If you had dissolved 4g of ammonium nitrate in the calorimeter instead of 16g wo

Question

If you had dissolved 4g of ammonium nitrate in the calorimeter instead of 16g would you expect the total heat that was transferred by the process to be different









If you had dissolved 4g of ammonium nitrate in the calorimeter instead of 16g would you expect to measure a different molar heat. Of solution. If you had dissolved 4g of ammonium nitrate in the calorimeter instead of 16g would you expect the total heat that was transferred by the process to be different









If you had dissolved 4g of ammonium nitrate in the calorimeter instead of 16g would you expect to measure a different molar heat. Of solution.









If you had dissolved 4g of ammonium nitrate in the calorimeter instead of 16g would you expect to measure a different molar heat. Of solution.

Explanation / Answer

A) The amount of heat energy (Q) transferred depends on three factors:
1. The capacity of the substance to absorb heat – called the specific heat capacity (c).
2. The amount (moles) of the substances reacting
3. The change in temperature

T moles and Q moles. So if the number of moles increases the temperature increases and the amount of heat energy transferred will be greater.

Similarly since we are reducing the amount of ammonium nitrate we expect the total heat energy transferred to be lesser.

B) Molar heat of solution, or, molar enthalpy of solution, is the energy released or absorbed per mole of solute being dissolved in solvent.

So the molar heat of solution measured will be same when you change the weight of the solute as the number of moles are to be considered and will get incorporated in the formula accordingly as

Molar heat (enthalpy) of solution has the units J mol-1 or kJ mol-1

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