How much heat must 575 grams of water absorb to change from ice at 0 degrees C to all gas at 100 degrees C? will medal

Question

anonymous · Answer

$$Energy = mL_{melt} + mC\Delta T + mL_{vap}$$ Remember to check your units and make sure they match.

anonymous · Answer

how do I plug in what I know to the equation you provided?

anonymous · Answer

L_melt is the latent heat of melting, C is the specific heat of water as a liquid, and L_vap is the latent heat of vaporization, m is the mass, and Delta T is the change in temperature, in your case 100.

anonymous · Answer

Energy  = mass * latent heat of melting + mass * specific heat of water * change in temperature + mass * latent heat of vaporization

anonymous · Answer

energy = 575 * .334 + 575 * 4.179 * 100 + 575 * 2.260
energy = 241,784.05 joules 
does this look right?

anonymous · Answer

@thomaster @dan815 @Whitemonsterbunny17 @Ashleyisakitty @Compassionate

anonymous · Answer

I think your values for the latent heat of fusion and the latent heat of vaporization are off by a factor of 3. Your specific heat is in J/g while it seems your latent heat is in kJ/g. The latent heat of fusion is 334 J/g and the latent heat of vaporization is 2260 J/g. But the equation looks correct.

anonymous · Answer

575 * 334 + 575 * 4.179 * 100 + 575 * 2260
energy = 1.7318425 x 10^6
This answer seems kinda high