6. A 40.00 g sample of water at 22.00°C is put in a calorimeter. After 60.00g of water at 65.00°C is added to the calorimeter, the mixture is stirred,and the final temperature is 47.00°C. Calculate the heat capacity of thecalorimeter in calfC.7. A piece of metal weighing 7.00 g is heated to 93.0°C and placed into thecalorimeter described in the previous problem. The calorimeter contains 25.0g of water at 30.0°C. If the final temperature of the water is 33.0°C, cal-culate the specific heat of the metal in cal/g °C.

(6) Given - Mass of water at 22.00°C = 40.00 g Mass of water at 65.00°C = 60.00 g Final…

6. A 40.00 g sample of water at 22.00°C is put in a calorimeter. After 60.00 g of water at 65.00°C is added to the calorimeter, the mixture is stirred, and the final temperature is 47.00°C. Calculate the heat capacity of th. calorimeter in calPC. 7. A piece of metal weighing 7.00 g is heated to 93.0°C and placed into the calorimeter described in the previous problem. The calorimeter contains 25. g of water at 30.0°C. If the final temperature of the water is 33.0°C, cal- ifin hoot off the metal in cal/g °C. 0uloto

6. A 40.00 g sample of water at 22.00°C is put in a calorimeter. After 60.00 g of water at 65.00°C is added to the calorimeter, the mixture is stirred, and the final temperature is 47.00°C. Calculate the heat capacity of th. calorimeter in calPC. 7. A piece of metal weighing 7.00 g is heated to 93.0°C and placed into the calorimeter described in the previous problem. The calorimeter contains 25. g of water at 30.0°C. If the final temperature of the water is 33.0°C, cal- ifin hoot off the metal in cal/g °C. 0uloto

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions

Section: Chapter Questions

Problem 39PS: A piece of titanium metal with a mass of 20.8 g is heated in boiling water to 99.5 C and then...

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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.
9.35 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.
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 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?
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.
A typical fat in the body is glyceryl trioleate, C57H104O6. When it is metabolized in the body, it combines with oxygen to produce carbon dioxide, water, and 3.022104 kJ of heat per mole of fat. (a) Write a balanced thermochemical equation for the metabolism of fat. (b) How many kilojoules of energy must be evolved in the form of heat if you want to get rid of five pounds of this fat by combustion? (c) How many nutritional calories is this? (1 nutritional calories =1103 calories)
When a 0.740-g sample of trinitrotoluene (TNT), C7H5N2O6, is burned in a bomb calorimeter, the temperature increases from 23.4 C to 26.9 C. The heat capacity of the calorimeter is 534 J/C, and it contains 675 mL of water. How much heat was produced by the combustion of the TNT sample?
The temperature of the cooling water as it leaves the hot engine of an automobile is 240 F. After it passes through the radiator it has a temperature of 175 F. Calculate the amount of heat transferred from the engine to the surroundings by one gallon of water with a specific heat of 4.184 J/g oC.
9.18 Calculate (a) q when a system does 54J of work and its energy decreases by 72 J and (b) E for a gas that releases 38 J of heat and has 102 J of work done on it.
The Group 2A carbonates decompose when heated. For example, MgCO3(s)MgO(s)+CO2(g) Use enthalpies of formation (see Appendix C) and calculate the heat required to decompose 10.0 g of magnesium carbonate.
Another reaction that is used to propel rockets is N2O4(l)+2N2H4(l)3N2(g)+4H2O(g) This reaction has the advantage that neither product is toxic, so no dangerous pollution is released. When the reaction consumes 10.0 g liquid N2O4, it releases 124 kJ of heat. (a) Is the sign of the enthalpy change positive or negative? (b) What is the value of H for the chemical equation if it is understood to be written in molar quantities?
Assume 200. mL of 0.400 M HCl is mixed with 200. mL of 0.400 M NaOH in a coffee-cup calorimeter The temperature of the solutions before mixing was 25.10 C; after mixing and allowing the reaction to occur, the temperature is 27.78 C. What is the enthalpy change when one mole of acid is neutralized? (Assume that the densities of all solutions are 1.00 g/mL and their specific heat capacities are 4.20 J/g K.)