2. A chemist designed an experiment to measure the heat transfer. She submerged a flask with chemical reaction inside into a water bath. She found that 66.4 kJ energy of heat flowed out of the water bath into the flask. The water bath contained 9.90 kg of water at 24.0 °C in the experiment. It is known that water has a specific heat of 4.184 J/g °C. Questions: i) ii) What is the final temperature of the water bath? For the chemical reaction in the flask, is it an endothermic or exotherm.c process?

2. A chemist designed an experiment to measure the heat transfer. She submerged a flask with chemical reaction inside into a water bath. She found that 66.4 kJ energy of heat flowed out of the water bath into the flask. The water bath contained 9.90 kg of water at 24.0 °C in the experiment. It is known that water has a specific heat of 4.184 J/g °C. Questions: i) ii) What is the final temperature of the water bath? For the chemical reaction in the flask, is it an endothermic or exotherm.c process?

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

the temperature of a silver coin decreases by 353°c as it releases 5,550 joules of heat. what is the mass of the coin? the specific heat of silver =0.34J/g°C
A calorimeter holds 50 g water at 29.0°C. A sample of hot iron is added to the water, and the final temperature of the water and iron is 22.0°C. What is the change in enthalpy associated with the change in the water's temperature? Note: The specific heat of water is 4.18 J/g°C.
A 45.90 g sample of pure copper is heated in a test tube to 99.40°C. The copper sample is then transferred to a calorimeter containing 61.04 g of deionized water. The water temperature in the calorimeter rises from 24.51°C to 29.10°C. The specific heat capacity of copper metal and water are J and 4.184 J respectively. g• °C 0.387 g• °C Assuming that heat was transferred from the copper to the water and the calorimeter, determine th heat capacity of the calorimeter. Heat capacity of calorimeter =
What is the specific heat of a metal with a mass of 14g,heat of 3.45kj and a change in temperature of 3.2 °c
How much heat, in joules and calories, is needed to heat up 253 mL of water from 13.3 °C to 85.2 °C? Assume the density of water to be 1.00 g/mL.
In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to Thermometer measure the energy of a solution phase reaction. Stirring rod A student heats 65.13 grams of copper to 98.95 °C and then drops it into a cup containing 84.76 grams of water at 23.02 °C. She measures the final temperature to be 27.86 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.60 J/°C. Water- Assuming that no heat is lost to the surroundings calculate the specific heat of copper. Metal sample Specific Heat (Cu) = J/g°C. 2000 Thomson-BrooksCole
In an experiment, 26.5 g of metal was heated to 98.0°C and then quickly transferred to 150.0 g of water in a calorimeter. The initial temperature of the water was 22.5°C, and the final temperature after the addition of the metal was 32.5°C. Assume the calorimeter behaves ideally and does not absorb or release heat.
Please help me complete this question
1 A piece of metal with a specific heat of 1.011 J/gºC is heated to 123.1ºC and then placed in 111.031 g of water which is at a temperature of 3.6 ºC. After a minute, the temperature of the water has stopped changing and is now 55.8ºC. Assuming that there are no heat losses to the container or surroundings, what is the mass of the piece of metal in grams? Assume that water has a specific heat of 4.184 J/gºC. Enter your answer with at least 3 sig figs.
Which of the reactions are exothermic? 2 Mg(s) + O,(g) → 2 MgO(s) + heat O NH, (g) + HCI(g) → NH,CI(s) + heat AgCl(s) + heat – Ag*(aq) + Cl¯(aq) 2 Fe, 0, (s) + 3 C(s) + heat → 4Fe(s) + 3 CO, (g) O C(graphite) + 0,(g) → CO,(g) + heat O CH, (g) + 20,(g) → CO,(g) + 2 H,O(1) + heat
A gas expands and does work on the surroundings equal to 4.92 Latm. At the same time, it releases 98.6 J of heat to the surroundings. What is the change in energy in J of the gas? (write the solution without decimals)
A 4.81 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. If 3.12 × 10³ J of heat was gained by the solution, what is the total heat for the dissolution reaction of the 4.81 g of salt? How many moles of the unknown salt were used in the reaction ? _______ J?