Answer:
375.3KJ
Explanation:
The following data were obtained from the question:
Mass of water = 166g
Heat of Vaporisation (ΔHv) = 40.7kJ/mol
Heat (Q) =..?
Next, we shall determine the number of mole in 166g of water. This is illustrated below:
Mass of H2O = 166g
Molar mass of H2O = (2x1) + 16 = 18g/mol
Number of mole = Mass/Molar Mass
Number of mole of H2O = 166/18
Number of mole of H2O = 9.22 moles.
Now, we can obtain the heat required to vaporise the water as shown below:
Q = n·ΔHv
Q = 9.22 mol x 40.7kJ/mol
Q = 375.3KJ
Therefore, the heat required to vaporise the water is 375.3KJ.
A solution is supersaturated when more concentration is dissolved into a solution that is already saturated.
Answer:
66.5% (3 s.f.)
Explanation:
Please see the attached pictures for the full solution.
*Mr stands for relative formula mass
Answer:
IM VERY SORRY HAVE A GOOD DAY\\
Explanation:
porque o gás carbônico afasta o oxigênio da parte que está em chamas, e não existe fogo sem oxigênio
