Calculate the temperature change when 100 g of water absorbs 500 J of heat, given the specific heat capacity…

Question

Calculate the temperature change when 100 g of water absorbs 500 J of heat, given the specific heat capacity of water is 4.18 J/g°C.

ScanSolve AI Tutor · Accepted Answer

To calculate the temperature change, we use the formula for heat transfer: $Q = mc\Delta T$ .

Identify the given values and the specific heat capacity of water.
- Heat supplied ( $Q$ ) = $500 \text{ J}$
- Mass of water ( $m$ ) = $100 \text{ g}$
- Specific heat capacity of water ( $c$ ) = $4.18 \text{ J/g}^\circ\text{C}$ (This is a standard value for liquid water.)
Rearrange the formula to solve for the temperature change ( $\Delta T$ ).
$Q = mc\Delta T$ $\Delta T = \frac{Q}{mc}$
Substitute the values into the formula and calculate $\Delta T$ .
$\Delta T = \frac{500 \text{ J}}{(100 \text{ g}) \times (4.18 \text{ J/g}^\circ\text{C})}$ $\Delta T = \frac{500 \text{ J}}{418 \text{ J/}^\circ\text{C}}$ $\Delta T \approx 1.196 \text{ }^\circ\text{C}$
Rounding to three significant figures:
$\Delta T \approx 1.20 \text{ }^\circ\text{C}$
The temperature change is:
$\text{1.20 }^\circ\text{C}$

Calculate the temperature change when 100 g of water absorbs 500 J of heat, given the specific heat capacity of water is 4.18 J/g°C.