Consider a 27.5 g piece of ice at 0.00 C.

a) how much heat is required to convert the ice to water that is also 0.00 C?

b) how much heat would be required to warm this water from 0.00 C to 17.50 C?

HELP!!

I think the fusion is 333 J/g at 0 C... But I'm not sure what to do with that.

Heat to melt=Hf*mass

Heat to raisetemp=specificheat*changeTemp*mass

Memorize those.

is Hf triangleH'f?? and if so would the value be -285.83?

for b, would we want the specific heat of h2o (l) or (s)?

To determine the amount of heat required in each scenario, you need to use the specific heat and heat of fusion values for ice and water. Let's break down the calculations step by step.

a) To convert the ice to water at 0.00 °C, you need to calculate the heat required for phase change or the heat of fusion. The equation you can use here is:

Heat (q) = mass (m) × heat of fusion (ΔHf)

Given:
mass = 27.5 g
heat of fusion (ΔHf) = 333 J/g

Plugging in these values, the calculation is:
q = 27.5 g × 333 J/g

Make sure units are consistent. In this case, the grams cancel out, leaving you with Joules (J) as the unit of heat energy.

b) To warm the water from 0.00 °C to 17.50 °C, you need to calculate the heat required for a temperature change. The equation you can use here is:

Heat (q) = mass (m) × specific heat (c) × change in temperature (ΔT)

Given:
mass = 27.5 g
specific heat (c) = a known value to warm water from 0 °C is typically 4.18 J/g°C
change in temperature (ΔT) = 17.50 °C - 0.00 °C

Plugging in these values:
q = 27.5 g × 4.18 J/g°C × 17.50 °C

Again, ensure units are consistent, and the grams cancel out, resulting in Joules (J) as the unit of heat energy.

Remember to carry out the calculations using the correct units and numbers to get accurate results.