Calculate the total amount of energy required in calories to convert 50.0 g of ice at 0.00 degrees Celsius to steam at 100. degrees Celsius. Specific heat capacity of water is 1.00 cal/g OC

Hfusion = 80 cal/g OC and Hvap = 540 cal/g OC

Write the complete equation you will use.

Substitute the values in the equation in step 1.

Report the math answer with 3 sig figs and the correct unit.

The amount of heat absorbed is

Explanation:

Few processes involved are:

(1):

(2):

(3):

Calculating the heat absorbed for the process having same temperature:

......(i)

where,

q is the amount of heat absorbed, m is the mass of sample and is the enthalpy of fusion or vaporization

Calculating the heat released for the process having different temperature:

......(ii)

where,

= specific heat of solid or liquid

are final and initial temperatures respectively

We are given:

Putting values in equation (i), we get:

We are given:

Putting values in equation (i), we get:

We are given:

Putting values in equation (i), we get:

Calculating the total amount of heat released:

Hence, the amount of heat absorbed is

at the bottom

explanation:

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.