Give Up? Resources 9.4% ore: Hint f8 Given that AH [CI(g)] = 121.3 kJ-mol1 f. AH [C(g)] = 716.7 kJ-mol 1 AH CCI, (g)] = -95.7 kJ-mol ! calculate the average molar bond enthalpy of the carbon-chlorine bond in a CCl, molecule. ДНо CI kJ mol Question Source: MRG-General Chemistry about us privacy policy careers terms of use help contact us

Give Up? Resources 9.4% ore: Hint f8 Given that AH [CI(g)] = 121.3 kJ-mol1 f. AH [C(g)] = 716.7 kJ-mol 1 AH CCI, (g)] = -95.7 kJ-mol ! calculate the average molar bond enthalpy of the carbon-chlorine bond in a CCl, molecule. ДНо CI kJ mol Question Source: MRG-General Chemistry about us privacy policy careers terms of use help contact us

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

?
Can you help me?
Consider the following reactions: AH = -393.5 kJ + O2(g) CO 2(9) (graphite) AH = -285.8 k) + V2 O2(g) H2(9) AH = -726.4 k CH,OH + 3/2 0, CO2(9) + 2H,0) (1) Choose... Calculate the enthalpy change for the following reaction: CH;OH) (graphite) + 2 H2(g) + 2 02
You are given the following average bond energies:H-H 436 kJ/molH-X 431 kJ/molH-C 414 kJ/molC-X 339 kJ/molX-X 243 kJ/molBalance the following chemical reaction and compute the estimated heat of reaction using the values above.CH4(g) + X2(g) → CH1X3(g) + HX (g)
2. Calculate the heat evolved by 4.5 g of propane from the equation C, He + 502 3CO2 + 4 H,O From the following data AH in kJ/mol C3 H = - 2043 CO = - 393.5 %3D H,O = - 255.83 %D
changé if 1.25 g of NO is completely converted into NO,? #36. Acetic acid, CH3CO2H, is made industrially by the reaction by the reaction of methanol and carbon monoxide. CH3OH(I) + CO2(g) CH;CO2H (1) H= -134,6 KJ/mol-rxn What is the enthalpy change for producing 1.00L of acetic acid ( d= 1.044g/mL) by this reaction? Op
28. Write the equation that corresponds to the standard enthalpy of formation for each of the following compounds: a) NaI(s), b) HC1O,(g), and c) CH;OCH;(g)
A east.cengagenow.com/ilrn/takeAssignment/takeCXPCompliantActivity.do?locator=Dassignment-take References Use the References to access Important values If needed for this question. A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.5021 g sample of heptadecanoic acid (C,,H,0,) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.246x10 g of water. During the combustion the temperature increases from 21.91 to 25.07 °C. The heat capacity of water is 4.184 Jg1°C1. tin The heat capacity of the calorimeter was determined in a previous experiment to be 822.9 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of heptadecanoic acid based on these data. Cmbe te car C,,H3402(s) + (49/2) O2(g) → 17 H2O(1) + 17 CO2(g) + Energy kJ/mol Molar Heat of Combustion = Save and Exit Cengage Learning | Cengage…
Use the data below to calculate the bond energy for a C-F bond in kJ/mol. Bond Energy (kJ/mol) С-Н 413 H-F 567 С-С 347 H-CI .431 F-F 159 H-Br 364 Cl-CI 243 H-I 297. Br-Br 193 I-I 151 The reaction shown below has AH = -3372 kJ as written C2H6lg) + 7 F2(g) → 2 CF4(g) + 6 HFig) In C2H6 each C makes 3 bonds with H and 1 bond with C 485 kJ/mol O 489 kJ/mol O -503 kJ/mol O none of the answers are correct
The combustion of 0.1566 g benzoic acid increases the temperature of a bomb calorimeter by 2.51°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) Heat capacity = kJ/°C A 0.2195-g sample of vanillin (Cg H3 O3) is then burned in the same calorimeter, and the temperature increases by 3.21°C. What is the energy of combustion per gram of vanillin? Energy = kJ/g Per mole of vanillin? Energy = kJ/mol
6. Calculate the AH for the reaction: 7. CS2 (1) + 2 O2 (g) → CO2 (g) + 2 SO2 (g) Given: AHCO2 (g) = - 393.5 kJ/mol; AHSO2 = -296.8 kJ/mol; %3D AHCS2 (1) = 87.9kJ/mol
2. Acetylene is commonly used in welding torches and is known for burning very hot. Given the heats of formation in the table below, calculate the heat of combustion of acetylene in excess oxygen. Substance C₂H2 H₂O CO₂ Standard Heat of Formation +226.7 kJ/mol -285.8 kJ/mol -393.509 a. Find the heat of combustion of one mole of acetylene in oxygen: C₂H2 + 5/2 02 ----> 2CO₂+ H₂O b. An acetylene tank, like many others of gas we use in the lab, is often pressurized. If a 4L tank containing pure acetylene at 298 K is pressurized to 10 atm, how much heat will be released if a welder burns all of it on a single job?