Question

You are running a calorimetry experiment where you are trying to determine the number of Calories (with a capital C!) in a peanut. You set up your aluminum can of water and take all your initial data, putting it in the table below. Then, you set your peanut ON FIRE!!!!!!! You finish filling out your table once the peanut has gone out. How many Calories of heat did your peanut release? Round your answer to two digits after the decimal point.
Initial Mass of Peanut 3.11 grams
Final Mass of Peanut 0.52 grams
Mass of Water 55.2 grams
Initial Temp of Water 23.2 degrees C
Final Temp of Water 71.3 degrees C

Answer 1

Answer:

The number of calories of heat released by the peanut is $H =2655.12 \ Calories$

Explanation:

  Now from the data given we can evaluate the mass of the peanut that is burnt as

              $M_b = Initial \Mass \ of \ Peanut - Final\ Mass\ of\ Peanut$

Substituting values

              $M_b = 3.11 - 0.52$

                   $= 2.59 g$

Generally the heat gained by the water can be mathematically represented as

        $H = m_w c_w \Delta T$

Where $m_w$ is the mass of water which is given as $m_w = 55.2 g$

           $c_w$ is the specific heat of water which has a constant value of  $c_w = 1 cal / g ^oC$

    Now is $\Delta T$ is the change in temperature which can be evaluated as follows$\Delta T = Final\ Temp\ of\ Water - Initial\ Temp\ of\ Water = 71.3 - 23.2 = 48.1^oC$

 Now

         $H = 55.2 * 1 * 48.1$

         $H =2655.12 \ Calories$