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2. To calibrate your calorimeter, you first put 45 mL of cold water in the cup, and measure its temperature to be 21.7 °C. You then pour 59 mL of hot water, initial temperature = 50.1 °C, into the cup and measure the temperature every thirty seconds over a 10-minute period. You extrapolate this cooling curve to the time of addition and find that the final temperature after mixing is 36.2 °C. What is the heat change of the hot water, q??? (Assume the density of the water is 1.00 g/mL, and remember that the specific heat of water is 4.184 J/g·K or J/g·°C.) What is the heat change of the cold water, q??? What is the heat change of the calorimeter, q???? What is the heat capacity of the calorimeter, Ccal? 3. You would like to measure the heat of neutralization of an acid-base reaction. You mix 225 mL each of 0.65 M HNO? and 0.65 M LiOH, both at a temperature of 18.1 °C in a calorimeter equilibrated to that same temperature. After following the temperature change for 10 minutes and extrapolating it to the time of addition, you find that the final temperature after mixing was 22.3 °C. Previously you measured the heat capacity of the calorimeter (Ccal) as 47 J/°C. Assuming that the density of the two solutions is 1.00 g/mL, and that their specific heats are the same as water, 4.184 J/g·°C, what is the heat absorbed by the two solutions, q????? What is the heat absorbed by the calorimeter, q???? What is the heat change for the neutralization reaction, q???? What is the ?H for the neutralization? HESS'S LAW - ENTHALPY OF A SLOW REACTION: PRE-LAB

2. To calibrate your calorimeter, you first put 45 mL of cold water in the cup, and measure its temperature to be 21.7 °C. You then pour 59 mL of hot water, initial temperature = 50.1 °C, into the cup and measure the temperature every thirty seconds over a 10-minute period. You extrapolate this cooling curve to the time of addition and find that the final temperature after mixing is 36.2 °C.

What is the heat change of the hot water, q???
(Assume the density of the water is 1.00 g/mL, and remember that the specific heat of water is 4.184 J/g·K or J/g·°C.)

What is the heat change of the cold water, q???

What is the heat change of the calorimeter, q????

What is the heat capacity of the calorimeter, Ccal?

3. You would like to measure the heat of neutralization of an acid-base reaction. You mix 225 mL each of 0.65 M HNO? and 0.65 M LiOH, both at a temperature of 18.1 °C in a calorimeter equilibrated to that same temperature. After following the temperature change for 10 minutes and extrapolating it to the time of addition, you find that the final temperature after mixing was 22.3 °C. Previously you measured the heat capacity of the calorimeter (Ccal) as 47 J/°C.

Assuming that the density of the two solutions is 1.00 g/mL, and that their specific heats are the same as water, 4.184 J/g·°C, what is the heat absorbed by the two solutions, q?????

What is the heat absorbed by the calorimeter, q????

What is the heat change for the neutralization reaction, q????

What is the ?H for the neutralization?

HESS'S LAW - ENTHALPY OF A SLOW REACTION: PRE-LAB

2. To calibrate your calorimeter, you first put 45 mL of cold water in the cup, and measure its temperature to be 21.7 °C. You then pour 59 mL of hot water, initial temperature = 50.1 °C, into the cup and measure the temperature every thirty seconds over a 10-minute period. You extrapolate this cooling curve to the time of addition and find that the final temperature after mixing is 36.2 °C.

What is the heat change of the hot water, q???
(Assume the density of the water is 1.00 g/mL, and remember that the specific heat of water is 4.184 J/g·K or J/g·°C.)

What is the heat change of the cold water, q???

What is the heat change of the calorimeter, q????

What is the heat capacity of the calorimeter, Ccal?

3. You would like to measure the heat of neutralization of an acid-base reaction. You mix 225 mL each of 0.65 M HNO? and 0.65 M LiOH, both at a temperature of 18.1 °C in a calorimeter equilibrated to that same temperature. After following the temperature change for 10 minutes and extrapolating it to the time of addition, you find that the final temperature after mixing was 22.3 °C. Previously you measured the heat capacity of the calorimeter (Ccal) as 47 J/°C.

Assuming that the density of the two solutions is 1.00 g/mL, and that their specific heats are the same as water, 4.184 J/g·°C, what is the heat absorbed by the two solutions, q?????

What is the heat absorbed by the calorimeter, q????

What is the heat change for the neutralization reaction, q????

What is the ?H for the neutralization?

HESS'S LAW - ENTHALPY OF A SLOW REACTION: PRE-LAB

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