Part A Find A:U for the combustion of ethanol (C,H:OH) to carbon dioxide and liquid water from the following data: The heat capacity of the bomb calorimeter is 34.65 kJ K-1 The combustion of 1.746 g of ethanol raises the temperature of the calorimeter from 204.150 K to 295.648 K. The molar mass of ethanol is 46.07 g mol". Enter your answer using four significant figures. A,U= kJ mol Submit Request Answer

Part A Find A:U for the combustion of ethanol (C,H:OH) to carbon dioxide and liquid water from the following data: The heat capacity of the bomb calorimeter is 34.65 kJ K-1 The combustion of 1.746 g of ethanol raises the temperature of the calorimeter from 204.150 K to 295.648 K. The molar mass of ethanol is 46.07 g mol". Enter your answer using four significant figures. A,U= kJ mol Submit Request Answer

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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Phereseadula has to determine the specific heat capacity of milk. He uses a constant volume calorimeter with a heat capacity of 758 J/K and the combustion of acetylene (C2H2) to do the experiment: 2C2H2(g) + 502(g) 4CO2(g) + 2H20(g) --- ArH = -2610kJ The calorimeter is filled with 1.190L of milk (instead of water). The density of milk is 1.034 g/ cm3. When 4.413 g of acetylene is burned in excess oxygen in the reaction vessel (bomb) of the calorimeter, the temperature of the milk and the bomb increased from 22.5°C to 61.9°C. The heat absorbed by the bomb is:
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Give your interpretation in Determination of Heat Capacity of Calorimeter using the collected data
When a 1.50g sample of solid sodium hydroxide dissolves in 60.0g of water in a coffe cup calorimeter, the temperature rises from 15.0°C to 32.8°C 1. Calculate the quntity of the heat in (kJ) released in the reaction. 2. Using the result in no1, Calculate the △H in (kJ mol -1 NaOH) for the solution process. Assume that the specific heat of the solution is the same as the pure water (4.184 J •g-1 °C-1)
*Ch.5 sect. 6 ~ * Adding 4.379 of the Salt NH₁ NO 3 (S) +0 130g of water in a coffee-cup Calorimetry (with stirring to dissolve resulted 17.1°C 10 in a decrease in temperature from 14,9 °C Calculate the enthalry Change for dissolving NH₂ NO₂ (s) in water in K5/mol. Assume the solution (whose mass 134. 4g) has a specific heat capacity of is 4.23/g.k (cold packs take advantages of the nitrate fact that dissolving is ammonium an endothermic Process) Enthalpy Change alt) A col pack uses the endothermic of a solution of ammonium nitrate. = - KJ/mol in water enthalpy 6 I v.k
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a) From the table of standard enthalpies of formation given below, calculate the standard enthalpy of the following reaction. Ca3P2(s) + 6HCl(g) ----> 3CaCl2(s) + 2PH3(g) Compound ΔHfo(KJ/mole) Ca3P2(s) -504 HCl(g) -92 CaCl2(s) -794 PH3(g) +9
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1. (STA student synthesized a fictional solid compound A2D6 when he mixed a 500. mL solution 0.500 M A3 and of 45.0 g of solid D4 (MW: 193.04). In this process 94.00 kJ of heat was used and the student noticed the flask getting colder. Write the thermochemical reaction for the synthesis of fictional solid compound A2D6. endo-colder (+)