Converting Water to Steam

Sounds like homework; what do you know about specific heat?

Sounds like homework. You need to dig into the books to find the solution and have your own "Ah ha" moment...

When I was in school, I wouldn't have even considered asking strangers for help on something this basic...whatever textbook you are using will have the formula in bold somewhere in the chapter. All I'll say is remember the phase change, as well as the temperature change.

first get the amount of energy you need to get 22 degree water to 300 degree senable heat. mc delt T

then convert that water to steam at 300 degree, latent heat

calculate, add the two

bish bash bosh

homework done

Alternatively, just use the Steam Tables and multiply by the weight of water.

Assuming the water is at sea level and ready to boil ( 100° C ), it should take 62.27 btu's to convert the .0639334 lbs. (or 10.23 oz.) of water to 100°C steam, then another 12.03 btu's to reach 300° C.

974 btu/#/°F for latent conversion then .48 btu/#/°F for steam.

Note: ice is .46 btu/#/°F

raising water temperature is 1 btu/#/°F

changing ice to water is 144 btu/#/°F

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Look in the steam tables the relative enthalpies of both.Multiply the difference by the quantity (the enthalpies are given per unit weight).

→ Steam tables.

Look it up there.

Nobody asked our guest for following basic: at which pressure would the vaporization process take place? Final result is different, if pressure is 1, or 5, or 20 bar, and so on.

I suggest that you find a general chemistry college text book and make the calculations for yourself.Only then will you have a good understanding of the answer.