How many litres of water at 100°C are vaporized by the addition of 5.00 MJ of heat

Answer 1

5 MJ = 5E6 J
q = mass H2O in grams x delta H vap in J/g.
5E6J = mass H2O x delta H vap.
Look up delta H vaporization/condensation, substitute and solve for mass H2O, then look up the density of H2O at 100 C and convert grams H2O to mL H2O, then convert to L.

Answer 2

Would I need to multiply this to get the mass?
(2.26*10^6)(5*10^6)

Answer 3

I don't know what you're asking?
5E6 J = grams H2O x 2260 J/g
grams H2O = 5E6J/2260 J/g = ? grams H2O

Then use density H2O at 100 C to convert to L H2O.

Answer 4

So the mass H20 would be
5E6/2260 X 2260 = 5E6 grams?

Answer 5

water density is 0.9584 L from 100°C

Answer 6

I mean 958.4 kg/m3 from 100°C

Answer 7

No. mass H2O = 5E6/2260 =?g just as I said above.
Then mass = volume x density. Substitute ?g for mass and the density and solve for volume.

Answer 8

5E6/2260=2.21g then converted 2.21g to 0.00221L

0.00221X958.4= 2.119064