A piece of metal with a mass of 22.9 g at 153.0°C is placed in a styrofoam cup containing 35.0 g of water at 23.6°C. Once the system has reached equilibrium, the final temperature of the water in 34.0°C. What is the specific heat of the metal to four significant digits? The specific hest of water is 4.18 - 508

A piece of metal with a mass of 22.9 g at 153.0°C is placed in a styrofoam cup containing 35.0 g of water at 23.6°C. Once the system has reached equilibrium, the final temperature of the water in 34.0°C. What is the specific heat of the metal to four significant digits? The specific hest of water is 4.18 - 508

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

Il Metro by T-Mobile 1:06 AM n 24% Question 15 of 35 Submit Specific Heat Capacity J/(g•°C) Metal Aluminum 0.90 Сopper 0.38 Iron 0.45 Magnesium 1.00 Silver 0.23 Tin 0.32 Titanium 0.52 A) Fe B) Sn C) Ag D) Cu Tap here or pull up for additional resources
A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.8608 g sample of glutaric acid (C3HgO4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.029x103 g of water. During the combustion the temperature increases from 25.01 to 27.84 °C. The heat capacity of water is 4.184 J gl°c-!. The heat capacity of the calorimeter was determined in a previous experiment to be 839.5 J°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of glutaric acid based on these data. C;HgO4(s) + 50,(g) 4 H,O(1) + 5 CO,(g) + Energy Molar Heat of Combustion = kJ/mol
What is the change in enthalpy for the reaction: 2B (s) + 3H2(g) → B2H6 (g) given these thermochemical equations? B2H6 (g) + 302 (g) →B2O3 (s) + 3 H₂O (g) AH = -2032 kJ 2B (s) + 3/2 O2 (g) → B2O3 (s) AH = -1272 kJ H2(g) + 1/2 O2 (g) → H2O (g) AH -241.8 kJ -4029 kJ +518.2 kJ +34.6 kJ -3546 kJ
Sucrose is common sugar. It is produced naturally in plants, from which table sugar is refined. A sample of sucrose (C12H22O11) with a mass of 2.68 g is burned in a bomb calorimeter. The heat capacity of this calorimeter is 8.91 kJ/°C. The temperature changes from 23.0°C to 30.5°C. Calculate the heat of combustion of sucrose in kilojoules per mole. Question options: a. -8.54 x 103 b. 4.64 x 105 c. 2.01x 10-4 d. -1.88 x 102
Chlorofluorocarbons are commonly used as Freon in refrigerators and air conditioners. Cooling the average dorm room from 35°C to 22°C requires the air conditioner to convert ~2700 g of C2Cl3F3 from a liquid at 24.7 °C to a gas at 87.0 °C. How much energy in kJ is absorbed by the chlorofluorocarbon when cooling this room? The chlorofluorocarbon C2Cl3F3 has a normal boiling point of 47.6 °C. The specific heat of the liquid is 0.91 J/g⋅K. The specific heat of the gas is 0.67 J/g⋅K. The heat of vaporization is 27.49 kJ/mol.
A 21.42g sample of an unknown metal was heated to 99.5ºC, and the added to 50.00g of water contained in a foam coffee cup. The initial temperature of the water was 20.5ºC, and the final temperature of the metal and water was 25.1ºC. The calorimeter constant for the coffee-cup calorimeter was 13.5 J/ºC. What was the specific heat of the metal? * the answer is 0.64 J/gºC, but I need to know how to get there
When 1.836 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?
Calculate the energy required to heat 874.0 mg of cyclohexane from 22.6 °C to 38.6 °C. Assume the specific heat capacity of cyclohexane under these conditions is 1.85 J-g K -1 -1 . Round your answer to 3 significant digits.
A 6.55 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. Wht is the change in teperature in celcios inside the calometer? was the dissolution process endothermic or exothermic? how much heat, in J, was hained b the solution? assume the specific heat of the solution is the same as water, 4.184 J/g. celcius
A 75g sample of a metal at temperature of 100℃ is placed in a calorimeter. The calorimeter contains 100g of water at a temperature of 34.4℃. The final temperature of the metal and the water in the calorimeter is 44.9℃. What is the specific heat of the metal? (cwater = 4.184J/g℃)
1.) The molar heat of combustion of octane to form carbon dioxide and water vapour is ─5470.1kJ/mol. Using this value, determine the mass of octane required to increase the temperature of 1.50 L of water from 22.0°C to 85.6°C. 2.) A simple calorimeter is filled with 250g of water initially at 25.0°C. A mass of 0.500g of benzene is completely burned to heat the water in the calorimeter. The highest temperature of the calorimeter water is measured at 44.0°C. What is the experimental value of the molar enthalpy of combustion of benzene?
A 39.7 g block of an unknown metal at 97.2°C is placed into 500.0 g of water initially at 17.0°C and has a final temperature of the water and the metal of 24.2°C. What is the specific heat capacity of the unknown metal in J/g･°C? The specific heat capacity of water is 4.184 J/g･°C.