1. A 32.07 gram sample of vanadium was heated to 75 deg. It was then dumped in which the initial temperature of the water inside was 22.50 deg C. After the metal was allowed to release its heat to the calorimeter's water, 26.30 deg C was read to be the final temperature. What is the mass (g) of the water inside the calorimeter? Specific heat capacity of water and vanadium is 4.184 and 0.4886 J/g-C, respectively.

1. A 32.07 gram sample of vanadium was heated to 75 deg. It was then dumped in which the initial temperature of the water inside was 22.50 deg C. After the metal was allowed to release its heat to the calorimeter's water, 26.30 deg C was read to be the final temperature. What is the mass (g) of the water inside the calorimeter? Specific heat capacity of water and vanadium is 4.184 and 0.4886 J/g-C, respectively.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

a 30.0 g sample of chromium is heated to 100.0°C in a boiling water bath. the sample is added to a calorimeter charged with 45.0 mL of water at 34.1 °C. the final temp of the calorimeter contents is 38.5 °C. calculate the specific heat of chromium
A 30.0 g sample of chromium is heated to 100.0 °C in a boiling water bath. The sample is added to a calorimeter charged with 45.0 mL of water at 34.1 °C. The final temperature of the calorimeter contents is 38.5 °C. Calculate the specific heat of chromium.
A 1.595 g samples of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 23.67 degrees Celsius to 29.44 degrees Celsius. The heat capacity (calorimeter constant) of the calorimeter is 30.29 kJ/degrees Celsius, what is the heat of combustion per gram of the material?
10 A 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 37.48°C. The specific heat capacity of water is 4.184 J and the density of water is g. °C 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 = °C
A piece of molybdenum metal whose mass is 6.87 g is heated to 100.0 °C and then dropped into an ice calorimeter. As the molybdenum cools to 0.0°C, 0.513 g of ice melts (it takes 6.01 kJ of heat to melt exactly 1 mol of ice). What is the molar heat capacity (in J/mol·K) of molybdenum? i J/mol*K
22. A 44.97−g sample of water at 72.2°C is added to a sample of water at 25.7°C in a constant-pressure calorimeter. If the final temperature of the combined water is 38.4°C and the heat capacity of the calorimeter is 26.3 J/°C, calculate the mass of the water originally in the calorimeter.
75.0 mL of 1.80 M CuSO 4 solution is mixed with 150 mL of 1.80 M NAOH solution in a coffee cup calorimeter of negligible heat capacity. If the initial temperature of the two solutions are both 21.0 degrees C, and the final temperature of the mixed solution is 27.1, how much heat was released by the reaction? Assume density of solution d is 1.00 g/mL and that the solution has the same specific heat as water. The thermochemical equation is: CuSO4 (ag) + 2NAOH (ag) --> Cu(OH)2 (s) + Na SO4 (ag) AH xn = - 42.3 kJ/mol rxn Hint: no limiting reagent, substances are presented in correct molar ratios. O 6180 J O 9270 J O 3120 J O 5740 J O 9300 J O 1250 J O 6230 J O 3380 J
A piece of chromium metal with a mass of 24.50 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 23.4 °C. When thermal equilibrium is reached, the final temperature is 25.7 °C. Calculate the specific heat capacity of chromium. (The specific heat capacity of liquid water is 4.184 J/g ⋅ K.)
When 14.2 g KBr is dissolved in 100.0 g of water in a coffee-cup calorimeter, the temperature drops from 28.88 °C to 23.38 °C. What is the enthalpy change per gram of KBr dissolved in the water? Assume that the solution has a specific heat capacity of 4.18 J/g·K.
A sample of water in a constant pressure calorimeter has a temperature of 23.4 ̊C. (You may assume the heat capacity of the calorimeter is negligible). If you put 28.6 g of aluminum at a temperature of 96.2 ̊C into this water and the final temperature is 26.1 ̊C, what volume of water is in the calorimeter? You may assume the density of water is 1.00 g/mL.
A sample of aluminum, initially at 5.0 °C, was placed in 18.0 g of water, initially at 25.0 °C. The final temperature of the water and the metal was 21.0 °C. The specific heat of water is 4.184 J g-1 °c-1 and aluminum is 0.940 J g-1 °C-1. Ignore the heat capacity of the container. What is the mass (in g) of the aluminum?