2. Calorimetry: A0.692 gram sample of glucose (Ct06) was hurned with excess oxygen in a bomb calorimeter. The calo. er contained 575. grams of water. The initial temperature of the calorimeter and the water was 21.70°C. The final temperature of the calorimeter and water was 25.22°C. a. Find the AH per 0.692 gram sample of glucose. b. Find the AH per mole of glucose.

2. Calorimetry: A0.692 gram sample of glucose (Ct06) was hurned with excess oxygen in a bomb calorimeter. The calo. er contained 575. grams of water. The initial temperature of the calorimeter and the water was 21.70°C. The final temperature of the calorimeter and water was 25.22°C. a. Find the AH per 0.692 gram sample of glucose. b. Find the AH per mole of glucose.

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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#18
22. Consider the following reaction. N2 + 3 H2 -> 2 NH3 ΔH = -92 kJ/mol How many grams of nitrogen gas react if 45 kJ of energy is released? A.4140 g B.148 g C.6.85 g D.13.6 g
Please answer question 20 part A
12. When 1.025 g of naphthalene (C10H8) is burned in a bomb calorimeter, the temperature rises from 24.25°C to 32.33°C. Find AEren for combustion of naphthalene in kJ/mol. Heat capacity of the calorimeter is 5.11 kJ/°C. 13. When 10.0 g of phosphorus is burned in oxygen gas to form solid P4O10, enough heat is generated to raise the temperature of 2960 g of water from 18.0°C to 38.0°C. Calculate the enthalpy of formation of solid P4O10 under these conditions.
A. Directions: Solve the following problem using the thermochemical equation. Write your answer on your answer sheet. 1. Using the following thermochemical equation, calculate how much heat is associated with the decomposition of 4 mol of NH.CI. NHJ + HCl - NH.Cl AH- -176 kJ 2. How many grams of Na are needed to make -550.0 kJ? Naw+ 3Ha + 2NHs AH - -92.6 kJ 3. Calculate the mass of ethane, CaHo which must be burned to produce 100 KJ of heat. 2C,Heg + 70ag - 4CO2g + 6H,O AH - -3120 KJ B. Calculate the enthalpy change of the reaction using Hess's Law. Write your answer on your answer sheet. 1. Calculate AH for the reaction CaHag + Ha -->C:Hoog, from the following data. C,Ha + 30a - 2COa + 2H,Om C;Hoe + 7/20a - 200a + 3H,O Hag + 1/20z - H20 AH - -1411. kJ/mole AH - -1560. kJ/mole AH - -285.8 kJ/mole 2. Calculate AH for the reaction 4NH3 + 50z0 - 4NO + 6H2O, from the following data. Na + Oz - 2NO Naw + 3Ha - 2NH 2Hay + Oz + 2H20 AH - -180.5 kJ/mole AH - -91.8 kJ/mole AH - -483.6 kJ/mole 3.…
History Bookmarks Window Help Sun Mar 27 10:53 PM cvg.cengagenow.com 中 [References] Use the References to access important values if needed for this question. Ignition wires heat Thermometer Stirrer A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of sample fuels and the energy content of foods. In an experiment, a 0.5650 g sample of quinizarin (C14H804) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.187×103 g of water. During the combustion the temperature increases from 23.98 to Water 26.55 °C. The heat capacity of water is 4.184 J gloC1. The heat capacity of the calorimeter was determined in a previous experiment to be 770.8 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of quinizarin based on these data. C14H804(s) + 1402(g) → 4 H20(1) + 14 CO2(g) + Energy Sample dish Burning sample Steel bomb Insulated outside chamber Molar Heat of…
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.
3. A certain quantity of nitrous oxide (laughing gas) expands, doing 144 J of work. At the same time, it absorbs 299 J of heat from the surroundings. Which ONE represents the change in internal energy of the nitrous oxide? A. B. C. D. E. -443 J -155 J OJ 155 J 443 J
pt pt pt pt pt pt pt pt pt pt pt pt pt pt You should use care when dissolving H₂SO4 in water because the process is highly exothermic. To measure the enthalpy change, 5.8 g of concentrated H₂SO4() was added (with stirring) to 140. g of water in a coffee-cup calorimeter. This resulted in an increase in temperature from 21.0 °C to 30.3 °C. Calculate the enthalpy change for the process H₂SO4(l) → H₂SO4 (aq), in kJ/mol. Assume the specific heat capacity of the solution is 4.2 J/g. K. Enthalpy change = kJ/mol ?
When one mole of calcium carbonate reacts with ammonia, solid calcium cyanamide, CaCN2 and liquid water are formed. The reaction absorbs 90.1 KJ of heat. a. Write a balanced thermochemical equation for the reaction. b. Calculate ∆H°f for calcium cyanamide.
An 87.9 g sample of chromium metal at 99.1°C is placed in a calorimeter containing 100.00 g of water at 21.0°C The contents of the calorimeter come to a temperature of 25.7°C. The heat capacity of water is 4.18 J/(g* °C) a. Is this process exothermic or endothermic? b. Calculate the amount of heat released by the metal (q metal) in Joules. Show your work.
Which one of the following statements is not correct? Select one: a. In any physical process, such as dew forming on grass or carbon dioxide subliming, the internal energy of the system does not change. b. When dew forms on grass overnight, the energy of the water molecules decreases. c. When dry ice sublimes to form CO2(g), the energy of the carbon dioxide increases. d. When dew forms on grass overnight, the energy of the surroundings (grass, air, etc.) increases. e. When dry ice sublimes to form CO2(g), the internal energy of the surroundings decreases.