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Exam 6: Thermochemistry

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Question 41

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Use the ΔH°_f information provided to calculate ΔH°_rxn for the following: ΔH°_{f (kJ/mol)} SO₂Cl₂(g) + 2 H₂O(l) → 2 HCl(g) + H₂SO4(l) ΔH°_rxn = ? SO₂Cl₂(g) -364 H₂O(l) -286 HCl(g) -92 H₂SO₄(l) -814

A) -256 kJ
B) +161 kJ
C) -62 kJ
D) +800.kJ
E) -422 kJ

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Question 42

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Match the following. --w

A) work done by the system on the surroundings
B) system gains thermal energy from surroundings
C) energy flows out of system into the surroundings
D) system loses thermal energy to surroundings
E) work done on the system by the surroundings
F) energy flows into the system from the surroundings

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Question 43

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According to the following reaction,how much energy is evolved during the reaction of 2.50 L B₂H₆ and 5.65 L Cl₂ (Both gases are initially at STP) ? The molar mass of B₂H₆ is 27.67 g/mol. B₂H₆(g) + 6 Cl₂(g) → 2 BCl₃(g) + 6 HCl(g) ΔH°_rxn = -1396 kJ

A piece of iron (mass = 25.0 g) at 398 K is placed in a styrofoam coffee cup containing 25.0 mL of water at 298 K.Assuming that no heat is lost to the cup or the surroundings,what will the final temperature of the water be? The specific heat capacity of iron = 0.449 J/g°C and water = 4.18 J/g°C.

When 1.50 mol of CH₄(g) reacts with excess Cl₂(g) at constant pressure according to the chemical equation shown below,1062 kJ of heat are released.Calculate the value of ΔH for this reaction,as written. 2 CH₄(g) + 3 Cl₂(g) → 2 CHCl₃(l) + 3 H₂(g) ΔH = ?

According to the following reaction,how much energy is required to decompose 55.0 kg of Fe₃O₄? The molar mass of Fe₃O₄ is 231.55 g/mol. Fe₃O₄(s) → 3 Fe(s) + 2 O₂(g) ΔH°_rxn = +1118 kJ

According to the following thermochemical equation,what mass of H₂O (in g) must form in order to produce 488 kJ of energy? SiO₂(s) + 4 HF(g) → SiF₄(g) + 2 H₂O(l) ΔH°_rxn = -184 kJ

Calculate the amount of heat (in kJ) necessary to raise the temperature of 47.8 g benzene by 57.0 K.The specific heat capacity of benzene is 1.05 J/g°C

In the following reaction,energy is given off.Where does the energy go? C(s) +O₂ (g) = CO₂(g)

A motor does 30 kJ of work and loses 4 kJ as heat to the surroundings.What is the change in the internal energy of the motor?

Calculate the work done by the system when 2 moles of hydrogen gas is produced by the following reaction in a flask fitted with an inflatable balloon. Zn(s) +2HCl(aq) = ZnCl₂(aq) + H₂(g)

The enthalpy of combustion of gasoline (C₈H₁₈) is 5471 kJ mol^-1. How much heat will be produced by burning 1 gallon of gasoline at 25^°C? (Density of gasoline = 0.703 g/mL;1gallon = 3.78 L)

Which of the following signs on q and w represent a system that is doing work on the surroundings,as well as gaining heat from the surroundings?

The specific heat capacity of liquid water is 4.18 J/g ∙ K.How many joules of heat are needed to raise the temperature of 5.00 g of water from 25.1°C to 65.3°C?

Choose the thermochemical equation that illustrates ΔH°_f for Li₂SO₄.

Which of the following processes is endothermic?

An ice cube melts and cools the surrounding beverage.(The ice cube is the system. ) Which of the following statement is correct?

The combustion of titanium with oxygen produces titanium dioxide: Ti(s) + O₂(g) → TiO₂(s) When 2.060 g of titanium is combusted in a bomb calorimeter,the temperature of the calorimeter increases from 25.00°C to 91.60°C.In a separate experiment,the heat capacity of the calorimeter is measured to be 9.84 kJ/K.The heat of reaction for the combustion of a mole of Ti in this calorimeter is ________ kJ/mol.

Where does the energy absorbed during an endothermic reaction go?

Which of the following (with specific heat capacity provided) would show the smallest temperature change upon gaining 200.0 J of heat?