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Exam 9: Thermochemistry: Chemical Energy

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Question 61

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For the expansion of an ideal gas into a vacuum at constant temperature,ΔH = 0.What can be said about ΔE and ΔS?

A) ΔE is negative and ΔS is positive.
B) ΔE is zero and ΔS is positive.
C) ΔE is negative and ΔS is zero.
D) ΔE is positive and ΔS is negative.

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Question 62

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Which of the following is not a state function?

A) depth
B) heat
C) internal energy
D) gas

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Question 63

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Most chemical reactions are carried out in one of two ways: I.in an open vessel at constant atmospheric pressure II.in a closed vessel Which is true?

A process is carried out at constant pressure.Given that ΔE is positive and ΔH is negative,

The enthalpy of fusion,or heat of fusion (ΔH_fusion) ,of water is positive and corresponds to which physical change?

The following drawing is a representation of a reaction of the type A → B,where different shaded spheres represent different molecular structures.For this reaction ΔH° = -30 kJ.This reaction is likely to be

When 10.0 mol of benzene is vaporized at a constant pressure of 1.00 atm and at its normal boiling point of 80.1°C,339 kJ are absorbed and PΔV for the vaporization process is equal to 29.0 kJ,then

What are the signs of ΔH,ΔS,and ΔG for the following spontaneous change?

Which is expected to have the largest carbon-oxygen bond dissociation energy?

In the reaction below,is energy released or absorbed by the system? What is the sign of the energy change,E? 432 kJ + A + 2B → 3C

Calculate ΔG° for the reaction below and tell whether it is spontaneous or nonspontaneous under standard conditions at 25°C. 2 S (s) + 3 O₂ (g) + 2 H₂O (l) → 2 H₂SO₄ (l) ΔH° = -1056 kJ/mol ΔS° = -505 J/mol

Ethyl alcohol is produced by the fermentation of glucose,C₆H₁₂O₆. C₆H₁₂O₆(s) → 2 C₂H₅OH(l) + 2 CO₂(g) ΔH° = -69.1 kJ Given that the enthalpy of formation is -277.7 kJ/mol for C₂H₅OH(l) and -393.5 kJ/mol for CO₂(g) ,find the enthalpy of formation for C₆H₁₂O₆.

For which reaction is H expected to be most positive?

Energy can be classified as either ________ energy (energy of motion)or ________ energy (stored energy).

At a given temperature and pressure,which of the following would be expected to have the greatest molar entropy?

The specific heat of copper is 0.385 J/(g ∙ °C) .If 34.2 g of copper,initially at 21.0°C,absorbs 4.689 kJ,what will be the final temperature of the copper?

When 0.700 g of anthracene,C₁₄H₁₀,is combusted in a bomb calorimeter that has a water jacket containing 500.g of water,the temperature of the water increases by 13.27°C.Assuming that the specific heat of water is 4.18 J/(g ∙ °C) ,and that the heat absorption by the calorimeter is negligible,estimate the enthalpy of combustion per mole of anthracene.

Given: S (s) + O₂ (g) → SO₂ (g) ΔH° = -296.1 kJ 2 SO₃ (g) → 2 SO₂ (g) + O₂ (g) ΔH° = 198.2 kJ Find ΔH° for : 2 S(s) + 3 O₂(g) → 2 SO₃(g)

A reaction is performed in a water bath initially at 28°C which decreases to 10°C by the end of the reaction.For this reaction the sign of heat transfer is ________,and the reaction is classified as ________.

For a system at constant pressure,19,400 calories of heat are released.This quantity of heat is equivalent to