To determine the heat of reaction, we need to use the principle of conservation of energy. According to this principle, the heat absorbed by the calorimeter [tex]\( (q_{\text{cal}}) \)[/tex] is equal in magnitude but opposite in sign to the heat of the reaction [tex]\( (q_{r \times n}) \)[/tex].
Given:
[tex]\[ q_{\text{cal}} = 49,936.64 \text{ J} \][/tex]
Using the principle of conservation of energy, the heat of reaction can be calculated as:
[tex]\[ q_{r \times n} = -q_{\text{cal}} \][/tex]
So, substituting the given value into the equation:
[tex]\[ q_{r \times n} = -49,936.64 \text{ J} \][/tex]
Thus, the heat of reaction is:
[tex]\[ q_{r \times n} = -49,936.64 \text{ J} \][/tex]
Therefore, the heat of reaction [tex]\( (q_{r \times n}) \)[/tex] is:
[tex]\[ -49,936.64 \text{ J} \][/tex]
As per the instructions, the correct answer is:
[tex]\[ -49,936.64 \][/tex]
