Taking into account the definition of calorimetry, 0.0185 moles of water are required.
Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.
Sensible heat is defined as the amount of heat that a body absorbs or releases without any changes in its physical state (phase change).
So, the equation that allows to calculate heat exchanges is:
Q = c× m× ΔT
where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation.
In this case, you know:
Replacing in the expression to calculate heat exchanges:
92.048 kJ = 4.186 [tex]\frac{J}{gC}[/tex]× m× (100 °C -34 °C)
92.048 kJ = 4.186 [tex]\frac{J}{gC}[/tex]× m× 66 °C
m= 92.048 kJ ÷ (4.186 [tex]\frac{J}{gC}[/tex]× 66 °C)
m= 0.333 grams
Being the molar mass of water 18 [tex]\frac{g}{mole}[/tex], that is, the amount of mass that a substance contains in one mole, the moles of water required can be calculated as:
[tex]amount of moles=0.333 gramsx\frac{1 mole}{18 grams}[/tex]
amount of moles= 0.0185 moles
Finally, 0.0185 moles of water are required.
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