acellus_engine.html?ClassID=1463972376#A 50.0 g sample of unknown metal at 230.0 °C isplaced in a calorimeter containing 110. g of waterat 15.0 °C. The final temperature of thecombination is 19.3 °C. The heat capacity of thecalorimeter is 8.2 J/°C and the specific heatcapacity of the water is 4.18 J/g °C.What is the energy change for the calorimeter?acal = [? ] JEnter either a + or - sign AND the magnitude. Donot round.q,rxn (J)Enter03- 2033 Informational

Given, Heat capacity of calorimeter= 8.2J/g-°c Temperature difference = 19.3 - 15 = 4.3 °c

0.0 g sample of unknown metal at 230.0 °C ed in a calorimeter containing 110. g of wat at 15.0 °C. The final temperature of the mbination is 19.3 °C. The heat capacity of th alorimeter is 8.2 J/°C and the specific heat capacity of the water is 4.18 J/g °C. at is the energy change for the calorimeter acal = [?] J

0.0 g sample of unknown metal at 230.0 °C ed in a calorimeter containing 110. g of wat at 15.0 °C. The final temperature of the mbination is 19.3 °C. The heat capacity of th alorimeter is 8.2 J/°C and the specific heat capacity of the water is 4.18 J/g °C. at is the energy change for the calorimeter acal = [?] J

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 109AE: A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g...

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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.
A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g water at 23.5C. After the metal cools, the final temperature of metal and water mixture is 25.0C. If the specific heat capacity of nickel is 0.444 J/C g, what mass of nickel was originally heated? Assume no heat loss to the surroundings.
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In earlier times, ethyl ether was commonly used as an anesthetic. It is, however, highly flammable. When five milliliters of ethyl ether, C4H10O(l)(d=0.714g/mL), are burned in a bomb calorimeter, the temperature rises from 23.5C to 39.7C. The calorimeter contains 1.200 kg of water and has a heat capacity of 5.32 kJ/C. (a) What is qH2o? (b) What is qcal? (c) What is q for the combustion of 5.00 mL of ethyl ether? (d) What is q for the combustion of one mole of ethyl ether?
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