The heat released from the calculation is 33.56 kJ.
<h3>Heat of vaporization</h3>
The heat of vaporization is the heat absorbed when a substance changes from liquid to vapor. It is equal to the heat released when the vapor is condensed.
The total heat released = Heat of condensation + Heat lost to the skin
= (13.3 g × 2260 J/g) + (13.3 g × 4.18 J/g/°C × ( 100 - 37)°C)
= 30058 + 3502
= 33.56 kJ
The heat released from the calculation is 33.56 kJ.
Learn more about heat of vaporization: brainly.com/question/2427061
Answer:
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Well you are at a 86% so t<span>his is considered a "B" grade on an average grade scale. If you take 50 points we would need to know the Total point you could have got in that class to be able to see how much a percent was the assignment work and then take that percentage of the assignment and subtract it from the 86% to see where on the scale you would fall in after the assignment points were taken off. Hope this helps :)
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True, but it only burns about 8 extra calories.
<u>Given:</u>
Mass of H2O2 solution = 5.02 g
Mass of H2O2 = 0.153 g
<u>To determine: </u>
The % H2O2 in solution
<u>Explanation:</u>
Chemical reaction-
2H2O2(l) → 2H2O(l) + O2(g)
Mass % of a substance in a solution = (Mass of the substance/Mass of solution) * 100
In this case
% H2O2 = (Mass H2O2/Mass of solution)* 100 = (0.153/5.02)*100 = 3.05%
Ans: % H2O2 in the solution = 3.05%
