No, the added heat melts the ice, but the result is water at the same temperature. Hence, option B is correct.
<h3>What is temperature?</h3>
The degree of hotness or coldness is measured on a definite scale.
Temperature doesn't change as heat is added during a phase change; for example, when the ice melts.
During the phase change, the added heat doesn't make the molecules move faster, but rather further apart.
Thus, No, the added heat melts the ice, but the result is water at the same temperature.
Learn more about the temperature here:
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Answer:
81 °C
Explanation:
This is a calorimetry question so a few things you will need for this. The calorimetry equation q=mcΔT & the specific heat of water (4.2J/g•°C). Other definitions are:
q = heat added/released by a sample
m = mass of sample
c=specific heat of sample
ΔT = change in temperature
from here we can rearrange the equation to state:
q/(mc) = ΔT
1200J/((20.0g)(4.2J/g•°C)) = ΔT
14°C = ΔT
If the starting temperature was 95.0°C and we know that the temperature was cooled by 14°C then the final temperature of the water would be 81.
The moles of NaCl would be 0.2669277996234607 cause one gram of NaCl is equal to 0.017110756386119273 moles
Atomic mass of Potassium = Mass of 1 atom of Potassium = 39.1 amu
Then
Mass of 6.02 x 1023 atoms of potassium = 39.1 x 6.02 x 1023 amu
=
We already know that
1 mole = 6.02 x 1023 atoms
Also
Number of mole = mass in grams/ atomic mass
Then
Mass in gram = Number of mole x atomic mass
= (39.1 x 6.02 x 1023)/(6.02 x 1023)
= 39.1 g
The correct option among all the options that are given in the question is the third option or option "B".