How many joules are required to heat 2.0 L of water from 20^$\circ$C to its boiling point of 100^$\circ$C? The specific heat of water is 4.18 J/g.^$\circ$C and the density of water is 1 g/mL.

Question

Quizplus · Accepted Answer

To calculate the energy required to heat water from 20°C to 100°C, use the formula $q = mc\Delta T$, where $m$ is the mass of water, $c$ is the specific heat capacity of water, and $\Delta T$ is the change in temperature. Given 2.0 L of water (2000 mL), and using the density of water (1 g/mL), the mass $m$ is 2000 g. The specific heat $c$ is 4.18 J/g°C, and the temperature change $\Delta T$ is $100°C - 20°C = 80°C$. Plugging these values into the formula gives $q = 2000 \times 4.18 \times 80 = 668,800 J$, or $6.7 \times 10^5 J$.

How Many Joules Are Required to Heat 2 ∘\circ∘ C to Its Boiling Point of 100

How Many Joules Are Required to Heat 2 $\circ$ C to Its Boiling Point of 100