Student A measured the heat capacity of an insulated calorimeter and reported a value of -247.7 J/°C. Student B did the same experiment and reported a value of 156.7 J/°C. Which statement(s) represent(s) valid conclusions about this experiment? O Student B was correct to conclude that a value of 156.7 J/°C is reasonable. This value supports our hypothesis that a thermal insulator will need to absorb a relatively large amount of energy in order to increase its temperature by 1°C. O Student B was correct to conclude that Student A had an error in their experiment or their calculations because the heat capacity value being reported by Student A would imply that the calorimeter was absorbing energy resulting in a decrease in temperature. O Student A was correct to conclude that a value of -247.7 J/°C is reasonable. This is because it supports our hypothesis that a thermal insulator will need a relatively large change in energy to produce a 1°C change in temperature. O Student A was correct to conclude that the value of 156.7 J/°C reported by Student B is unreasonable. This is because calorimeters always release energy into the system, therefore the heat capacity should have a negative value.

Student A measured the heat capacity of an insulated calorimeter and reported a value of -247.7 J/°C. Student B did the same experiment and reported a value of 156.7 J/°C. Which statement(s) represent(s) valid conclusions about this experiment? O Student B was correct to conclude that a value of 156.7 J/°C is reasonable. This value supports our hypothesis that a thermal insulator will need to absorb a relatively large amount of energy in order to increase its temperature by 1°C. O Student B was correct to conclude that Student A had an error in their experiment or their calculations because the heat capacity value being reported by Student A would imply that the calorimeter was absorbing energy resulting in a decrease in temperature. O Student A was correct to conclude that a value of -247.7 J/°C is reasonable. This is because it supports our hypothesis that a thermal insulator will need a relatively large change in energy to produce a 1°C change in temperature. O Student A was correct to conclude that the value of 156.7 J/°C reported by Student B is unreasonable. This is because calorimeters always release energy into the system, therefore the heat capacity should have a negative value.

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

For letter b, mass percent of water is to be computed. Will you be able to resolve this part? These are the questions to be determined. b.) - mass of solute = ? g - mass of solvent = ? g - mass percent of water = ? %
Sodium hydroxide solution was standardized against one gram of potassium phthalate. First trial used 52.0 mL of the solution while the second trial used 52.4 of the solution to reach the end point. (a) What is the standardized concentration of the solution? (b) If the task is to prepare a one tenth of a molar solution, what is the percent accuracy of the preparation?
To prepare 50 mL solutions of 0.01 M KMnO4 in water (calculation to prepare chemicals in spectrophotometer)
What experimental technique should you use to determine the concentration of a colored solution? O measurements of volume & mass calorimetry O spectrometry O titration a
12.1 g of goztic acid was dissolved in water weighing 87.9 G. The mass fraction (%) of acid in the solution was calculated.
Can the solution be written out and solved step by step?
[References] What volume of 0.0381 M calcium hydroxide is required to neutralize 22.10 mL of 0.0255 M nitric acid? Volume mL %3D
[References] A solution is prepared by dissolving 16.2 g ammonium sulfate in enough water to make 260.0 mL of stock solution. A 35.00-mL sample of this stock solution is added to 60.00 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution. Assume that the volumes are additive. Concentration of ammonium ions = Concentration of sulfate ions = M Suhmit Answer Toy Another Version
[References] Use the References to access important values if needed for this question. In the laboratory you dissolve 15.7 g of cobalt(II) fluoride in a volumetric flask and add water to a total volume of 125. mL. What is the molarity of the solution? M
Twenty tablets (labelled 300 mg aspirin per tablet) had a total mass of 6.9117 g. The tablets were powdered and 0.5423 g of powder was added to 30.0 mL 0.494 M sodium hydroxide solution and the mixture boiled gently for 10 minutes. The excess alkali in the cooled solution was titrated with 0.475 M hydrochloric acid solution and 20.25 mL required for neutralization. Given that aspirin (C9H8O4) and NaOH react in a 1:2 ratio calculate the percentage of aspirin as compared to the labelled claim. Aspirin Mr(C9H8O4) = 180.2
Masses : Ca = 40.08 g S= 32.07 g O= 16.00 g A 35.0 mL sample of CaSO4 was evaporated to dryness, leaving 0.967 g of residue. What was the molarity of the original solution? step by step please
FAFSA® Applicatio. NG www.cfnc.org | 520.. NC Residency Deter. + Scholarships - Goo.. wh ccsf E Read [References] Use the References to access important values if needed for this question. In the laboratory, a student dilutes 26.6 mL of a 11.7 M nitric acid solution to a total volume of 200.0 mL. What is the concentration of the diluted solution? Concentration = M Submit Answer Try Another Version 1 item attempt remaining