2. A solution is formed by combining 10 mL of solution A and 40 mL of solution B. Find out the heat of reaction by assuming that no heat is lost to the calorimeter, if the initial and final temperature of the system is 20.4 and 28.5 °C, respectively. Specific heat of a solution is 4.184 J/g°C and density is 1.6 g/ml.
2. A solution is formed by combining 10 mL of solution A and 40 mL of solution B. Find out the heat of reaction by assuming that no heat is lost to the calorimeter, if the initial and final temperature of the system is 20.4 and 28.5 °C, respectively. Specific heat of a solution is 4.184 J/g°C and density is 1.6 g/ml.
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...
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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
Transcribed Image Text:Data and Calculations:
Run 1
Run 2
Volume of HCl(ag) solution (ml)
Mass of HClaq) solution' (g)
Volume of Na0H(aq) solution (ml)
Mass of NaOH(aq) solution" (g)
msolns: The total mass of acid and base solutions (g)
Ti: Initial temperature of the Na0H(aq) solution (°C)
T: Highest temperature reached after mixing acid with base (°C)
AT: Temperature change (°C) of the reaction mixture = (T; – T¿)
Cavg: Average Heat capacity of the calorimeter from exp.#1 (J/°C)
9released by rxn (J) (show your calculation below)
Number of moles of HCle
Number of moles of NaOH(aq)
25 ml
So ml
27
(aq) used
used
Number of moles of water formed
AHn: Heat of neutralization (KJ/mol) (show your calculation below)
Average Heat of neutralization (KJ/mol) from the two trials
Assume the density of solutions = 1 g/ml
Calculation:
1. Show your calculations for qrelegsed by Trn in Joules and heat of neutralization (AH,) in
KJ/mol for trial 1
2. Calculate the % error in your average heat of neutralization AH9 compared to the accepted
or true value. Note: the "true" or accepted value is mentioned in the introduction section.
Transcribed Image Text:Questions:
1. A coffee cup calorimeter having a heat capacity of 451 J/°C was used to measure the heat
evolved when 100 ml of 1 M NaOHao) was added to 20 ml of 5 M HClag) initially at 23.000
°C. The temperature of the water rose to 28.855 °C. Calculate AH, (in kJ/mol) for this reaction.
Assume the specific heat of the final solution is 4.184 J/g°C and the density of each solution is
1.00 g/ml.
2. A solution is formed by combining 10 mL of solution A and 40 mL of solution B. Find out the
heat of reaction by assuming that no heat is lost to the calorimeter, if the initial and final
temperature of the system is 20.4 and 28.5 °C, respectively. Specific heat of a solution is 4.184
J/g°C and density is 1.6 g/ml.
10
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