First, a 5.500 g tablet of benzoic acid (C,H, CO, H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed insulation to rise from 15.00 °C to 42.56 °C over a time of 10.3 minutes. Next, 5.720 g of acetaldehyde (C, H,0) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 15.00 °C to 40.53 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 20,H,0(g) + 50, (g) → 4C0, (g) + 4 H,0 (3) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly match published values for this reaction. O exothermic Is this reaction exothermic, endothermic, or neither? O endothermic O neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. kJ kJ Calculate the reaction enthalpy AHn per mole of C, H,O. mol O

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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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A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at
right).
thermometer
stirrer
First, a 5.500 g tablet of benzoic acid (C,H,CO, H) is put into the "bomb" and burned completely in an excess of
water
oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed
insulation
to rise from 15.00 °C to 42.56 °C over a time of 10.3 minutes.
Next, 5.720 g of acetaldehyde (C2H,O}
are put into the "bomb" and similarly completely burned in an excess of
oxygen. This time the temperature of the water rises from 15.00 °C to 40.53 °C.
chemical reaction
"bomb"
Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below
about this reaction:
A "bomb" calorimeter.
2C,H,0(g) + 50, (g)
4CO, (g) + 4H,0 (g)
Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits.
Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly match
published values for this reaction.
exothermic
Is this reaction exothermic, endothermic, or neither?
endothermic
neither
If you said the reaction was exothermic or endothermic, calculate the amount of heat that was
released or absorbed by the reaction in the second experiment.
|kJ
kJ
Calculate the reaction enthalpy AH
rxn
per mole of C2H¸0.
mol
Transcribed Image Text:A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). thermometer stirrer First, a 5.500 g tablet of benzoic acid (C,H,CO, H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed insulation to rise from 15.00 °C to 42.56 °C over a time of 10.3 minutes. Next, 5.720 g of acetaldehyde (C2H,O} are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 15.00 °C to 40.53 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,0(g) + 50, (g) 4CO, (g) + 4H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly match published values for this reaction. exothermic Is this reaction exothermic, endothermic, or neither? endothermic neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. |kJ kJ Calculate the reaction enthalpy AH rxn per mole of C2H¸0. mol
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