Calculate the energy needed to melt 50.0 L of nitrogen (N2).
Opps... spelled Chemistry wrong.
q = mass x heat fusion.
Hey I know this is late but anyone else who might need the answer:
Q = mLfus = (50.0 L * 1mol/22.4L*28g/1mol) (25.7 J/g) = 1606 J = 1.61 kJ
To calculate the energy needed to melt nitrogen (N2), we need to use the specific heat of fusion and the mass of nitrogen being melted.
Knowing that 50.0 L of nitrogen is being melted, we need to convert the volume to mass using the density of nitrogen.
Here are the steps to find the energy needed:
Step 1: Convert volume to mass
The first step is to convert the volume of nitrogen to mass using its density. The density of nitrogen gas at standard conditions is approximately 1.165 kg/m³.
1 liter (L) is equal to 0.001 cubic meters (m³).
50.0 L x 0.001 m³/L = 0.05 m³
Now we can find the mass using the density:
mass = density x volume
mass = 1.165 kg/m³ x 0.05 m³ = 0.05825 kg
So, the mass of nitrogen being melted is 0.05825 kg.
Step 2: Find the heat of fusion
The heat of fusion is the amount of energy required to change a substance from a solid to a liquid at its melting point. For nitrogen, the heat of fusion is approximately 2.79 kJ/mol.
Step 3: Convert mass to moles
To calculate the energy needed to melt the nitrogen, we need to convert the mass to moles. To do this, we need to find the molar mass of nitrogen (N2).
The molar mass of nitrogen (N2) is approximately 28.02 g/mol.
moles = mass/molar mass
moles = 0.05825 kg x (1000 g/kg) / 28.02 g/mol = 2.077 mol
Therefore, the number of moles of nitrogen is approximately 2.077 mol.
Step 4: Calculate the energy needed
The energy needed to melt nitrogen can be calculated using the following formula:
Energy = moles x heat of fusion
Energy = 2.077 mol x 2.79 kJ/mol = 5.78983 kJ
Therefore, the energy needed to melt 50.0 L of nitrogen is approximately 5.79 kJ.