(a)
Interpretation : The melting point needs to be determined from the given heating curve of chloroform.
Concept Introduction : The phase transition curve represents the conversion of solid, liquid and gas with increasing the temperature. Here diagonal line shows one phase whereas the horizontal line represents the change in the phase of given substance. As temperature increases solid changes to liquid which further changes to gaseous state by increasing the temperature.
(b)
Interpretation : The boiling point needs to be determined from the given heating curve of chloroform.
Concept Introduction : The phase transition curve represents the conversion of solid, liquid and gas with increasing the temperature. Here diagonal line shows one phase whereas the horizontal line represents the change in the phase of given substance. As temperature increases solid changes to liquid which further changes to gaseous state by increasing the temperature.
(c)
Interpretation : The segments A, B, C, D and E needs to be identified in the given heating curve of chloroform.
Concept Introduction : The phase transition curve represents the conversion of solid, liquid and gas with increasing the temperature. Here diagonal line shows one phase whereas the horizontal line represents the change in the phase of given substance. As temperature increases solid changes to liquid which further changes to gaseous state by increasing the temperature.
(d)
Interpretation : The state of chloroform at the given temperature values needs to be determined.
Concept Introduction : The phase transition curve represents the conversion of solid, liquid and gas with increasing the temperature. Here diagonal line shows one phase whereas the horizontal line represents the change in the phase of given substance. As temperature increases solid changes to liquid which further changes to gaseous state by increasing the temperature.
Want to see the full answer?
Check out a sample textbook solutionChapter 10 Solutions
EBK BASIC CHEMISTRY
- 1. (9 points) A 15.0 gram piece of metal is heated to 65.0°C and then dropped into 175 grams of 24.0°C water. The system eventually comes to a stable temperature of 35.5 C. (The specific heat of water is 4.184 J/g °C) a. Energy is absorbed by the water. What is qWATER? b. Energy is released by the metal. What is qMETAL? (this one is easy) c. What is the specific heat (Cs) of the metal?arrow_forwarddoes it compare with the known melting and boiling point? (1) 9. The average kinetic energy of water molecules is a measure of the temperature of water. When the temperature of water remains constant the average kinetic energy of the molecules remains constant, even though the water is being heated by the Bunsen flame. So, energy is being taken in by the water, but it is not being used to increase the kinetic energy of the molecules. 9.1 What type of energy are the water molecules gaining during a phase change? (1) 9.2 Explain your reasoning (to question 9.1) with reference to the kinetic theory of matter. 10. Write the conclusion. (3) [30]arrow_forward53. The combustion of glucose, CH1,O, forms carbon dioxide gas and water vapour. When a 1.00 g sample of glucose was burned, it raised the temperature 100.0 mL of water by 37.0 °C. (5.2, 5.3, 5.5) AA (a) Write a balanced chemical equation for this reaction. (b) Use AH to calculate the enthalpy change of this of reaction. (c) Use bond energies in Table 1 on page 307 to calculate the enthalpy change of this reaction. The structural formula of glucose is shown in Figure 1.arrow_forward
- Match each of the following A quantity of 505 J of heat are added to 11.3 g of water at 28.3 °C. What is the final temperature of water? ( specific heat of water = 4.18 J/g.°C ). Choose... Choose... -48.25 188.7 A balloon of helium gas lost 36.4 kJ of heat while it was raising uP, simultaneously, the helium gas expanded from 64.0 L to 80.0 L against 563 mmHg pressure, Calculate the change in the internal energy (AU) of helium gas ( in kJ). Given that (atm.L = 101.3 J) -37.6 10.7 -238.7 39.0 268 11.85arrow_forwardWhat mass of liquid water at room temperature (25°C) can be raised to its boiling point with the addition of 24 kJ of energy? (77g)arrow_forwardA flask containing 1059 g of water is heated and a temperature increase from 32.4 °C to 67.6 °C. How much heat did one mole of water absorb in (J/mol). (s=4.18, molar mass of water 18 g/mol) a. 0.71 b. 4.30 C. 10.88 d. 2.50 е. 7.29 1.arrow_forward
- A cedarcrest.instructure.com Homework Set #2 Join conversation 16. Calculate the heat capacity of a brick if a 100. g sample absorbs 2439 J of heat, and its temperature changes from 28.0°C to 57.0°C. (3.6)arrow_forward10.105 Complete and balance each of the following: (10.7) a. ZnCO3(s) + H,SO,(aq) b. Al(s) + HBr(aq)arrow_forwardA coffee cup calorimeter contains 25.0 g water at 23.8 C. A 5.00 g sample of an unknown metal at an initial temperature of 78.3 C was dropped into the calorimeter. The final temperature of mixture was 46.3 C. Calculate the specific heat of the metal. The specific heat of water is (4.184)arrow_forward
- In a large building, oil is used in a steam boiler heating system.The combustion of 1.0 lb of oil provides 2.4 * 107 J. Howmany kilograms of oil are needed to heat 150 kg of water from22 °C to 100 °C? (3.4, 3.5)arrow_forward9.4 What is the energy change when the temperature of 11.9 grams of solid platinum is decreased from 39.4 °C to 23.8 °C ?Answer: _ Joules.arrow_forward00 2. 4. 9 #3 %23 V %24 Calculate q when 13.7 g of ice is cooled from -16.2°C to -82.9°C (Cire = 2.087 J/g-K)?arrow_forward
- Living By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHER