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qaws [65]
3 years ago
10

0.158 g of a mystery molecule is placed into a bomb calorimeter that has a heat capacity of 1650 J/C. After the sample is combus

ted the temperature of the calorimeter increased by 2.54 C. Determine the molar mass of the mystery molecule if the enthalpy of combustion for one mole is 2960 kJ/mol
Chemistry
1 answer:
Lunna [17]3 years ago
8 0

<u>Answer:</u> The molar mass of the mystery element is 111.27 g/mol

<u>Explanation:</u>

To calculate the heat absorbed by the calorimeter, we use the equation:

q=c\Delta T

where,

q = heat absorbed

c = heat capacity of calorimeter = 1650 J/°C

\Delta T = change in temperature = 2.54^oC

Putting values in above equation, we get:

q=1650J/^oC\times 2.54^oC=4191kJ

Heat absorbed by the calorimeter will be equal to the heat released by the reaction.

<u>Sign convention of heat:</u>

When heat is absorbed, the sign of heat is taken to be positive and when heat is released, the sign of heat is taken to be negative.

To calculate the number of moles of the mystery molecule, we use the equation:

\Delta H_{rxn}=\frac{q}{n}

where,

q = amount of heat released = -4191 J

n = number of moles = ? moles

\Delta H_{rxn} = enthalpy change of the reaction = -2960 kJ/mol = -2960000 J/mol    (Conversion factor = 1 kJ = 1000 J)

Putting values in above equation, we get:

-2960000=\frac{-4191J}{n}\\\\n=\frac{-4191}{-2960000}=0.00142mol

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Given mass of mystery molecule = 0.158 g

Moles of mystery molecule = 0.00142 mol

Putting values in above equation, we get:

0.00142mol=\frac{0.158g}{\text{Molar mass of mystery molecule}}\\\\\text{Molar mass of mystery molecule}=\frac{0.158}{0.00142}=111.27g/mol

Hence, the molar mass of the mystery element is 111.27 g/mol

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Explanation:

The given data is as follows.

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      Molarity = \frac{\text{weight of solute}}{\text{molecular weight of solute}} \times \frac{1000}{\text{volume of solution in ml}}

                    = \frac{75.8 g}{92.13 g/mol} \times \frac{1000}{200 ml}

                    = 4.11 M

Hence, molarity of toulene is 4.11 M.

  • As molality is the number of moles of solute present in kg of solvent.

So, we will calculate the molality of toulene as follows.

   Molality = \frac{\text{given weight of solute}}{\text{given molecular weight of solute}} \times \frac{1000}{\text{weight of solvent in grams}}

             = \frac{75.8 g}{92.13 g/mol} \times \frac{1000}{95.6 g}

             = 8.6 m

Hence, molality of given toulene solution is 8.6 m.

  • Now, calculate the number of moles of toulene as follows.

       No. of moles = \frac{mass}{\text{molar mass}}

                             = \frac{75.8 g}{92.13 g/mol}

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Now, no. of moles of benzene will be as follows.

     No. of moles = \frac{mass}{\text{molar mass}}

                             = \frac{95.6 g}{78.11 g/mol}

                             = 1.2239 mol

Hence, the mole fraction of toulene is as follows.

         Mole fraction = \frac{\text{moles of toulene}}{\text{total moles}}

                             = \frac{0.8227 mol}{(0.8227 + 1.2239) mol}

                             = 0.402

Hence, mole fraction of toulene is 0.402.

  • As density of given solution is 0.857 g/cm^{3} so, we will calculate the mass of solution as follows.

         Density = \frac{mass}{volume}

     0.857 g/cm^{3} = \frac{mass}{200 ml}      (As 1 cm^{3} = 1 g)

                      mass = 171.4 g

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      Mass % = \frac{\text{mass of solute}}{\text{mass of solution}} \times 100

                   = \frac{75.8 g}{171.4 g} \times 100

                   = 44.22%

Therefore, mass percent of toulene is 44.22%.

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