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.