Macmillan Learning Suppose a student performed an experiment similar to Experiment 1 and collected the data shown in the table. mass of cold water in the calorimeter initial temperature of the cold water mass of hot water added to the calorimeter initial temperature of the hot water final temperature in the calorimeter 24.000 g 21.5°C 24.000 g 71.0°C 45.1 °C Calculate the calorimeter constant for the calorimeter the student used in the experiment.

Macmillan Learning Suppose a student performed an experiment similar to Experiment 1 and collected the data shown in the table. mass of cold water in the calorimeter initial temperature of the cold water mass of hot water added to the calorimeter initial temperature of the hot water final temperature in the calorimeter 24.000 g 21.5°C 24.000 g 71.0°C 45.1 °C Calculate the calorimeter constant for the calorimeter the student used in the experiment.

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 103AE: The bomb calorimeter in Exercise 102 is filled with 987 g water. The initial temperature of the...

See similar textbooks

Similar questions

A sample of 0.562 g of carbon is burned in oxygen in a bomb calorimeter, producing carbon dioxide. Assume both the reactants and products are under standard state conditions, and that the heat released is directly proportional to the enthalpy of combustion of graphite. The temperature of the calorimeter increases from 26.74 C to 27.93 C. What is the heat capacity of the calorimeter and its contents?
Fructose is a sugar commonly found in fruit. A sample of fructose, C6H12O6, weighing 4.50 g is burned in a bomb calorimeter that contains 1.00 L of water (d=1.00g/mL). The heat capacity of the calorimeter is 16.97 kJ/PC. The temperature of the calorimeter and water rise from 23.49C to 27.72C. (a) What is q for the calorimeter? (b) What is q for water in the calorimeter? (c) What is q when 4.50 g of fructose are burned in the calorimeter? (d) What is q for the combustion of one mole of fructose?
How much heat is produced by combustion of 125 g of methanol under standard state conditions?
Indicate which state function is equal to heat, q, for each process described. a. The ignition of a sample in a bomb calorimeter, an unyielding, heavy metal chamberin which samples are burned for heat content analysis b.The melting of an icecube in a cup c.The cooling down ofthe inside of arefrigerator d.A fire in a fireplace
Determine whether the statements given below are true or false. Consider an endothermic process taking place in a beaker at room temperature. (a) Heat flows from the surroundings to the system. (b) The beaker is cold to the touch. (c) The pressure of the system decreases. (d) The value of q for the system is positive.
Quinone is an important type of molecule that is involved in photosynthesis. The transport of electrons mediated by quinone in certain enzymes allows plants to take water, carbondioxide, and the energy of sunlight to create glucose. A 0.1964-g sample of quinone (C6H4O2) is burned in a bomb calorimeter with a heat capacity of 1.56 kJ/C. The temperature of the calorimeter increases by 3.2C. Calculate the energy of combustion of quinone per gram and per mole.
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.
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?
Explain how calorimetry works to calculate H or E for a reaction. Does the temperature of the calorimeter increase or decrease for an endothermic reaction? For an exothermic reaction? Explain.
A 21.3-mL sample of 0.977 M NaOH is mixed with 29.5 mL of 0.918 M HCl in a coffee-cup calorimeter (see Section 6.6 of your text for a description of a coffee-cup calorimeter). The enthalpy of the reaction, written with the lowest whole-number coefficients, is 55.8 kJ. Both solutions are at 19.6C prior to mixing and reacting. What is the final temperature of the reaction mixture? When solving this problem, assume that no heat is lost from the calorimeter to the surroundings, the density of all solutions is 1.00 g/mL, the specific heat of all solutions is the same as that of water, and volumes are additive.
The reaction of 50 mL of acid and 50 mL of base described in Example 5.5 increased the temperature of the solution by 6.9 degrees C. How much would the temperature have increased if loo mL of acid and 100 mL of base had been used in the same calorimeter starting at the same temperature of 22.0 C? Explain your answer.