Question 2 (True/False Worth 3 points)
1 answer:
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(1) The quantity of heat required to melt 175 g Cu is 35.88 kJ.
(2) The substance that releases 21.2 kJ of energy when 1.42 mol of it freezes is iron.
<h3>What is heat of fusion?</h3>Heat of fusion is the energy required to melt 1 mole of a substance.
<h3>What is heat of vaporization?</h3>The heat energy required to vaporize 1 mole of a substance has been heat of vaporization.
Heat of fusion of copper (Cu) is given as 13 kJ/mol
Number of moles of 175 g of copper = 175/63.5 = 2.76 moles
Q = nΔH
Q = 2.76 mol x 13 kJ/mol = 35.88 kJ
Thus, the quantity of heat required to melt 175 g Cu is 35.88 kJ.
<h3>Heat of fusion of the substance</h3>ΔH(fus) = Q/n
where;
- n is number of moles
- Q is quantity of heat released
ΔH(fus) = 21.2 kJ / 1.42 mol
ΔH(fus) = 14.93 kJ/mol
From the table the substance with latent heat of fusion of 14.9 kJ/mol is iron.
Thus, the substance that releases 21.2 kJ of energy when 1.42 mol of it freezes is iron.
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Answer:
The ratio of the temperature of helium to that of hydrogen gas is 2:1.
Explanation:
Atomic mass of hydrogen = M
Temperature of hydrogen gas =T
Pressure of the hydrogen gas = P
Mass of the hydrogen gas = m
Moles of the hydrogen gas =
Volume of the hydrogen gas = V
Using an ideal gas equation:
...(1)
Temperature of helium gas =T'
Pressure of the helium gas = P'= P
Mass of the helium gas = m' =m
Moles of the helium gas =
Volume of the helium gas = V' = V
Using an ideal gas equation:
...(2)
Divide (2) by (1)
The ratio of the temperature of helium to that of hydrogen gas is 2:1.