Aluminum metal has a specific heat of 0.900 J/g·^$\circ$C. Calculate the amount of heat required to raise the temperature of 10.5 moles of Al from 30.5 ^$\circ$C to 225^$\circ$C.

Question

Quizplus · Accepted Answer

To calculate the amount of heat required, use the formula $q = m \cdot c \cdot \Delta T$, where $q$ is the heat energy, $m$ is the mass in grams, $c$ is the specific heat capacity, and $\Delta T$ is the change in temperature. First, convert moles of Al to grams using its molar mass (approximately 26.98 g/mol for Al), then calculate the change in temperature and finally apply the formula.

Aluminum Metal Has a Specific Heat of 0 ∘\circ∘ C Calculate the Amount of Heat Required to Raise the C

Aluminum Metal Has a Specific Heat of 0 $\circ$ C Calculate the Amount of Heat Required to Raise the C