Chemisty/Thermodynamics?

Use the following specific heats in J/g-C:


ice = 2.0


liquid = 4.18


steam = 2.0


Water has the following phase change enthalpies in kJ/mol


heat of fusion (solid to liquid) at 273 K = 6.01


heat of vaporization (liquid to gas) at 373 K = 40.7





a) How many joules of heat must be supplied to 5.7 g of ice at -22 degrees C to raise it to its melting point (without melting)?


Express answer to the nearest joule.


___J


b) How many joules of heat must be supplied to 5.7 g of liquid water at its melting point to raise it to its boiling point (without boiling)?


Express answer to the nearest joule.


____J


c) How many joules of heat must be supplied to 5.7 g of steam at its boiling point to raise it to 141 degrees C?


Express answer to the nearest joule.


___J


d) How many kilojoules of heat must be supplied to 5.7 g of ice at -22 degrees C to convert it to steam at 141?


Hint: The phase change enthalpy





Thanks for any help!!!

Chemisty/Thermodynamics?
a) q = mass (g) x spec. heat x deltaT


5.7 x 2.0 x 22 = 251J





b) q = mass x c T = 5.7 x 4.18 x 100 = 2383J





c) q = mass x Cp x T = 5.7 x 2.0 x 41 = 467J





d) a) + q(ice to liq) + b + q(liq to steam) + c)


251 + 5.7 x 6.01 + 2383 + 5.7 x 40.7 + 467


= 3367J
Reply:Q=m*L


Q=m*c*(T2-T1)





a) Q=5.7g*2.0J/gC*(0- -22C) = 250.8J





b) Q=5.7g*4.18J/gC*(100-0C) = 2382.6J





c) Q=5.7g*2.0J/gC*(141-100C) = 467.4J





d) Add a+b+c = 3100.8J = 3.1kJ