A student performs a calorimetry experiment. The student combines 100. g of 0.40 M HC1(aq) with 100. g of 0.40 M NAOH(ag). Data are given in the table. Temperature of HCI(ag) before mixing 25.0°C Temperature of NaOH(ag) before mixing 25.0°C Temperature of solution after mixing 27.8°C The value of q for the experiment is closest which of the following? (Assume that the heat capacity of the solution is the same as the heat capacity of water.) 560 J B) 1200 J c) 2300 J D 5900 J

6

When 145 mL of 0.212 M NaCl(aq) and 145 mL of 0.212 M AgNO3(aq), both at 21.1°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 23.7°C as solid AgCl forms. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) This precipitation reaction produces 3.14 ✕ 103 J of heat, assuming no heat is absorbed by the calorimeter, no heat is exchanged between the calorimeter and its surroundings, and that the specific heat and density of the solutions are the same as those for water (4.18 J/g·°C, and 0.997 g/mL, respectively). Using this data, calculate ΔH in kJ/mol of AgNO3(aq) for the given reaction.

In a Calorimetry experiment, a chemical reaction causes the temperature of the solution in the chamber to raise from 20.1 °C to 69.3 °C. Knowing that the solution weights 600. g, and specific heat of the solution is 4.18 J g–1 K–1, the heat released by the reaction is ______ .

A sample of 27.8 g of ammonium nitrate, NH4NO3, was dissolved in 130.2 g of water in a coffee cup calorimeter. The temperature changed from 28.94 °C to 16.51 °C. Calculate the heat of solution of ammonium nitrate in kJ/mol. Assume that the energy exchange involves only the solution and that the specific heat of the solution is 4.18 J/g°C. Heat of solution = i kJ/mol

A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with  22.4 mL  of  6.45 M  hydrochloric acid. The temperature of the mixture rises  17.2 ° C.  The density of the resulting solution is 1.00  g   mL  and has a specific heat capacity of 4.184  J   g  ·   ° C . The heat capacity of the calorimeter is 16.97  J   ° C .  Part 1:   (a) Identify the limiting reagent for the reaction.         Part 2:   (b) Calculate the heat of reaction (in J).    qrxn =      ×  10    JEnter your answer in scientific notation.   Part 3 out of 3   (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization =  ____ kj/mol

Consider these reactions: Reaction 1: H₂(g) + Cl₂(g) → 2HCl(g) Reaction 2: 20F₂ (g) → O₂(g) + 2 F₂ (g) Reaction 3: N₂(g) + 2O₂(g) → 2NO₂ (9) Use Reaction 1. AH = -184.6 kJ AH = -49.4 kJ AH = +66.4 kJ Determine the mass, in grams, of chlorine gas consumed (with excess H₂) when 1,861.0 kJ of energy is released from the system. Round to the nearest whole number. Answer:____ g

11.8 g of a soluble ionic compound is dissolved in 91.6 mL of water in a coffee-cup calorimeter, and the temperature of the solution changes from 24.80°C to 29.14°C. Assume the water has a density of 1.00 g/mL and that the total mass of the solution has the specific heat of water (4.186 J/g.K). Calculate the enthalpy change for the dissolution of this substance in kJ.

Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HCI(aq) → 2 MCl, (aq) + 3 H, (g) AH1 = -698.0 kJ HCl(g) → HCI(aq) AH = -74.8 kJ H, (g) + Cl, (g) → 2 HCl(g) AH3 = -1845.0 kJ MCI, (s) → MCI, (aq) AH = -292.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl, (g) → 2 MCI, (s) 2. 3. 4.

When 130. mL of 0.204 M NaCl(aq) and 130. mL of 0.204 M AgNO3(aq), both at 21.1°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 23.6°C as solid AgCl forms. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) This precipitation reaction produces 2.71x10³ J of heat, assuming no heat is absorbed by the calorimeter, no heat is exchanged between the calorimeter and its surroundings, and that the specific heat and density of the solutions are the same as those for water (4.18 J/g.°C, and 0.997 g/mL, respectively). Using this data, calculate AH in kJ/mol of AgNO3(aq) for the given reaction. 4.0✔✓ kJ/mol