A 28.5 g piece of gold is heated and then allowed to cool. What is the change in temperature (°C) if the gold releases 0.290 kJ of heat as it cools? The molar heat capacity of gold is 25.4 J/mol･°C.
1 . A 28.5 g piece of gold is heated and then allowed to cool. What is the change in temperature (°C) if the gold releases 0.290 kJ of heat as it cools? The molar heat capacity of gold is 25.4 J/mol･°C.
2. 3.15 mol of an unknown solid is placed into enough water to make 150.0 mL of solution. The solution's temperature increases by 15.41°C. Calculate ∆H, in kJ/mol, for the dissolution of the unknown solid. (The specific heat of the solution is 4.184 J/g･°C and the density of the solution is 1.20 g/mL).
3. Using the equations 2 Fe (s) + 3 Cl₂ (g) → 2 FeCl₃ (s) ∆H° = -800.0 kJ/mol Si(s) + 2 Cl₂ (g) → SiCl₄ (s) ∆H° = -640.1 kJ/mol Determine the molar enthalpy (in kJ/mol) for the reaction 3 SiCl₄ (s) + 4 Fe (s) → 4 FeCl₃ (s) + 3 Si (s)
4. A sample of 2.30 g of potato chips was burned in a calorimeter. The calorimeter was calibrated to have a heat capacity of 6.94 kcal/°C. The heat released caused the temperature of the calorimeter to increase 1.75°C. Calculate the food caloric content of the potato chips in nutritional calories per gram to three significant figures. Recall that 1 nutritional calorie (Cal) = 1 kcal.
5. Calculate the heat in kJ of combusting 1.0000 mol of cetane (C₁₆H₃₄), an analogous component in diesel fuel to octane in gasoline, given the following standard enthalpies of formation: CO₂(g) = -393.5 kJ/mol H₂O(l) = -285.8 kJ/mol C₁₆H₃₄(s) = -458.3 kJ/mol
6. In the following reaction, what is the quantity of heat (in kJ) released when 4.93 moles of CH₄ are burned? CH₄ (g) + 2 O₂ (g) → CO₂ (g) + 2 H₂O(g) ∆H° = -802 kJ/mol
7. The ∆Hvap for benzene is 30.7 kJ/mol at its boiling point of 80.0 °C. Calculate w for the vaporization of one mole of benzene at this temperature.
8. For the following combustion reaction CH₃COCH₃(l) + 4O₂(g) → 3CO₂(g) + 3H₂O(g) ∆H = -1.79 × 10³ kJ When a 20.6-g sample of acetone (molar mass = 58.08 g/mol) is burned, how much energy (in kJ) is released as heat?
9. If a system has 30.5 J of heat added to it, and the system does 75.5 J of work on its surroundings, what is the change in the internal energy of the system, in J?
10. Use the following table of bond energies to calculate the heat in kJ of combusting 1.000 mol of acetylene (C₂H₂) gas in oxygen, based on the following chemical equation: C₂H₂(g) + 2.5O₂(g) → 2CO₂(g) + H₂O(g)
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