# When #1.0# #g# of potassium chloride, #KCl#, is dissolved in #25# #mL# (=#25# #g#) of water, it causes the temperature to drop from #24.33^o# #C# to #22.12^o# #C#. What is the molar enthalpy of dissolution for #KCl#?

The energy absorbed from the water by this endothermic reaction is approximately

The response under consideration is:

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The molar enthalpy of dissolution for KCl can be calculated using the formula:

ΔH = q / n

where: ΔH is the molar enthalpy of dissolution, q is the heat absorbed or released by the solution (in joules), n is the number of moles of solute.

First, calculate the heat absorbed or released (q) using the formula:

q = mcΔT

where: m is the mass of the solvent (in grams), c is the specific heat capacity of the solvent (for water, it is approximately 4.18 J/g°C), ΔT is the change in temperature (in °C).

Then, calculate the number of moles of KCl using its molar mass (74.55 g/mol) and the mass of KCl used (1.0 g).

Finally, plug the values into the formula for ΔH to find the molar enthalpy of dissolution.

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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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