The density of liquid oxygen at its boiling point is 1.14 \rm{kg/L} , and its heat of vaporization is 213 \rm{kJ/kg} .
How much energy in joules would be absorbed by 4.0 L of liquid ox
q = mass oxygen x heat vap
Use density to convert volume oxygen to mass oxygen.
To find the energy absorbed by 4.0 L of liquid oxygen, we can use the formula:
Energy absorbed = mass of liquid oxygen x heat of vaporization
First, we need to find the mass of liquid oxygen. Since we know the density of liquid oxygen at its boiling point is 1.14 kg/L, we can calculate the mass using the formula:
Mass = density x volume
Mass = 1.14 kg/L x 4.0 L
Mass = 4.56 kg
Now, we can use the mass of liquid oxygen and the given heat of vaporization (213 kJ/kg) to calculate the energy absorbed.
Energy absorbed = 4.56 kg x 213 kJ/kg
Converting kJ to J:
1 kJ = 1000 J
Energy absorbed = 4.56 kg x 213 kJ/kg x 1000 J/1 kJ
Energy absorbed = 970,080 J
Therefore, 4.0 L of liquid oxygen would absorb approximately 970,080 J of energy.
To find out how much energy would be absorbed by 4.0 L of liquid oxygen, we can use the formula:
Energy = Mass × Heat of Vaporization
First, we need to determine the mass of the liquid oxygen. To do this, we'll use the density of the liquid oxygen at its boiling point.
Density = Mass / Volume
Rearranging the formula, we can solve for mass:
Mass = Density × Volume
Now we have all the necessary values to calculate the energy absorbed:
Mass = (Density of liquid oxygen at boiling point) × (Volume of liquid oxygen)
Mass = (1.14 kg/L) × (4.0 L)
Mass = 4.56 kg
Now, multiply the mass by the heat of vaporization to find the energy absorbed:
Energy = Mass × Heat of Vaporization
Energy = (4.56 kg) × (213 kJ/kg)
Energy = 973.28 kJ
Since 1 kJ is equal to 1000 J (joules), we can convert the energy to joules:
Energy = (973.28 kJ) × (1000 J/kJ)
Energy = 973280 J
Therefore, 4.0 L of liquid oxygen would absorb approximately 973,280 joules of energy.