Chapter 9: Problem 12
Are kinetic energy and potential energy both state functions?
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Chapter 9: Problem 12
Are kinetic energy and potential energy both state functions?
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A 100.0 mL sample of \(1.0 \mathrm{MNaOH}\) is mixed with \(50.0 \mathrm{mL}\) of \(1.0 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) in a large Styrofoam coffee cup; a thermometer is mounted in the lid of the cup to measure the temperature of the contents. The temperature of each solution before mixing is \(22.3^{\circ} \mathrm{C} .\) After mixing, their temperature reaches \(31.4^{\circ} \mathrm{C} .\) Assume that (1) the density of the mixed solutions is \(1.00 \mathrm{g} / \mathrm{mL},(2)\) the specific heat of the mixed solutions is \(4.18 \mathrm{J} /\left(\mathrm{g} \cdot^{\circ} \mathrm{C}\right),\) and (3) no heat is lost to the surroundings. a. Write a balanced chemical equation for the reaction that takes place in the cup. b. Is any \(\mathrm{NaOH}\) or \(\mathrm{H}_{2} \mathrm{SO}_{4}\) left in the cup when the reaction is over? c. Calculate the enthalpy change per mole of \(\mathrm{H}_{2} \mathrm{O}\) produced in the reaction.
An expanding gas does \(150.0 \mathrm{J}\) of work on its surroundings at a constant pressure of 1.01 atm. If the gas initially occupied \(68 \mathrm{mL},\) what is the final volume of the gas?
Calculate \(\Delta H_{\mathrm{rxn}}^{\circ}\) for the reaction $$2 \mathrm{Ni}(s)+\frac{1}{4} \mathrm{S}_{8}(s)+3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{NiSO}_{3}(s) \quad \Delta H_{\mathrm{rxn}}^{\circ}=?$$ from the following data: (1) \(\mathrm{NiSO}_{3}(s) \rightarrow \mathrm{NiO}(s)+\mathrm{SO}_{2}(g) \quad \Delta H_{\mathrm{rxn}}^{\circ}=156 \mathrm{kJ}\) (2) \(\frac{1}{8} S_{8}(s)+O_{2}(g) \rightarrow \operatorname{SO}_{2}(g) \quad \quad \Delta H_{\operatorname{rxn}}^{\circ}=-297 \mathrm{kJ}\) (3) \(\mathrm{Ni}(s)+\frac{1}{2} \mathrm{O}_{2}(g) \rightarrow \mathrm{NiO}_{2}(s) \quad \Delta H_{\mathrm{rxn}}^{\circ}=-241 \mathrm{kJ}\)
How are energy and work related?
Use standard enthalpies of formation from Appendix 4 to calculate the standard enthalpy of reaction for the following methane-generating reaction of methanogenic bacteria, given \(\Delta H_{f}^{\circ}\) of \(\mathrm{CH}_{3} \mathrm{NH}_{2}(g)=-22.97 \mathrm{kJ} / \mathrm{mol}:\) $$4 \mathrm{CH}_{3} \mathrm{NH}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow 3 \mathrm{CH}_{4}(g)+\mathrm{CO}_{2}(g)+4 \mathrm{NH}_{3}(g)$$
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