A sample of solid biphenyl (C12H10) that weighs 0.4858 g is burned in an excess of oxygen to CO2(g) Ignition wires heat sample Thermometer and H20(,) in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.070 Stirrer °C. The heat capacity of the calorimeter and its contents is known to be 9.488×10³ J K-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank. Water Based on this experiment: (b) Assuming that AH° is approximately equal to AE, calculate the standard enthalpy change for the combustion of 1.000 mol of biphenyl to CO2(g) and H20( ). Insulated outside chamber Sample dish Burning sample Steel bomb kJ mol-! Combustion (bomb) calorimeter. (c) Calculate the standard enthalpy of formation per mole of biphenyl, using the following for the standard enthalpies of formation of CO2(g) and H20(). AH° H2O (2) = -285.83 kJ mol" ; AHº CO2(g) = -393.51 kJ mol" kJ mol-!

A sample of solid biphenyl (C12H10) that weighs 0.4858 g is burned in an excess of oxygen to CO2(g) Ignition wires heat sample Thermometer and H20(,) in a constant-volume calorimeter at 25.00 °C. The temperature rise is observed to be 2.070 Stirrer °C. The heat capacity of the calorimeter and its contents is known to be 9.488×10³ J K-1. (a) Write and balance the chemical equation for the combustion reaction. Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank. Water Based on this experiment: (b) Assuming that AH° is approximately equal to AE, calculate the standard enthalpy change for the combustion of 1.000 mol of biphenyl to CO2(g) and H20( ). Insulated outside chamber Sample dish Burning sample Steel bomb kJ mol-! Combustion (bomb) calorimeter. (c) Calculate the standard enthalpy of formation per mole of biphenyl, using the following for the standard enthalpies of formation of CO2(g) and H20(). AH° H2O (2) = -285.83 kJ mol" ; AHº CO2(g) = -393.51 kJ mol" kJ mol-!

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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Part B 2.0000 g of the unknown compound is burned in a bomb calorimeter. During the combustion, the temperature of the calorimeter increases from 23.125°C to 28.997 °C. During calibration, the heat capacity of the calorimeter was found to be 9.9897kJ °C-1. In the previous experiment, the molar mass of the substance was found to be 148.16 gmol-1. What is AcombU for the unknown compound? να ΑΣφ ? kJ mol1 Submit Request Answer
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2.000g of Compound X with molecular formula C4H6 are burned in a constant-pressure calorimeter containing 40.00kg of water at 25°C. The temperature of the water is observed to rise by 0.5325°C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25°C. Be sure your answer has a unit symbol, if necessary, and round it to 3 significant digits.
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If 9.5 grams of C3H8O was burned to change the temperature of 31.5 mL of water from 12 to 19.9 degrees Celsius, what is the experimental value of the enthalpy change of combustion of C3H8O?
Phenol undergoes combustion in oxygen to produce carbon dioxide gas and The standard heat of combustion of phenol, CgH,OH(s), is -3054 kJ/mol. AH?[CO,(g)] = -393.5 kJ/mol and AHÇ [H,O(1)] = -285.8 kJ/mol, what is t %3D enthalpy of formation of phenol? +164.4 kj/mol +328.8 kj/mol -164.4 kj/mol -328.8 kj/mol
Phenol undergoes combustion in oxygen to produce carbon dioxide gas and liquid water. The standard heat of combustion of phenol, CH,OH(s), is -3054 kJ/mol. Given that AHÇ [CO2(g)] = -393.5 kJ/mol and AHS [H,O(1)] = -285.8 kJ/mol, what is the standard %3D enthalpy of formation of phenol? +164.4 kj/mol +328.8 kj/mol -164.4 kj/mol -328.8 kj/mol
1. 0.5 mole of monoatomic ideal gas, initially at 45 °C and 1 bar, is heated and allowed to expand reversibly against a constant pressure of 1 bar until the final temperature is 128 °C. 1.1 Calculate the work (w) that the gas does during this expansion. 1.2 Calculate the internal energy change (AU) of this expansion process. 1.3 Calculate the enthalpy change (AH) of this expansion process.
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