How long would it take for 1.50 mol of water at 100.0 ∘c to be converted completely into steam if heat were added at a constant rate of 24.0 j/s ? express your answer to three significant figures and include the appropriate units?

The total heat that is needed by the water to get converted to steam is calculated below through the equation,

     H = (Hv)(n)

where H is the heat, Hv is the heat of vaporization (40.67 kJ/mol), and n is the number of mols. Substituting the known values,

   H = (40.66 kJ/mol)(1.5 mol) = 60.99 kJ

Calculating for the time,

    t = (60990 J) / (24 J/s)
    t = 2541.25 s

2541.25 s or approximately 42.35 minutes

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Multiply the 3 dimensions, assuming it is a rectangular cuboid, to get the volume in cm³ divide mass by volume to get density in g/cm³