N OH AH = kJ b. Caa (PO4)2(s) + 3H2SO (1) 3CASO (s) +2H3PO4(1) AH" kJ %3D c. NH3 (g) + HCI(g) → NH4 C1(s) AH" = kJ

Use the following information to answer Questions 6-9: A sample of NH4NO3 with a mass of 5.0 g is dissolved in 40.1 g of deoinized water in a calorimeter.  The initial temperature of the water is 21.2 oC.  The final temperature of the solution is 15.4 oC.  The calorimeter constant = 25.2 J/oC.   If qH2O = -910 J and qcal = -130 J for 5.0 g of NH4NO3, calculate the heat of solution in J per gram of NH4NO3.

45 kJ of energy are associated with dissolving a certain amount of solid sodium hydroxide (NaOH) pellets in water. If the temperature of the resulting solution rises, which option best describes this process? Н20 NaOH(s) > NaOH(aq) AH px = -45 kJ/mol %3D rnx Н20 NaOH(s) – → Na*(aq) + O2(g) + H2(g) AH, nx = -45 kJ/mol Н20 Na(s) + H20(1) –→ Na*(aq) + OH¯(aq) AH, -45 kJ/mol rnx Н20 NaOH(s) > NAOH(s) AHnx = +45 kJ/mol rnx Н20 NaOH(s) > Na*(aq) + OH(aq) AHmx = +45 kJ/mol %3D rnx

A 28.79 g sample of a substance is initially at 21.2 ∘C. After absorbing 1817 J of heat, the temperature of the substance is 161.0 ∘C. What is the specific heat (SH) of the substance? SH = _____ J/g⋅∘C

9.)

When a 8.47 g sample of sodium iodide, NaI, dissolves in 160.0 g of water in a calorimeter, the temperature rises from 20.5 to 22.5°C.  The heat associated with this process is known as the heat of solution.  What is qsolution for this reaction  in kJ (not J) to 2 sig figs?

A chemist carefully measures the amount of heat needed to raise the temperature of a 0.38 kg sample of C,HgO, from 53.1 °C to 64.4 °C. The experiment shows that 6.73 × 10° J of heat are needed. What can the chemist report for the molar heat capacity of C,H,O,? Round your answer to 2 significant digits. | J- mol 1 - 1 ·K

Energy cannot be created nor destroyed, but it can be transferred between a system and its surroundings. The change in internal energy, AU, is positive if the system absorbs energy, and it is negative if the system releases energy. (Figure 1) The total change in internal energy is the sum of the heat, q, and work, w: AU =q+w. Figure 1 of 1 Surroundings AU pystem u System >0 Surroundings AU system System u <0 AU = q + w

Calculate the energy required to heat 593.0 g of cyclohexane from 11.1 °C to 35.6 °C. Assume the specific heat capacity of cyclohexane under these conditions -1 -1 is 1.85 J.g .K Round your answer to 3 significant digits. 0 0.0 X H 00 S

When methanol, CH, OH, is burned in the presence of oxygen gas, O₂, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH₂OH(g) + O₂(g) → CO₂(g) + 2 H₂O(1) AH = -764 kJ How much methanol, in grams, must be burned to produce 983 kJ of heat? mass: g