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Exam 8: Thermochemistry: Chemical Energy

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Question 31

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A process is carried out at constant pressure.Given that 0 > ΔH > ΔE,

A) the system absorbs heat and expands during the process.
B) the system absorbs heat and contracts during the process.
C) the system loses heat and expands during the process.
D) the system loses heat and contracts during the process.

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Question 32

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

A) CO
B) CO₂
C) HCO₂H
D) CO₃^2-

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Question 33

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Which of the following can be interpreted as a measure of randomness?

When 0.455 g of anthracene,C₁₄H₁₀,is combusted in a bomb calorimeter that has a water jacket containing 500.0 g of water,the temperature of the water increases by 8.63°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.

What is expected when the reaction shown below takes place in a thermally-insulated container outfitted with a movable piston at a constant atmospheric pressure of 1 atm? 2 C₂H₆(g) + 7 O₂(g) → 4 CO₂(g) + 6 H₂O(g)

The specific heat of copper is 0.385 J/(g ∙°C) .If 34.2 g of copper,initially at 25°C,absorbs 4.689 kJ,what will be the final temperature of the copper?

Heat transfer measured in a coffee-cup calorimeter at constant pressure is a measure of ________,but heat transfer measured in a bomb calorimeter at constant volume is a measure of ________.

Determine the sign of ΔS° for each of the following: I.The mixing of two gases at a given temperature and pressure II.C(s) + 2 H₂O(g) → CO₂(g) + 2 H₂(g)

The sign of ΔS° for reaction below is expected to be ________. 2 H₂(g)+ O₂(g)→ 2 H₂O(g)

The following drawing is a representation of the exothermic reaction in which ozone forms dioxygen. -What are the signs of ΔH and ΔS for this reaction?

Under thermodynamic standard state conditions the element oxygen occurs as

Which of CH₄(g) ,C₂H₂(g) ,and CH₃OH(l) provides the most energy per gram upon combustion and which provides the least? CH₄(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(l) ΔH° = -890 kJ 2 C₂H₂(g) + 5 O₂(g) → 4 CO₂(g) + 2 H₂O(l) ΔH° = -2599 kJ 2 CH₃OH(l) + 3 O₂(g) → 2 CO₂(g) + 4 H₂O(l) ΔH° = -1453 kJ

When 1.00 mol of benzene is vaporized at a constant pressure of 1.00 atm and at its normal boiling point of 80.1°C,33.9 kJ are absorbed and PΔV for the vaporization process is equal to 2.90 kJ,then

Calculate the work energy,w,gained or lost by the system when a gas expands from 15 L to 35 L against a constant external pressure of 1.5 atm.[1 L ∙ atm = 101 J]

At 25°C the heat of fusion of aluminum is 10.6 kJ/mol and the heat of sublimation is 326.4 kJ/mol.What is the heat of vaporization of aluminum at 25°C?

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

Because the number of moles of gas are increasing from 6 to 7 in the reaction shown below,at constant pressure ΔE is predicted to be slightly ________ negative than ΔH. C₃H₈(g)+ 5 O₂(g)→ 3 CO₂(g)+ 4 H₂O(g)

It takes 11.2 kJ of energy to raise the temperature of 145 g of benzene from 25.0°C to 70.0°C.What is the specific heat of benzene?

The enthalpy of fusion of naphthalene,C₁₀H₈,is 19.1 kJ/mol at 78.2°C,its melting point.Calculate the entropy of fusion at the melting point.

At constant pressure,the combustion of 5.00 g of C₂H₆(g) releases 259 kJ of heat.What is ΔH for the reaction given below? 2 C₂H₆(g) + 7 O₂(g) → 4 CO₂(g) + 6 H₂O(l)