Solid potassium nitrate dissolves in water according to the equation below. KNO3 (s) → K+ (aq) + NO3(aq) AH° = +34.89 kJ 15.00 grams of solid KNO3 dissolves in 125.0 grams of water initially at a temperature of 25.00 °C in a perfect calorimeter. Calculate the final temperature of the solution in the calorimeter. [You may assume that no heat escapes the calorimeter and that all solutions have the same specific heat capacity as pure water (4.184 J/g °C)] • Is this salt dissolving process Endothermic or Exothermic? Endothermic • Does the chemical reactions (salt dissolving) release or absorb energy? Absorb • AH for the reaction above is +34.89 kJ per mol of KNO3 that dissolves. This is the quantity that tells us how much energy is released or absorbed as the salt dissolves. It is usually measured in per mol. However, we are not dissolving 1 mol of salt in this experiment, we are dissolving 15.00 grams of KNO3. How many moles of KNO3 are being dissolved? moles of KNO3 How much energy is released or absorbed as the salt dissolves? This quantity is call "q" for the reaction (qreaction). It is a measure of the amount of heat released or absorbed by the chemical reaction based on the amount used in this particular experiment. greaction= • Energy does not escape the calorimeter. We must account for all of that energy. If energy is released by the reaction (the salt), it must go somewhere. Where does it go? It goes INTO the wate in the calorimeter. If the reaction absorbs energy, where does it get it? It gets it by pulling it out of the water. Notice how the direction (sign) of the energy transfer changes depending on which point of view we take, the salt or the water. When we measure the temperature in the calorimeter we are measuring the temperature of the WATER (solution). Therefore there is a difference in sign for the energy transfer. Greaction=-qsolution- What is the value of qsolution? qsolution= J?
Solid potassium nitrate dissolves in water according to the equation below. KNO3 (s) → K+ (aq) + NO3(aq) AH° = +34.89 kJ 15.00 grams of solid KNO3 dissolves in 125.0 grams of water initially at a temperature of 25.00 °C in a perfect calorimeter. Calculate the final temperature of the solution in the calorimeter. [You may assume that no heat escapes the calorimeter and that all solutions have the same specific heat capacity as pure water (4.184 J/g °C)] • Is this salt dissolving process Endothermic or Exothermic? Endothermic • Does the chemical reactions (salt dissolving) release or absorb energy? Absorb • AH for the reaction above is +34.89 kJ per mol of KNO3 that dissolves. This is the quantity that tells us how much energy is released or absorbed as the salt dissolves. It is usually measured in per mol. However, we are not dissolving 1 mol of salt in this experiment, we are dissolving 15.00 grams of KNO3. How many moles of KNO3 are being dissolved? moles of KNO3 How much energy is released or absorbed as the salt dissolves? This quantity is call "q" for the reaction (qreaction). It is a measure of the amount of heat released or absorbed by the chemical reaction based on the amount used in this particular experiment. greaction= • Energy does not escape the calorimeter. We must account for all of that energy. If energy is released by the reaction (the salt), it must go somewhere. Where does it go? It goes INTO the wate in the calorimeter. If the reaction absorbs energy, where does it get it? It gets it by pulling it out of the water. Notice how the direction (sign) of the energy transfer changes depending on which point of view we take, the salt or the water. When we measure the temperature in the calorimeter we are measuring the temperature of the WATER (solution). Therefore there is a difference in sign for the energy transfer. Greaction=-qsolution- What is the value of qsolution? qsolution= J?
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Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.109QP: A 21.3-mL sample of 0.977 M NaOH is mixed with 29.5 mL of 0.918 M HCl in a coffee-cup calorimeter...
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![THIS QUESTION MUST BE COMPLETED
Solid potassium nitrate dissolves in water according to the equation below.
KNO3 (s) → K+ (aq) + NO3- (aq) AH° = +34.89 kJ
15.00 grams of solid KNO3 dissolves in 125.0 grams of water initially at a temperature of 25.00 °C in a perfect calorimeter. Calculate the final temperature of the solution in the calorimeter.
[You may assume that no heat escapes the calorimeter and that all solutions have the same specific heat capacity as pure water (4.184 J/g.°C)]
• Is this salt dissolving process Endothermic or Exothermic? Endothermic
• Does the chemical reactions (salt dissolving) release or absorb energy? Absorb
• AH for the reaction above is +34.89 kJ per mol of KNO3 that dissolves. This is the quantity that tells us how much energy is released or absorbed as the salt dissolves. It is usually measured in
per mol. However, we are not dissolving 1 mol of salt in this experiment, we are dissolving 15.00 grams of KNO3. How many moles of KNO3 are being dissolved?
moles of KNO3
How much energy is released or absorbed as the salt dissolves? This quantity is call "q" for the reaction (qreaction). It is a measure of the amount of heat released or absorbed by the chemical
reaction based on the amount used in this particular experiment.
qreaction =
●
Energy does not escape the calorimeter. We must account for all of that energy. If energy is released by the reaction (the salt), it must go somewhere. Where does it go? It goes INTO the wate
in the calorimeter. If the reaction absorbs energy, where does it get it? It gets it by pulling it out of the water. Notice how the direction (sign) of the energy transfer changes depending on which
point of view we take, the salt or the water. When we measure the temperature in the calorimeter we are measuring the temperature of the WATER (solution). Therefore there is a difference in
sign for the energy transfer.
greaction = -0
= -9solution.
What is the value of qsolution?
qsolution
J?
=](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F416ff6d2-799f-43c9-9dc0-e44c7b16bb4d%2Fee29304e-d9e0-4253-a287-0822d88e760d%2Fj5zklwa_processed.png&w=3840&q=75)
Transcribed Image Text:THIS QUESTION MUST BE COMPLETED
Solid potassium nitrate dissolves in water according to the equation below.
KNO3 (s) → K+ (aq) + NO3- (aq) AH° = +34.89 kJ
15.00 grams of solid KNO3 dissolves in 125.0 grams of water initially at a temperature of 25.00 °C in a perfect calorimeter. Calculate the final temperature of the solution in the calorimeter.
[You may assume that no heat escapes the calorimeter and that all solutions have the same specific heat capacity as pure water (4.184 J/g.°C)]
• Is this salt dissolving process Endothermic or Exothermic? Endothermic
• Does the chemical reactions (salt dissolving) release or absorb energy? Absorb
• AH for the reaction above is +34.89 kJ per mol of KNO3 that dissolves. This is the quantity that tells us how much energy is released or absorbed as the salt dissolves. It is usually measured in
per mol. However, we are not dissolving 1 mol of salt in this experiment, we are dissolving 15.00 grams of KNO3. How many moles of KNO3 are being dissolved?
moles of KNO3
How much energy is released or absorbed as the salt dissolves? This quantity is call "q" for the reaction (qreaction). It is a measure of the amount of heat released or absorbed by the chemical
reaction based on the amount used in this particular experiment.
qreaction =
●
Energy does not escape the calorimeter. We must account for all of that energy. If energy is released by the reaction (the salt), it must go somewhere. Where does it go? It goes INTO the wate
in the calorimeter. If the reaction absorbs energy, where does it get it? It gets it by pulling it out of the water. Notice how the direction (sign) of the energy transfer changes depending on which
point of view we take, the salt or the water. When we measure the temperature in the calorimeter we are measuring the temperature of the WATER (solution). Therefore there is a difference in
sign for the energy transfer.
greaction = -0
= -9solution.
What is the value of qsolution?
qsolution
J?
=
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