1. What is the essence of detemining the heat capacity of the calorimeter? Is it possible to replace the calorimeter in the middle of the experiment, say you use same type of calorimeter, but you borrowed from another group to perform part C and D? Why? 2. Explain the temperature profiles of the contents of the calorimeter. 3. What is the relationship of the temperature with the calculated AH? Compare the AH of the three reactions.

1. What is the essence of detemining the heat capacity of the calorimeter? Is it possible to replace the calorimeter in the middle of the experiment, say you use same type of calorimeter, but you borrowed from another group to perform part C and D? Why? 2. Explain the temperature profiles of the contents of the calorimeter. 3. What is the relationship of the temperature with the calculated AH? Compare the AH of the three reactions.

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

Simple Calorimetry. A piece of solid aluminum at 15.0°C is immersed in 12.3 g of nitrogen gas which is initially at 51.1°C and the system is allowed to equilibrate. Given that the specific heat of solid aluminum is 0.908 J/K/g and the specific heat of nitrogen gas is 1.0 J/K/g, what is the mass of the piece of solid aluminum if the final temperature is 34.7°C?
For an exothermic reaction, how is the measured temperature change affected if some of the heat produced transfers to the calorimeter? How will the determination of the specific heat of the metal be affected if the thermometer used to record the temperature of the water bath reads too low?
1.What would be the significance of covering the calorimeter? 2.What would happen to the reaction if the some of Mg is not submerged in the solution?
A 30.0 g sample of chromium is heated to 100.0 °C in a boiling water bath. The sample is added to a calorimeter charged with 45.0 mL of water at 34.1 °C. The final temperature of the calorimeter contents is 38.5 °C. Calculate the specific heat of chromium.
To measure the enthalpy of an acid-base reaction, a student places the thermometer in the hydrochloric acid solution, and then, without rinsing with DI water, places it in the sodium hydroxide solution prior to adding the hydrochloric acid solution to the calorimeter. How would this affect the calculated enthalpy of the reaction, be too high, too low, or unaffected? Why?
Rsimi, Nour 2023VVA Chemistry.7b.FA1 An unknown solid substance is heated according to the temperature versus time graph below. Temperature (°C) 70 40 30 20 288 8 2 0 0 5 15 Time (min) 20 00 4 of 5 1 2 3 4 5 25 While the substance is a liquid, at what temperature do the molecules of the substance have the greatest average kinetic energy? 2 % 3 4 5 16 7 8 insert
Calculate the calorimeter constant for her calorimeter by following the steps below. 1. Calculate the mass of the warm water. 2. Calculate the change in temperature of the warm water. 3. Calculate the heat lost by the warm water. 4. Calculate the mass of the cold ocean water. 5. Calculate the change in temperature of the cold water. 6. Calculate the heat gained by the cold water. 7. Calculate the heat lost to the surroundings. 8. Calculate the calorimeter constant.
Please help with questions 5-12. Note: mass of HCl solution = 50.0g and mass of NaOH solution = 50.0g
A chemist measures the energy change AH during the following reaction: Cl₂(g) + H₂(g) → 2 HC1 (g) AH=184. kJ Use the information to answer the following questions. endothermic. This reaction is... 0 exothermic. Suppose 28.0 g of Cl₂ react. Yes, absorbed. Yes, released. Will any heat be released or absorbed? No. If you said heat will be released or absorbed in the second part of this question, calculate how much heat will be released or absorbed. Round your answer to 3 significant digits. ☐kJ x10 X ?
3. Suppose the 25.0 g of the following substances all initially at 27.0 °C absorb 2.35 kJ of energy. What is the final temperature of each? D) Water. You will need to look up specific heat values.
Show work to support your answer to this question. a) In a study of gaseous xenon, a chemist finds that 27.6 J of energy must be added to increase the temperature of 10.7 g of xenon from 22.7° C to 39.9° C. What is the experimental specific heat value for xenon gas? b) Using the specific heat you calculated for gaseous xenon, how much heat will be required to heat the 10.7 g sample of xenon from 39.9° C to 278.9° C?
The enthalpy change for a chemical reaction is the sum of the energy consumed in breaking bonds and the energy released during bond formation. One way to determine the overall energy change for a chemical reaction is to apply Hess’s law to add together a group of reactions which can be arranged such that the chemical equations, when combined, give the overall equation we are trying to characterize. a. Write a balanced chemical equation for the combustion of gaseous propane in gaseous oxygen to produce gaseous carbon dioxide and liquid water. C3H8(g)+ O2(g) ---->CO2(g)+ H2O(g) b. Combine the following equations to determine the enthalpy change for the combustion of 1 mole of propane. Assume that solid carbon is graphite. 3C(s,graphite)+4H2(g)--->C3H8(g) ΔHo = -103.8 kJ/mol C(s,graphite)+O2(g)--->CO2(g) ΔHo= -393.5 kJ/mol H2(g)+1/2 O2(g)--->H2O(g) ΔHo= -285.8 kJ/mol kJ/mol…