Chapter 6 Practice Test Flashcards Preview

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Flashcards in Chapter 6 Practice Test Deck (25)
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1
Q

What is the SI unit for energy?

A

joule

2
Q

What is the kinetic energy of a basketball having a mass of 0.65 kg that is falling at 3.5 m / s?

A

4.0 J

3
Q

Which of the following objects has non-zero potential energy, but zero kinetic energy?

A

An encyclopedia on the top shelf of a bookcase

4
Q

What are the products of metabolizing food?

A

carbon dioxide and water

5
Q

How many Calories are in 3 servings of the food described in the following label?

A

424.5 Cal

6
Q

How is excess energy stored in the body?

A

as fat

7
Q

What is the First Law of Thermodynamics?

A

The total energy in the universe is constant.

8
Q

In the equation E = q + w, what does the q represent

A

heat

9
Q

Which of the following is not a state function?

A

work

10
Q

What is the work in joules when a gas expands from 3.10 L to 6.40 L against a constant external pressure of 2.00 atm?
Use 1 L-atm = 101.325 J.

A

−669 J

11
Q

When w is positive, which of the following is true?

A

Work was done by the surroundings on the system.

12
Q

When q is negative, which of the following is true?

A

Heat flowed from the system to the surroundings.

13
Q

What is the correct definition of heat?

A

Heat is the energy that flows because of difference in temperature between the system and its surroundings.

14
Q

How much heat (in kJ) is absorbed by a 500. g sample of water when it is heated from 44.0°C to 67.0°C?
The specific heat capacity of water is 4.184 J / g°C.

A

48.1 kJ

15
Q

The first law of thermodynamics is written as, ΔE = q + w. What would ΔE be equal to when imposing a constant volume restriction to a system?

A

ΔE = qV

16
Q

Which of the following describes an endothermic reaction?

A

A reaction that moves heat from the surroundings into the system

17
Q

Change in enthalpy is equal to heat measured under what condition?

A

constant pressure

18
Q

A friend wants you to calculate the molar heat capacity of a given metal. He gives you the initial and final temperatures of the water in the calorimeter, the initial temperature of the metal, and the mass of the metal. You know that the molar heat capacity of water is 75.4 J / mol. What other information do you need before you can calculate the molar heat capacity of the metal?

A

The amount of water

19
Q

A calorimeter contains 75.0 g of water at an initial temperature of 25.2 °C. 151.28 g of copper metal at a temperature of 95.5 °C was placed in the calorimeter. The equilibrium temperature was 36.2 °C. The molar heat capacity of water is 75.4 J / mol °C. Determine the molar heat capacity of the copper.

A

24.5 J / mol °C

20
Q

What does the C in the equation qsurr = CΔT represent?

A

The heat capacity of the calorimeter and its surroundings

21
Q

A reaction is carried out in a bomb calorimeter. Which of the following is TRUE if the heat of the reaction is found to be a negative value?

A

The heat of the surroundings increased

22
Q

The combustion of methane is given by the following equation:
CH4(g) + 2 O2(g) → CO2(g) + H2O(g) ΔH = −890 kJ
What is the enthalpy change for 5 moles of methane?

A

−4450 kJ

23
Q

When one mole of ice melts, the change in enthalpy is +6.0 kJ. What is the enthalpy change for the freezing of one mole of water?

A

−6.0 kJ

24
Q

Which of the following is not a standard enthalpy of formation reaction?

A

2H2(g) + O2(g) → 2H2O(l)

25
Q

Which of the following statements is not true about allotropes?

A

Allotropes have different forms at room temperature, but the same enthalpy.

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