Question

Calculate the heat required to convert 1.90 g of ice at -5.75��C into liquid at 28.8��C. Given cwater = 4.187 J g�����K�����, cice = 2.093 J g�����K�����, and hfus = 334 J g�����.

Answer 1

To calculate the heat required to convert ice at a certain temperature to liquid at a different temperature, we need to consider two steps: heating the ice to its melting point, and then melting the ice.

Step-by-step explanation:

To calculate the heat required to convert ice at a certain temperature to liquid at a different temperature, we need to consider two steps: heating the ice to its melting point, and then melting the ice.

First, we calculate the heat required to heat the ice from -5.75°C to 0°C using the formula Q = m × c × ΔT, where Q is the heat, m is the mass of the ice, c is the specific heat capacity of ice, and ΔT is the change in temperature.

Next, we calculate the heat required to melt the ice at 0°C using the formula Q = m × hfus, where Q is the heat, m is the mass of the ice, and hfus is the heat of fusion.

Finally, we add the heat from the two steps to find the total heat required.

Let's calculate it:

Q1 = 1.90 g × 2.093 J/g·°C × (0 - (-5.75))°C

Q2 = 1.90 g × 334 J/g

Total heat required = Q1 + Q2