Question

calculate the amount of heat required to raise the temperature of a 56 g sample of water from 34 °c to 67 °c. express your answer using two significant figures. q = j

Explanation:

Step1: Identify the formula

The formula for heat transfer is $Q = mc\Delta T$, where $Q$ is the heat, $m$ is the mass, $c$ is the specific - heat capacity, and $\Delta T$ is the change in temperature. The specific - heat capacity of water $c = 4.18\ J/(g\cdot^{\circ}C)$.

Step2: Calculate the change in temperature

$\Delta T=T_{2}-T_{1}=67^{\circ}C - 34^{\circ}C=33^{\circ}C$.

Step3: Calculate the heat

$Q = mc\Delta T$. Substitute $m = 56\ g$, $c = 4.18\ J/(g\cdot^{\circ}C)$, and $\Delta T = 33^{\circ}C$ into the formula.
$Q=56\ g\times4.18\ J/(g\cdot^{\circ}C)\times33^{\circ}C$.
$Q = 56\times4.18\times33\ J$.
$Q=7701.36\ J$.
Rounding to two significant figures, $Q = 7700\ J$.

Answer:

$7700\ J$