Questions: A 5.27 g sample of an unknown salt (MM=116.82 g / mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. What quantity in moles of the unknown salt were used in the reaction?

A 5.27 g sample of an unknown salt (MM=116.82 g / mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. What quantity in moles of the unknown salt were used in the reaction?
Transcript text: A 5.27 g sample of an unknown salt ( $\mathrm{MM}=116.82 \mathrm{~g} / \mathrm{mol})$ is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is $23.72^{\circ} \mathrm{C}$. After the salt has completely dissolved, the temperature of the solution is $28.54^{\circ} \mathrm{C}$. What quantity in moles of the unknown salt were used in the reaction?
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Solution

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Solution Steps

Step 1: Calculate the Moles of the Unknown Salt

To find the quantity in moles of the unknown salt, we use the formula:

\[ \text{moles} = \frac{\text{mass}}{\text{molar mass}} \]

Given:

  • Mass of the salt = 5.27 g
  • Molar mass of the salt = 116.82 g/mol

Substitute the given values into the formula:

\[ \text{moles} = \frac{5.27 \, \text{g}}{116.82 \, \text{g/mol}} = 0.0451 \, \text{mol} \]

Final Answer

The quantity in moles of the unknown salt used in the reaction is \(\boxed{0.0451 \, \text{mol}}\).

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