Question

multiple choice 1 point
a beaker containing 85 g of water is heated from 22.5°c to 31.2°c. how much heat energy (q, in joules, j) was transferred into the water? assume no heat loss to the surroundings.
the specific heat capacity of water is 4.184 j/g.°c
q = cp·m·δt
δt = q / cp·m
m = mass of the substance in grams
q = 4124 joules
q = 3094 joules
q = 5482 joules
q = 2865 joules
dont test me yet, i am trying to gain an understanding before attempting to answer this question.

Explanation:

Step1: Calculate the temperature change

$\Delta T=T_{final}-T_{initial}=31.2 - 22.5=8.7^{\circ}C$

Step2: Use the heat - transfer formula

The formula for heat transfer is $q = C_{p}\cdot m\cdot\Delta T$. Given that $C_{p}=4.184\ J/g^{\circ}C$, $m = 85\ g$, and $\Delta T=8.7^{\circ}C$.
Substitute the values into the formula: $q=4.184\times85\times8.7$.
First, calculate $4.184\times85 = 355.64$.
Then, calculate $355.64\times8.7=3094.068\approx3094\ J$.

Answer:

$q = 3094\ Joules$