kJ/mol at 298 K, calculate the equilibrium constant (K) for the reaction. Assume R = 8.314 J/mol·K.
When is the enthalpy change of a reaction equal to the heat exchanged at constant pressure?
When is the enthalpy change of a reaction equal to the heat exchanged at constant pressure?
What does the third law of thermodynamics state about the entropy of a perfect crystal at absolute zero (0 K)?
What does the third law of thermodynamics state about the entropy of a perfect crystal at absolute zero (0 K)?
Which of the following correctly relates entropy (S) to the number of microstates (W) according to the Boltzmann equation?
Which of the following correctly relates entropy (S) to the number of microstates (W) according to the Boltzmann equation?
Flashcards
Enthalpy Change (ΔH)
Enthalpy Change (ΔH)
Heat absorbed or released during a reaction at constant pressure.
Hess's Law
Hess's Law
The total enthalpy change for a reaction is the same whether it occurs in one step or multiple steps.
Standard Enthalpy of Formation (ΔHf°)
Standard Enthalpy of Formation (ΔHf°)
Enthalpy change when one mole of a compound is formed from its elements in their standard states.
First Law of Thermodynamics
First Law of Thermodynamics
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Second Law of Thermodynamics
Second Law of Thermodynamics
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Third Law of Thermodynamics
Third Law of Thermodynamics
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Entropy (S)
Entropy (S)
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Gibbs Free Energy (G)
Gibbs Free Energy (G)
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ΔG° and Equilibrium Constant (K)
ΔG° and Equilibrium Constant (K)
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Study Notes
Study notes about thermodynamics
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