Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- A piece of chromium metal with a mass of 24.64 g is heated in boiling water to 98.3 °C and then dropped into a coffee-cup calorimeter containing 82.3 g of water at 22.6 °C. When thermal equilibrium is reached, the final temperature is 25.0 °C. Calculate the specific heat capacity of chromium. (The specific heat capacity of liquid water is 4.184 J/g ⋅ K.)arrow_forwardA student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 38.86°C. The specific heat capacity of water is 4.184 J g.°C and the density of water is g 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = = °Carrow_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
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