Mass of aluminum 16.27 g Initial temperature of Al 83.85°C Volume of water 52.4 mL Initial temperature of water 20.30°C Final water temperature 23.90°C g 1.00 mL Density of water J 4.184 g• °C Specific heat of water J 22.44 °C Calorimeter constant A student adds a heated sample of pure aluminum metal to a Styrofoam coffee cup calorimeter containing deionized water. Use the collected data to answer the following questions. (a) Assuming that heat was transferred from the aluminum to the water and the calorimeter, determine the specific heat of aluminum. J Specific heat of Al = g· °C (b) The actual specific heat of aluminum is 0.900 J Calculate the percent error for the g· °C' experimentally determined specific heat. Percent error = %

Mass of aluminum 16.27 g Initial temperature of Al 83.85°C Volume of water 52.4 mL Initial temperature of water 20.30°C Final water temperature 23.90°C g 1.00 mL Density of water J 4.184 g• °C Specific heat of water J 22.44 °C Calorimeter constant A student adds a heated sample of pure aluminum metal to a Styrofoam coffee cup calorimeter containing deionized water. Use the collected data to answer the following questions. (a) Assuming that heat was transferred from the aluminum to the water and the calorimeter, determine the specific heat of aluminum. J Specific heat of Al = g· °C (b) The actual specific heat of aluminum is 0.900 J Calculate the percent error for the g· °C' experimentally determined specific heat. Percent error = %

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...

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ALab Data Temperature of cold water (°C) Temperature of hot water (°C) Volume of cold water (mL) Volume of hot water (mL) Final temperature after mixing (°C) Mass of cold water (g) Mass of hot water (g) Calorimeter constant (J/°C) 4.0 87.0 98.0 83.0 41.0 98.0 83.0 How to calculate the calorimeter constant Sm -
9. A researcher sets out to calibrate a solution calorimeter. The researcher first adds a 75.000 mL sample of water to the calorimeter, measuring a temperature of 22.4°C after the water and calorimeter reach thermal equilibrium. The re- searcher then heats a separate 75.00 mL sample of water to 40.1°C and adds this sample to the previous one in the calorimeter. After the water has mixed and a new thermal equilibrium with the calorimeter is reached, a temperature of 27.0°C is measured. What is the heat capacity of the calorimeter?
4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6
Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 24.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 24.0 L. -23.0 W = Now calculate the work done if this process is carried out in two steps. 1. First, let the gas expand against a constant external pressure of 1.50 atm to a volume of 16.0 L. 2. From the end point of step 1, let the gas expand to 24.0 L against a constant external pressure of 1.00 atm. W = J J
Q5 a)A chemical reaction is run in which 465 Joules of heat are generated and the internal energy changes by -27 Joules. Calculate w for the system. w = Joules b)A chemical reaction is run in which 571 Joules of work is done by the system and the internal energy changes by + 95 Joules. Calculate q for the system. q = Joules c)A chemical reaction is run in which 365 Joules of heat are generated and 390 Joules of work are done by the system. Calculate the change in the internal energy of the chemical system.U = Joules
Measurements show that the enthalpy of a mixture of gaseous reactants decreases by 160. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 194. kJ of work is done on the mixture during the reaction. Calculate the change in energy of the gas mixture during the reaction. Be sure your answer has the correct number of significant digits. O exothermic Is the reaction exothermic or endothermic? O endothermic
One day while camping, a student used a propane stove to boil some water. The student heated 5.00 L of water from 15.6°C to 98.5°C. The molar enthalpy of combustion of propane is -2043.9 kJ/mol and heating the water required 1.38 mol of propane. Determine the efficiency of the propane camp stove if the heat released from the stove was used to heat the water. 62.4 % 38.4% D162 % 61.6%
To calibrate a calorimeter, 10.0 ml of 1.0 M NaOH and 5.0 ml of 1.0 M HCl was used in a calorimetry experiment. Which of the following will have NO EFFECT on the calculated heat capacity of the calorimeter, Ccal? a. Accidentally adding HNO3 instead of HCl. b.Adding a smaller volume of 1.0 M HCl. c.Using a bigger styrofoam ball for calibration. d.Using a wet test tube for calibration.
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
Consider the following reaction: 2 Mg + O22 MgO AH xn=-1203 kJ Calculate the amount of heat (in kJ) associated with complete reaction of 97.2 grams of Mg. O-3862 kJ O-4812 kJ O-601.5 kJ -2406 kJ O-1203 kJ 13
General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 24.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 24.0 L. w = J Now calculate the work done if this process is carried out in two steps. 1. First, let the gas expand against a constant external pressure of 1.50 atm to a volume of 16.0 L. 2. From the end point of step 1, let the gas expand to 24.0 L against a constant external pressure of 1.00 atm. w = J
A student is attempting to determine the heat capacity of a Styrofoam cup calorimeter by pouring hot water into a Styrofoam cup containing cold water. The student determined the mass of the cold water to be 21.2455 g and its initial temperature to be 20.36 °C. The mass of the hot water was 24.2646 g and its initial temperature as 34.54 °C. The final temperature of the water after mixing was determined to be 24.57°C. The specific heat capacity of the water is 4.184 J/(g•°C). What is the heat capacity of the Styrofoam cup calorimeter? Assume the temperature of the calorimeter is the same temperature as the cold water. 4.184 J/°C 132.5 J/°C