A 21.3-mL sample of benzene at 26.0°C was cooled to its melting point, 5.5 °C, and then frozen at 5.5 °C. Calculate the quantity of energy transferred to the surroundings in this process. The density of benzene is 0.876 g/mL. The specific heat capacity of the liquid is 1.74 J g' K!. Its fusion enthalpy is 127 J/g.

A 21.3-mL sample of benzene at 26.0°C was cooled to its melting point, 5.5 °C, and then frozen at 5.5 °C. Calculate the quantity of energy transferred to the surroundings in this process. The density of benzene is 0.876 g/mL. The specific heat capacity of the liquid is 1.74 J g' K!. Its fusion enthalpy is 127 J/g.

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

Given the following theoretical chemical equation of the gaseous substances D, E, and F, how fast is D decreasing when F is increasing at a rate of 2 mol/L-s? * 2 D-E + F - 2 mol/L-s - 5 mol/L-s O - 4 mol/L-s - 3 mol/L-s
A 30.0 g sample of water at 280 K is mixed with 50.0 g water at 330 K. Calculate the final temperature of the mixture assuming no heat loss to the surrounding. Specific heat of water is 1 cal/g.°C
Diethyl ether, used as a solvent for extraction of organic compounds from aqueous solutions, has a high vapor pressure which makes it a potential fire hazard in laboratories in which it is used. How much energy is released when 315.0 g is cooled from 153.0°C to 0.0°C? boiling point: 34.5°C Heat of vaporization: 351 J/g Specific heat capacity, (CH3)2O(l): 3.74 J/(g·K) Specific heat capacity, (CH3)2O(g): 2.35 J/(g·K) 145 kJ 158 kJ 116 kJ 63.1 kJ 21.1 kJ
thermometer. A sample of aluminum, which has a specific heat capacity of 0.897 J·g *.°C*, is put into a calorimeter (see sketch at right) that insulated container contains 100.0 g of water. The aluminum sample starts off at 91.4 °C and the temperature of the water starts off at 19.0 °C. When the temperature of the water stops changing it's 26.9 °C. The pressure remains constant at 1 atm. water Calculate the mass of the aluminum sample. Be sure your answer is rounded to 2 significant digits. sample a calorimeter x10
6. Suppose 1.0 x 102 grams of ice absorbs 1255 J of heat, reaching a final temperature of -2.0°C. What was the initial temperature change of the ice? The specific heat capacity of H20(s) = 2.1 J/(g.°C).
Carbon tetrachloride (CCl4) boils at 77∘C. The measured enthalpy of vaporization is 29.8 kJ/mol What is the heat of vaporization?
The molar heat of solution of a substance is found to be +21.38 kJ/mol. The addition of 0.100 mol of this substance to 1.000L of water initially at 40.0 degrees celsius results in a temperature decrease. Assume the specific heat of the resulting solution to be equal to that of pure water. Find the final temperature of the solution (Also assume that the heat capacity of the calorimeter is negligible).
If 31.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The ∆H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g°C), and that no heat is gained or lost by the container, what will be the final temperature of the solution?
A block of iron weighing 4.50 kg at a temperature of 107.0 °C was inserted into a container containing 1.2 liter of water at a temperature of 30.0 °C isolated from the environment. What is the final temperature (in °C) of the water and the iron at the end of the process? (The specific heat of solid iron is 0.450 J lg .r and the specific heat of water is 4.184 J/ g°C) Density of water = 1.0 g/mL.
A sample of steam with a mass of 0.529 g at a temperature of 100 °C condenses into an insulated container holding 4.25 g of water at 5.0 °c. (For water, AHvap = 40.7 kJ/mol and Cwater = 4.18 J/(g · °C).) - Part A Assuming that no heat is lost to the surroundings, what is the final temperature of the mixture? Express your answer using three significant figures.
How much heat energy is required to convert 77.6 g of solid iron at 21 °C to liquid iron at 1538 °C? The molar heat of fusion of iron is 13.8 kJ/mol. Iron has a normal melting point of 1538 °C. The specific heat capacity of solid iron is 0.449 J/(g · °C). q= kJ
Calculate the amount of heat (in kJ) required to raise the temperature of a 86.0 g sample of ethanol from 198.0 K to 300.0 K. The specific heat capacity of ethanol is 2.42 J/g°C. 60.0 kJ 21.2 kJ 11.9 kJ 75.6 kJ 28.4 kJ