AP Chemistry - Unit 6 – Thermodynamics

Quiz
•
Science
•
10th Grade
•
Medium
+2
Standards-aligned
Jordan L
Used 24+ times
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14 questions
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1.
MULTIPLE CHOICE QUESTION
3 mins • 9 pts
I affirm that I will not give or receive any unauthorized help on this exam, and that all work will be my own.
I agree
I disagree
2.
MULTIPLE CHOICE QUESTION
3 mins • 7 pts
1. Which of the following is defined by the measure of the average kinetic energy?
A. Potential Energy
B. Velocity
C. Heat
D. Temperature
Answer explanation
Temperature is defined as the measure of the average kinetic energy of the sample.
Tags
NGSS.MS-PS1-4
NGSS.MS-PS3-4
3.
MULTIPLE CHOICE QUESTION
3 mins • 7 pts
2. What is the amount of energy is required to raise the temperature of 43 g of liquid water from 25°C to 55°C? Water's specific heat is 4.18 J/g°C.
A. 5.39 kJ
B. 5390 kJ
C. 4.49 kJ
D. 9.88 kJ
Answer explanation
Use the equation Q=mCΔT. The change in temperature (ΔT) is 30°C, the mass is 43 g, and the specific heat of liquid water is 4.18 J/g°C. There are 1000J for every kJ. Therefore, the hear is 5.39 kJ.
Tags
NGSS.HS-PS3-1
4.
MULTIPLE CHOICE QUESTION
3 mins • 7 pts
3. What is the amount of energy required to melt 7.2 g of water at 0°C? Water's enthalpy of fusion is 6.01 kJ/mol and water's enthalpy of vaporization is 40.7 kJ/mol.
A. 16.3 kJ
B. 43.3 kJ
C. 293 kJ
D. 2.40 kJ
Answer explanation
We must use water's enthalpy of fusion because that refers to the amount of energy required to melt 1 mol of water. The heat of vaporization refers to vaporizing 1 mol of water.
Tags
NGSS.HS-PS3-1
5.
MULTIPLE CHOICE QUESTION
3 mins • 7 pts
4. When this reaction occurs, 75.0 kJ of energy is released. What mass of copper is produced?
A. 0.588 g
B. 36.7 g
C. 110 g
D. 1.73 g
Answer explanation
1 mol of copper is produced for every 129.7 kJ of energy that is released by this reaction. Using this as a conversion factor, one finds that 0.588 mol of copper should be produced. Multiply by 63.55 g/mol, copper's molar mass, to find 36.7 g of copper is produced.
Tags
NGSS.HS-PS1-4
6.
MULTIPLE CHOICE QUESTION
3 mins • 7 pts
5. Which of the following statements is true regarding the following reaction?
A. The reaction will cause the surrounding's temperature to increase because the reaction is exothermic.
B. The reaction will cause the surrounding's temperature to decrease because the reaction is exothermic.
C. The reaction will cause the surrounding's temperature to increase because the reaction is endothermic.
D. The reaction will cause the surrounding's temperature to decrease because the reaction is endothermic.
Answer explanation
When enthalpy (ΔH) is negative, this indicates the reaction is exothermic. Therefore, the reaction will release energy to the surrounding causing the temperature to increase.
Tags
NGSS.HS-PS1-4
NGSS.HS-PS3-4
7.
MULTIPLE CHOICE QUESTION
3 mins • 7 pts
6. Determine the enthalpy of the reaction given the following data.
A. 352.6 kJ/mol
B. -352.6 kJ/mol
C. 176.3 kJ/mol
D. -176.3 kJ/mol
Answer explanation
Given the heats of formation we can use the "products minus reactants" equation. ΔH = [2x-268.6]-[2x-92.3]
Tags
NGSS.HS-PS1-4
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