A student wishes to determine the specific heat capacity of a certain material. After she places 5.000 g of the material at 95.10 °C to 50.0 g of water, already in the calorimeter, at 26.80 °C, the final temperature of the system is 34.70 °C. What is the specific heat capacity of the material? (specific heat capacity of water = 4.184 J/g•"C) Select one: O a. 0.183 J/g•°C O b. 0.754 J/g.°C O c. 320 J/g•°C O d. 5.47 J/g•°C One of the stages in obtaining iodine from oil brines is the conversion of aqueous iodide (as Fel,) to solid iodine in the presence of chlorine gas. The other product of this reaction is aqueous ferric chloride. Which is the correct balanced chemical equation for this process? Select one: O a. 2 Fel2(aq) + 3 Cl2íg) → 2 FeCla(aq) + 2 l2(s) O b. Felz(aq) + Cl2(g) → FeCla(aq) + \z{g) Oc. Felz(ag) + Cl2(s) → FeCla(aq) + Iz(g) O d. 3 Fel2(aq) +2 Cl2(s) → 2 Fecla(aq) + 3 I2(s)

A student wishes to determine the specific heat capacity of a certain material. After she places 5.000 g of the material at 95.10 °C to 50.0 g of water, already in the calorimeter, at 26.80 °C, the final temperature of the system is 34.70 °C. What is the specific heat capacity of the material? (specific heat capacity of water = 4.184 J/g•"C) Select one: O a. 0.183 J/g•°C O b. 0.754 J/g.°C O c. 320 J/g•°C O d. 5.47 J/g•°C One of the stages in obtaining iodine from oil brines is the conversion of aqueous iodide (as Fel,) to solid iodine in the presence of chlorine gas. The other product of this reaction is aqueous ferric chloride. Which is the correct balanced chemical equation for this process? Select one: O a. 2 Fel2(aq) + 3 Cl2íg) → 2 FeCla(aq) + 2 l2(s) O b. Felz(aq) + Cl2(g) → FeCla(aq) + \z{g) Oc. Felz(ag) + Cl2(s) → FeCla(aq) + Iz(g) O d. 3 Fel2(aq) +2 Cl2(s) → 2 Fecla(aq) + 3 I2(s)

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.104PAE: 9.104 An engineer is using sodium metal as a cooling agent in a design because it has useful thermal...

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9.50 When a 13.0-g sample of NaOH(s) dissolves in 400.0 mL of water in a coffee cup calorimeter, the temperature of the water changes from 22.6°C to 30.7C Assuming that the specific heat capacity of the solution is the same as for water, calculate (a) the heat transfer from system to surroundings and (b) H for the reaction NaOH(s)Na+(aq)+OH(aq)
A piece of titanium metal with a mass of 20.8 g is heated in boiling water to 99.5 C and then dropped into a coffee-cup calorimeter containing 75.0 g of water at 21.7 C. When thermal equilibrium is reached, the final temperature is 24.3 C. Calculate the specific heat capacity of titanium.
9.104 An engineer is using sodium metal as a cooling agent in a design because it has useful thermal properties. Looting up the heat capacity, the engineer finds a value of 28.2 J mol-l °C-l. Carelessly, he wrote this number down without units. As a result, it was later taken as specific heat. (a) What would he the difference between these two values? (b) Would the engineer overestimate the ability of sodium to remove heat from the system or underestimate it because of this error? Be sure to explain your reasoning.
A sample of 0.562 g of carbon is burned in oxygen in a bomb calorimeter, producing carbon dioxide. Assume both the reactants and products are under standard state conditions, and that the heat released is directly proportional to the enthalpy of combustion of graphite. The temperature of the calorimeter increases from 26.74 C to 27.93 C. What is the heat capacity of the calorimeter and its contents?
Nitrogen gas (2.75 L) is confined in a cylinder under constant atmospheric pressure (1.01 105 pascals). The volume of gas decreases to 2.10 L when 485 J of energy is transferred as heat to the surroundings. What is the change in internal energy of the gas?
A 5.00-g sample of aluminum pellets (specific heat capacity = 0.89 J/C g) and a 10.00-g sample of iron pellets (specific heat capacity = 0.45 J/C g) are heated to 100.0C. The mixture of hot iron and aluminum is then dropped into 97.3 g water at 22.0C. Calculate the final temperature of the metal and water mixture, assuming no heat loss to the surroundings.
Nitrogen gas is confined in a cylinder with a movable piston under a constant pressure of 9.95 104 Pa. When 695 J of energy in the form of heat is transferred from the gas to the surroundings, its volume decreases by 1.88 L. What is the change in internal energy of the gas?
How much heat is produced when loo mL of 0.250 M HCl (density, 1.00 g/mL) and 200 mL of 0.150 M NaOH (density, 1.00 g/mL) are mixed? HCl(aq)+NaO(aq)NaCl(aq)+H2O(l)H298=58kJ If both solutions are at the same temperature and the heat capacity of the products is 4.19 J/g C, how much will the temperature increase? What assumption did you make in your calculation?
The addition of 3.15 g of Ba(OH)28H2O to a solution of 1.52 g of NH4SCN in loo g of water in a calorimeter caused the temperature to fall by 3.1 C. Assuming the specific heat of the solution and products is 4.20 J/g C, calculate the approximate amount of heat absorbed by the reaction, which can be represented by the following equation: Ba(OH)28H2O(s)+2NH4SCN(aq)Ba(SCN)2(aq)+2NH3(aq)+10H2O(l)
9.35 A piece of titanium metal with a mass of 20.8 g is heated in boiling water to 99.5°C and then dropped into a coffee cup calorimeter containing 75.0 g of water at 2 1.7°C. When thermal equilibrium is reached, the final temperature is 24.3°C. Calculate the specific heat capacity of titanium.
Ammonium nitrate is an oxidizing agent and can give rise to explosive mixtures. A mixture of 2.00 mol of powdered aluminum and 3.00 mol of ammonium nitrate crystals reacts exothermically yielding nitrogen gas, water vapor, and aluminum oxide. How many grams of the mixture are required to provide 245 kJ of heat? See Appendix C for data.