\( q = 199.86 \cdot ( 4.184 \frac { J } { g C } ) \cdot \Delta 9.3 \)

It looks like you're trying to calculate the heat transfer \( q \) using the formula: \[ q = m \cdot c \cdot \Delta T \] where: - \( m \) is the mass (in grams), - \( c \) is the specific heat capacity (in \( \frac{J}{g \cdot C} \)), - \( \Delta T \) is the change in temperature (in degrees Celsius). In your equation, you have: - \( m = 199.86 \, g \) - \( c = 4.184 \, \frac{J}{g \cdot C} \) - \( \Delta T = 9.3 \, C \) Now, substituting these values into the equation: \[ q = 199.86 \cdot (4.184) \cdot (9.3) \] Now, let's calculate it step by step: 1. Calculate \( 4.184 \cdot 9.3 \): \[ 4.184 \cdot 9.3 = 38.8952 \] 2. Now multiply by the mass \( 199.86 \): \[ q = 199.86 \cdot 38.8952 \approx 7775.56 \, J \] So, the heat transfer \( q \) is approximately \( 7775.56 \, J \).