Question

How does the temperature and specific heat capacity of a sample of water (the calorimeter) change...

  1. How does the temperature and specific heat capacity of a sample of water (the calorimeter) change as a different mass or temperature of hot metal is added to it?
  2. How does the temperature and specific heat capacity of a sample of water (the calorimeter) change as the volume of water is changed?
  3. How does the molar enthalpy of dissolution change with the amount of substance added to water?
  4. How does the molar enthalpy of dissolution change with the volume of water the substance is added to?
  5. How does the molar enthalpy of neutralization change with the amount and/or concentration of acid and base present?
Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Specific heat of a substance is the amount of heat required to increase the temperature of 1 g of the substance by 1°C. It is an intrinsic property. The total amount of heat energy absorbed or released by a substance and also the change in temperature may vary with the mass but the specific heat does not change.
Similarly change in volume changes the density of the substance but the specific heat is not affected.

Total enthalpy change during a process is an extensive property and changes with mass or volume of a substance.
However, molar enthalpy change for a process(here dissolution) is an intensive property and does not change with the quantity of the substance.

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
When 7.56 g of NaCl is added to a coffee cup calorimeter, the water temperature changes...
When 7.56 g of NaCl is added to a coffee cup calorimeter, the water temperature changes by 4.1 ºC. If the heat of solution (the enthalpy change upon dissolving in water) is 3.8 kJ/mol, what mass of solution must be in the cup? Assume the specific heat capacity of the solution is the same as the specific heat capacity of water.
A 6.40 g sample of iron (specific heat capacity = 0.451 J/g*C) is placed in a...
A 6.40 g sample of iron (specific heat capacity = 0.451 J/g*C) is placed in a boiling water bath until the temperature of the metal is 100.0*C. The metal is quickly transferred to 119.0g of water at 25.0*C in a calorimeter (specific heat capacity of water = 4.18 J/g*C). Determine the final temperature of the water in the calorimeter (3 significant figures).
A 6.40 g sample of iron (specific heat capacity =0.451 J/g*C) is placed in a boiling...
A 6.40 g sample of iron (specific heat capacity =0.451 J/g*C) is placed in a boiling water bath until the temperature of the metal is 100.0*C. The metal is quickly transferred to 119.0g of water at 25.0*C in a calorimeter (specific heat capacity of water = 4.18 J/g*C). Determine the final temperature of the water in the calorimeter (3 significant figures).
SETUP In today’s lab we will measure specific heat using a calorimeter. A calorimeter consist of...
SETUP In today’s lab we will measure specific heat using a calorimeter. A calorimeter consist of a small metal cup inside a larger metal container, with a lid.  The cups are thermally separated from each other by means of air and a wooden ring, thus reducing the thermal conduction to a minimum. To keep track of how much water etc. we have, the whole calorimeter will be placed on a digital scale. Make sure to zero the scale before you place...
A 0.505 g sample of KCl is added to 61.0 g of water in a calorimeter....
A 0.505 g sample of KCl is added to 61.0 g of water in a calorimeter. If the temperature decreases by 1.06°C, what is the approximate amount of heat (in J) involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g°C?
PART A) A sample of metal at a known hot temperature is placed in to a...
PART A) A sample of metal at a known hot temperature is placed in to a calorimeter containing water of known mass and known initial temperature. The temperature of the water rises and the final temperature of the water is recorded. What equation is used to calculate the amount of heat the calorimeter water absorbed? PART B) How do you deermine the amount of heat lost by the metal if you know the amount of heat gained by the calorimeter...
In a calorimetry experiment to determine the specific heat capacity of a metal block, the following...
In a calorimetry experiment to determine the specific heat capacity of a metal block, the following data was recorded: Quantity Mass of the metal block 0.50 kg Mass of empty calorimeter + Stirrer 0.06 kg Mass of calorimeter + stirrer + water 0.20 kg Mass of water 0.14 kg Initial Temperature of metal block 55.5 ⁰C Initial Temperature of water and calorimeter 22 ⁰C Final Temperature of block- water system 27.4 ⁰C Take the specific heat capacity of water to...
A calorimeter contains 30.0 mL of water at 11.5 ∘C . When 2.10 g of X...
A calorimeter contains 30.0 mL of water at 11.5 ∘C . When 2.10 g of X (a substance with a molar mass of 42.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 30.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...
A calorimeter contains 17.0 mL of water at 11.5 ∘C . When 1.60 g of X...
A calorimeter contains 17.0 mL of water at 11.5 ∘C . When 1.60 g of X (a substance with a molar mass of 79.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 30.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...
A calorimeter contains 35.0 mL of water at 15.0 ∘C . When 1.70 g of X...
A calorimeter contains 35.0 mL of water at 15.0 ∘C . When 1.70 g of X (a substance with a molar mass of 76.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 25.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT