A 275-g sample of nickel at 100.0°C is placed in 100.0 mL of water at 22.0°C. What is the final temperature of the water? Assume that no heat is lost to or gained from the surroundings. Specific heat capacity of nickel = 0.444 J/(g·K)

Question

Quizplus · Accepted Answer

The heat lost by nickel equals the heat gained by water. Using the formula $q = mc\Delta T$, where $q$ is heat, $m$ is mass, $c$ is specific heat capacity, and $\Delta T$ is the change in temperature, we can set the heat lost by nickel equal to the heat gained by water and solve for the final temperature. Given the specific heat capacity of water is $4.18 \, \text{J/(g·K)}$, and assuming the density of water is $1 \, \text{g/mL}$, the mass of water is $100.0 \, \text{g}$. Solving the equation with these values leads to a final temperature of approximately $39.6°C$.

A 275-G Sample of Nickel at 100