Chemistry College

The balanced combustion reaction for C 6 H 6 C6H6 is 2 C 6 H 6 ( l ) + 15 O 2 ( g ) ⟶ 12 CO 2 ( g ) + 6 H 2 O ( l ) + 6542 kJ 2C6H6(l)+15O2(g)⟶12CO2(g)+6H2O(l)+6542 kJ If 7.300 g C 6 H 6 7.300 g C6H6 is burned and the heat produced from the burning is added to 5691 g 5691 g of water at 21 ∘ 21 ∘ C, what is the final temperature of the water?

Answers

Answer 1

Answer: The final temperature of the water is [tex]33.85^{o}C[/tex].

Explanation:

We know that molar mass of [tex]C_{6}H_{6}[/tex] is 78 g/mol. And, the amount of heat produced when 2 mol of [tex]C_{2}H_{6}[/tex] burns is 6542 KJ.

This means that,

   [tex]78 \times 2[/tex] = 156 g of [tex]C_{2}H_{6}[/tex] burns, heat produced is 6542 kJ.

Therefore, heat produced (Q) by burning  7.3 g of [tex]C_{6}H_{6}[/tex] is as follows.

               [tex]\frac{6542 \times 7.3 g}{156 g}[/tex]

              = 306.13 kJ

or,           = 306130 J      (as 1 KJ = 1000 J)

For water, mass is given as 5691 g and specific heat capacity of water is 4.186 [tex]J/g^{o}C[/tex].

So, we will calculate the value of final temperature as follows.

            Q = [tex]m \times C \times (T_{f} - T_{i})[/tex]

  306130 J = [tex]5691 g \times 4.186 J/g^{o}C \times (T_{f} - 21)^{o}C[/tex]

       [tex](T_{f} - 21)^{o}C = \frac{306130 J}{23822.53 J/^{o}C}[/tex]

          [tex]T_{f}[/tex] = 12.85 + 21

                      = [tex]33.85^{o}C[/tex]

Thus, we can conclude that the final temperature of the water is [tex]33.85^{o}C[/tex].

Answer 2

Final answer:

To determine the final temperature of water when 7.300 g of benzene is burned, use the enthalpy of combustion for benzene and apply stoichiometry to find the heat transferred to the water, then use the specific heat capacity formula to find the change in water's temperature.

Explanation:

The question asks about finding the final temperature of water after burning 7.300 g of benzene (C6H6) and adding the heat produced to the water at an initial temperature of 21 °C. To answer this, we need to use thermochemical principles and calculate the energy involved in the combustion of benzene which will then be absorbed by the water, causing a change in its temperature.

The heat absorbed by the water (q_water) can be calculated using the formula q = m * c *
igtriangleup T, where m is the mass of the water, c is the specific heat capacity of water (4.184 J/g°C), and
igtriangleup T is the change in temperature. Since we're given the enthalpy of combustion of benzene (6,542 kJ per 2 moles of C6H6), we can calculate the heat produced by burning 7.300 g of benzene using stoichiometry and the molar mass of C6H6 (78.11 g/mol).

Using this information allows us to solve for the final temperature of the water. Remember to convert the energy units appropriately when performing these calculations.

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