Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- A 4.77 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C. What is the change in temperature, in °C, inside the calorimeter? What quantity of heat, in J, was gained by the solution? Assume the specific heat of the solution is the same as water, 4.184 J/g・ °C.arrow_forwardA 36.0−g sample of an unknown metal at 99 ° C was placed in a constant-pressure calorimeter containing 90.0 g of water at 24.0 ° C. The final temperature of the system was found to be 28.4 ° C. Calculate the specific heat of the metal. (The heat capacity of the calorimeter is 13.4 J/ ° C.)arrow_forward2. Cold packs take advantage of the fact that dissolving NH4NO3 in water is an endothermic process. When 5.44 g of solid ammonium nitrate is added to 150.0 g of water in a coffee cup calorimeter, the temperature of the solution changes from 18.6 °C to a final temperature which you will determine. Calculate the enthalpy change for dissolving ammonium nitrate in water, in kJ/mol. Assume the specific heat of the solution is 4.2 J/g·K.g. Using the value of qsolution, calculate ∆T, as well as the final temperature reached by the solution.arrow_forward
- A student conducts a calorimetry experiment on an unknown metal object. The unknown metal object with a mass of 82.522 g is heated to 100.5 °C and then transferred to a coffee-cup calorimeter containing 67.225 g of water at 22.3 °C. If the metal object and the water reach a final temperature of 30.5 °C and the heat absorbed by the water was calculated to be 2310 J. What is the specific heat of this metal object? (The specific heat of water is 4.18 J/g°C)arrow_forwardA 4.81 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. What is the total mass inside the calorimeter in grams? What is the change in temperature, in °C inside the calorimeter ?arrow_forwardIn a coffee-cup calorimeter, 100 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCI are mixed. Both solutions were originally at (2.22x10^1) °C. After the reaction, the temperature is (2.9200x10^1) °C. Assuming all solutions have a density of 1.00 g/mL and a heat capacity of 4.18 J/°C.g, what is the enthalpy change for the neutralization of HCI by NaOH? Assume that no heat is lost to the surroundings or the calorimeter. Enter your answer in kJ. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: Answer x10 unitsarrow_forward
- If 0.066 mol of hydrochloric acid (HCl) is mixed with 0.066 mol of sodium hydroxide (NaOH) in a "coffee cup" calorimeter, the temperature of 5.0 g of the resulting solution increases from 25.0°C to 30.0°C. Given that the energy released is 1.2 × 101 cal when the specific heat of the resulting solution is 1.00 cal/g−°C, use a conversion factor to convert the energy released to joules (J). Enter your answer in scientific notation. Be sure to answer all parts.arrow_forwardThe combustion of propane (C3H8) produces 2220 kJ of energy per mole of propane consumed. What mass in grams of propane will be required to heat 55.0 gal of bathtub water from 25.0°C to 35.0°C if the process is 80.0% efficient? (1 gal = 3.785 L, 1 cal = 4.184 J, the density of water is 1.00 g/mL, the specific heat of water is 1.00 cal/(g°C)arrow_forwardIn a coffee-cup calorimeter, 110.0 mL of 1.3 M and 110.0 mL of 1.3 M are mixed. Both solutions were originally at 22.2°C. After the reaction, the final temperature is 30.9°C. Assuming that all the solutions have a density of 1.0 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.arrow_forward
- 150. g of water (Cs = 4.184 J/g°C) at 20.0 °C is added to a coffee cup calorimeter. A 35.0 g sample of silver (Cs = 0.129 J/g°C) is then placed into the water. At thermal equilibrium, the temperature of the calorimeter is 22.07 °C. What was the initial temperature of the silver sample?arrow_forwardConsider the following reaction: 2 Mg(s) + O2(g) --> 2 MgO(s) ΔH = - 1204 kJ/rxn Is this reaction exothermic or endothermic? Describe what you observed when you did this reaction in the lab and what physical observations you made to confirm your answer. Calculate the enthalpy change when 0.20 grams of Mg(s) reacts. How many kJ are required to decompose 1.25 grams of MgO at constant pressure?arrow_forward2) When 100 g of unknown metal at 100 °C added to a calorimeter containing 50.00 g of water the temperature rises from 24.00°C to 36.54°C. Calculate the specific heat of the unknown metal in J/°C. The specific heat of water is 4.184 J/g °C.arrow_forward
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