Answer:
Enthalpy change = 74.36 kJ
Explanation:
Enthalpy change is defines as the heat absorbed or evolved during a chemical reaction at constant pressure and volume
Reaction:
H2O(l) --> H2O(g)
DHr = mCsDT
Where m is the mass of water
Cs is the specific heat capacity
DT is the temperature difference
= 31.6 * 4.18 * (25 - 3.2)
= 2879.518 J
DHvap = 44kJ/mol
Moles of water = mass/molecular weight
Molecular weight = (1*2) + 16
= 18g/mol
Moles of water = 31.6/18
= 1.756 moles
DHvap = 44 * 1.756
= 77.244kJ
DH = DHproduct - DHreactant
DHproduct = DHvap = 77.24kJ
DHreactant = DHr = 2879.518J = 2.880kJ
= 77.24 - 2.880
DH = 74.36kJ
Enthalpy change = 74.36 kJ
Answer:
The mass of heavier isotope is 345.6 amu.
Explanation:
Given data:
atomic wight of compound = 342.38 amu
lighter isotope mass = 340.91 amu
abundance of lighter isotope = 68.322%
mass of heavier isotope = ?
Solution:
average atomic mass = ( % age abundance of lighter isotope × its atomic mass) + (% age abundance of heavier isotope × its atomic mass) / 100
percentage of heavier isotope = 100- 68.322 = 31.678
Now we will put the values in formula.
342.38 = (68.322× 340.91) + (31.678 × X) / 100
342.38 = 23291.65302 + (31.678 × X) / 100
342.38 × 100 = 23291.65302 + (31.678 × X)
34238 -23291.65302 = (31.678 × X)
10946.35 / 31.678 = X
345.6 = X
The mass of heavier isotope is 345.6 amu.
I believe cc would result in a recessive pair.
D. The final substance in Beaker A is a mixture and in Beaker B is a pure substance.
