how many grams of ice would be melted by the energy obtained as 18g of steam is condensed at 100 deg C and?

Question

cooled to 0deg C

Answer 1

It depends also on how cold the ice is at the start.

assuming 0 deg ice to 0 deg water

18g * 2260j*g^-1 = 40680j condense steam to 100 deg water
18g * 4.18j*g^-1 * 100K = 7524j cool from 100 deg liquid to 0 deg liquid
40680j + 7524j = 48204j sum of exothermic

40680j / 334j*g^-1 = 144g

actually you only have 2 sig figs so:
14 * 10^1 grams ice melted

Answer 2

Condensing generates 40.7 kJ/mol 50g of H2O is 50/18 = 2.seventy 8 mol; So this generates 2.seventy 8*40.7 = 113.a million kJ, If the steam continues to be at 100ºC, then it is the warmth will soften m = 113.a million/6.07 = 10.6 mol of ice = 335 g of ice. If the condensed steam is delivered all the way down to 0ºC, then this demands fifty*a hundred*4.184 = 20.ninety two kJ which will soften one extra 20.ninety two/6.07 = 3.40 5 mol of ice, or sixty two.0 g. the full mass of ice melted is then 335 + sixty two = 397 g

Answer 3

Assuming the ice is at the melting point of 0 oC.

The 18 g of steam is equivalent to one mole of steam. Multiply this by the molar heat of vaporization for water. This is the amount of energy released.

Now apply this to the ice. Divide the heat available by the heat of fusion of ice and you get the moles of ice that can be melted. Multiply by 18 and you have the grams.

Answer 4

Use the heat of fusion and heat of vaporization.

Energy obtained: q = 1mol * Cv J/mol

Now use that as "q" in the second equation:
q = "x" mol * Cf J/mol

Solve for x. (This process can be used whatever units you are working in.)