Thermochemistry to the Rescue

Calculate the amount of heat (q) produced by the combustion of 4.05 g CH₄ (H_comb = -890.4 kJ). See the calculation shown in the lab manual for help with this calculation.

Consider that the 4.05 g methane is burned and all of the heat from this combustion is absorbed by 1.0 kg of 20. ºC water (ignore the pot holding the water, and use 4.18 J g^-1 ºC^-1 for the specific heat of the water). What would be the final temperature of the water? Solve by following the steps below.

First, rearrange equation 3 to solve for delta T.  Show your rearrangement of equation 3 below. 

Now, plug into your equation the values for q, m, and sp ht to find deltaT (be mindful of your kJ and J units).

Finally, knowing delta T and the initial temperature, T_I, find the final temperature, T_F,  of the water.