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Practice Exercise 2
Given the following standard enthalpy change, use the standard enthalpies of formation in Table 5.3 to calculate the standard enthalpy of formation Of CuO(s):
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Chapter 5 Solutions
Chemistry: The Central Science, Books a la Carte Edition & Solutions to Red Exercises for Chemistry & Mastering Chemistry with Pearson eText -- Access Card Package
- Practice TEXT ANSWER A calorimeter holds 75 g water at 24.0°C. A sample of hot silver is added to the water. The final temperature of the water and silver is 28.0°C. What is the change in enthalpy associated with the change in the water's temperature? J FC Note: The specific heat of water is 4.18 gº Use the formula ΔΗ = = - cm ^T Show your work. H Normal X₂ X² 2 Ix Enter your answer here : A A ||| ||| e BIUS ×1arrow_forwardA scientist measures the standard enthalpy change for the following reaction to be 543.0 kJ : 2BRF3(g)- →Br2(g) + 3 F2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of Br2(g) is kJ/mol. Submit Answer Try Another Version 1 item attempt remainingarrow_forwardA scientist measures the standard enthalpy change for the following reaction to be -773.2 kJ : 2C0(g) + 2 NO(g)- →2CO2(g) + N2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CO2(g) is kJ/mol. Submit Answer Try Another Version 2 item attempts remainingarrow_forward
- Homework 3 • Use standard enthalpies of formation from Table 7.2 to determine the enthalpy change at 25 °C for the following reaction. 2 Cl2(g) + 2H20(1) 4 HCI( g) + O2(g) AH° = ?arrow_forwardExercise 9.42 Enhanced with Feedback and Hints MISSED THIS? Watch KCV 9.4, IWE 9.2; Read Section 9.4. You can click on the Review link to access the section in your e Text. Part A How much heat is required to warm 1.30 kg of sand from 30.0 °C to 100.0 °C? Express the heat in joules to three significant figures. » View Available Hint(s) ΑΣφ Jarrow_forwardBurning 1.09 g of a fuel causes the water in a calorimeter to increase by 14.7°C. If the calorimeter has a heat capacity of 3.09 kJ/°C, what is the energy density of the fuel (in kJ/g)? Type answer: CHECKarrow_forward
- Practice Exercise 2 Carbon occurs in two forms, graphite and diamond. The en- thalpy of the combustion of graphite is -393.5 kJ /mol, and that of diamond is -395.4 kJ/mol: C(graphite) + O2(g) → CO2(8) AH = -393.5 kJ - C(diamond) + O2(8) CO2(8) AH = -395.4 kJ - %3D Calculate AH for the conversion of graphite to diamond: C(graphite) C(diamond) AH = ? - %3Darrow_forwardA 150.9-g sample of a metal at 74.5°C is added to 150.9 g H2O at 15.1°C. The temperature of the water rises to 18.4°C. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the water. The specific heat capacity of water is 4.18 J/°C•g. Specific heat capacity J/°C•9 Submit Answer Try Another Version 3 item attempts remaining Not Visitedarrow_forwardQuestion 2 of 20 Attempt 3 If a system has 5.00 x 10 kcal of work done to it, and releases 5.00 x 10 kJ of heat into its surroundings, what is the change in internal energy (AE or AU) of the system? AE = 1000 uestion 2 of 2o If a system has 5.00 x 10 kcal of work done to it, and releases 5.00 x 10 kJ of heat into its surroundings, what is the change in internal energy (AE or AU) of the system? 1000 AE = Incorrect n s OT 2U At constant pressure, which of these systems do work on the surroundings? O2 A(g)+B(g) 2 A(g)+B(s) V 2 A(g)+B(g) C(g) - 4C(g) - 3 C(g) O A(g)+B(g) C(g) Incorrectarrow_forward
- Exercise 97 has a heat capacity of 6.66 KJ/ degree C.arrow_forward[References] It has been determined that the body can generate 5500 k) of energy during one hour of strenuous exercise. Perspiration is the body's mechanism for eliminating this heat. What mass of water would have to be evaporated through perspiration to rid the body of the heat generated during 2 hours of exercise? (The heat of vaporization of water is 40.6 kJ/mol.) Mass kg Submit Answer Try Another Version 2 item attempts remainingarrow_forwardSupplemental Exercise 1. The specific heat of copper is 0.385J/g°C, the specific heat of platinum is 0.133J/g°C, the specific heat of magnesium is 1.11J/g°C. If 100.g sample of each of these metals was heated to 100°C and dropped into a calorimeter with 100.g of water at 20°C. Which would have the highest final temperature? 2. If a student uses a very large piece of ice in part D, the ice might not completely melt and the thermometer might read 1°C at the end of the trial. Would this cause the magnitude of the calculated value of fusion to large or too small. Explain your reasoning.arrow_forward
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