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3.2 g of a salt was dissolved in 34.0 g of an acidic solution in a calorimeter with a calorimeter constant of 75.0 J K-1 with all substances initially at 91.0 °C. The resulting solution was observed to be at a temperature of 72.2 °C and have a heat capacity of 3.79 J g- K-'. Determine q for the dissolution process. а. 2650J b. -4060 J c. 4060 J d. -5.49 x 104 e. 5.49 x 104J

3.2 g of a salt was dissolved in 34.0 g of an acidic solution in a calorimeter with a calorimeter constant of 75.0 J K-1 with all substances initially at 91.0 °C. The resulting solution was observed to be at a temperature of 72.2 °C and have a heat capacity of 3.79 J g- K-'. Determine q for the dissolution process. а. 2650J b. -4060 J c. 4060 J d. -5.49 x 104 e. 5.49 x 104J

Chemistry
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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The calculations different, which is the correct one or are they all correct but different approach? all of the different equations encompass (constitute) the calorimeter constant but are still not right.

Some of the question have initial temperature higher and final lower while others have initial temperature lower but final higher.

I'm so confused, can you help?

3.2 g of a salt was dissolved in 34.0 g of an acidic solution in a calorimeter with a calorimeter constant of 75.0 J K-1 with all substances initially at 91.0 °C. The resulting solution was observed to be at a temperature of 72.2 °C and have a heat capacity of 3.79 J g-1 K-1. Determine q for the dissolution process. a. 2650 J Ob. -4060 J c. 4060 J d. -5.49 x 104 J e. 5.49 x 104 J Incorrect answer. You have left out a - sign in your equation. Given : Mass of salt=3.2 g 75.1 g of a basic solution was mixed with 32,5 a of water in a calorimeter with a calorimeter constant of 50.8 J K-1 with all substances initially at 59,4 °C. The resulting solution was observed to be at a temperature of 87.7 °C and have a heat capacity of 4.19 Jg K-1. Determine q for the mixing process. From the Relachon Mass of acidic solution =34.0 g Q= mC T Oa. 1.28 x 104 J Total mass of resultant solution, m = 3.2 + 34.0 = 37.2 g b. 1.67 x 105 J @= Total Heat Reguted The calorimeter constant, C cal=75.0 J K-1 c. -1.67 x 105 J m= Total mass= 75.1g+ 32.5g = 107669 d. -1.28 x 104 J The heat capacity of resultant solution, Csol=3.79 J g1 K-1 C= Heat capacity = 4.19 Jg"kl e. -1.42 x 104 Step 2 Temperature change , AT=(72.2+273)-(91.0+273 )=-18.8 K 41= Te-T, = (87.7- 59.4)°c change is alwayt same AT= 28.3°c= 28.3K Incorrect answer. Q = mc AT + C AT You have left out a - sign in your equation. Don't forget to include the heat required to change the temperature of the calorimeter. Q= 107.6g x 4. 19 Jg' k"x28-3 K Q = 37.2 g x3.79 J gʻ1 K-1 x(-18.8 K) + 75.0 J K-1 x (-18.8 K ) lo28 X104J Ans Heat of dissolution = Q = -4060.57 J Heat of dissolution = Q =-4060 J (Rounded) option (a) is comect
Transcribed Image Text:3.2 g of a salt was dissolved in 34.0 g of an acidic solution in a calorimeter with a calorimeter constant of 75.0 J K-1 with all substances initially at 91.0 °C. The resulting solution was observed to be at a temperature of 72.2 °C and have a heat capacity of 3.79 J g-1 K-1. Determine q for the dissolution process. a. 2650 J Ob. -4060 J c. 4060 J d. -5.49 x 104 J e. 5.49 x 104 J Incorrect answer. You have left out a - sign in your equation. Given : Mass of salt=3.2 g 75.1 g of a basic solution was mixed with 32,5 a of water in a calorimeter with a calorimeter constant of 50.8 J K-1 with all substances initially at 59,4 °C. The resulting solution was observed to be at a temperature of 87.7 °C and have a heat capacity of 4.19 Jg K-1. Determine q for the mixing process. From the Relachon Mass of acidic solution =34.0 g Q= mC T Oa. 1.28 x 104 J Total mass of resultant solution, m = 3.2 + 34.0 = 37.2 g b. 1.67 x 105 J @= Total Heat Reguted The calorimeter constant, C cal=75.0 J K-1 c. -1.67 x 105 J m= Total mass= 75.1g+ 32.5g = 107669 d. -1.28 x 104 J The heat capacity of resultant solution, Csol=3.79 J g1 K-1 C= Heat capacity = 4.19 Jg"kl e. -1.42 x 104 Step 2 Temperature change , AT=(72.2+273)-(91.0+273 )=-18.8 K 41= Te-T, = (87.7- 59.4)°c change is alwayt same AT= 28.3°c= 28.3K Incorrect answer. Q = mc AT + C AT You have left out a - sign in your equation. Don't forget to include the heat required to change the temperature of the calorimeter. Q= 107.6g x 4. 19 Jg' k"x28-3 K Q = 37.2 g x3.79 J gʻ1 K-1 x(-18.8 K) + 75.0 J K-1 x (-18.8 K ) lo28 X104J Ans Heat of dissolution = Q = -4060.57 J Heat of dissolution = Q =-4060 J (Rounded) option (a) is comect
41.9 g of a salt solution was mixed with 21.2 g of an acidic solution in a calorimeter with a calorimeter constant of 34.7 J K-1 with all substances initially at 43.7 °C. The resulting solution was observed to be at a temperature of 29.8 °C and have a heat capacity of 4.68 J g- K-1. Step 1 Determine q for the mixing process. Given data, a. 8.56 x 10*) Mass=63. 1g Ob. -3.45 x 104 AT=13, 9°C C(heat capacity)=4. 68J/g. K c. 4590 J Ccalo =34. 7J/K Od. 4100 J Ce. 3.45 x 104 J Step 2 The heat capacity of the calorimeter represents that it requires 34.7J energy to raise the temperature of the calorimeter by 1K. Incorrect answer. Don't forget to include the heat required to change the temperature of the calorimeter. So, the total heat change will be equal to the sum of total heat released by the mixing and heat absorbed by the calorimeter. NOTE: When the temperature of the system increases, it means that the reaction is releasing or producing heat, so the sign of the heat will be negative, and since the calorimeter absorbs heat, the sign will be positive. Change in temperature is always the same for kelvin and °C. Qreteased=-mC AT =-63. 1g x 4. 68J/g. K x 13.9K =-4104, 78J Qabsorbed=Ccallo x AT =34. 7JIK x 13.9K =482. 33J Total heat change=-4104. 78J + 482. 33J =-3622. 45J =-3. 62 x 10³J
Transcribed Image Text:41.9 g of a salt solution was mixed with 21.2 g of an acidic solution in a calorimeter with a calorimeter constant of 34.7 J K-1 with all substances initially at 43.7 °C. The resulting solution was observed to be at a temperature of 29.8 °C and have a heat capacity of 4.68 J g- K-1. Step 1 Determine q for the mixing process. Given data, a. 8.56 x 10*) Mass=63. 1g Ob. -3.45 x 104 AT=13, 9°C C(heat capacity)=4. 68J/g. K c. 4590 J Ccalo =34. 7J/K Od. 4100 J Ce. 3.45 x 104 J Step 2 The heat capacity of the calorimeter represents that it requires 34.7J energy to raise the temperature of the calorimeter by 1K. Incorrect answer. Don't forget to include the heat required to change the temperature of the calorimeter. So, the total heat change will be equal to the sum of total heat released by the mixing and heat absorbed by the calorimeter. NOTE: When the temperature of the system increases, it means that the reaction is releasing or producing heat, so the sign of the heat will be negative, and since the calorimeter absorbs heat, the sign will be positive. Change in temperature is always the same for kelvin and °C. Qreteased=-mC AT =-63. 1g x 4. 68J/g. K x 13.9K =-4104, 78J Qabsorbed=Ccallo x AT =34. 7JIK x 13.9K =482. 33J Total heat change=-4104. 78J + 482. 33J =-3622. 45J =-3. 62 x 10³J
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