How much energy is needed to change the temperature of 25.00 mL of water from 10.0$\degree$C to 95.0$\degree$C? [c_p= 4.18 J/(g . $\degree$C), d =1.00 g/mL]

Question

Quizplus · Accepted Answer

The energy needed can be calculated using the formula $q = mc\Delta T$, where $m$ is the mass of the water, $c$ is the specific heat capacity of water, and $\Delta T$ is the change in temperature. Given that the density of water is $1.00 g/mL$, the mass of $25.00 mL$ of water is $25.00 g$. The specific heat capacity of water is $4.18 J/(g\cdot°C)$. The temperature change is from $10°C$ to $95°C$, so $\Delta T = 95°C - 10°C = 85°C$. Thus, $q = 25.00 g \times 4.18 J/(g\cdot°C) \times 85°C = 8,892.5 J = 8.89 kJ$.

How Much Energy Is Needed to Change the Temperature of 25.00