water has a specific heat of 4.186 j/g°c. how much heat is required to increase 10.0 g of water from 25.0°c…

Explanation:

Step1: Identify the formula

The formula for heat $Q$ is $Q = mc\Delta T$, where $m$ is mass, $c$ is specific - heat capacity, and $\Delta T$ is the change in temperature.

Step2: Calculate the change in temperature

$\Delta T=T_2 - T_1=30.0^{\circ}C - 25.0^{\circ}C = 5.0^{\circ}C$

Step3: Substitute values into the formula

Given $m = 10.0\ g$, $c = 4.186\ J/g^{\circ}C$, and $\Delta T = 5.0^{\circ}C$. Then $Q=mc\Delta T=(10.0\ g)\times(4.186\ J/g^{\circ}C)\times(5.0^{\circ}C)$ $Q = 209.3\ J\approx209\ J$

Answer:

D. 209 J