# What is the amount of heat required to completely melt a 200gram sample of h2os at stp

## Introduction

The standard enthalpy of fusion for water is 333.55 kJ/mol. This means that it takes 333.55 kJ of heat to melt one mole of water or that one mole of water absorbs that much heat when it melts. To find the amount of heat required to melt a 200-gram sample of water, we need to convert it from moles to grams. Since one mole of water weighs 18 grams, we can divide 200 by 18 to find out how many moles are in our sample. This comes out to 11.11 moles. We can then multiply this by the standard enthalpy of fusion to find the amount of heat required. 11.11 moles * 333.55 kJ/mol = 3,704 kJ

## What is the heat required to completely melt a 200gram sample of h2os at stp?

In order to answer this question, we must first understand what melting is and the different states of matter. Melting is a process where a solid substance turns into a liquid when heated. The melting point is the temperature at which a substance changes from a solid to a liquid. The melting point of water is 0 degrees Celsius or 32 degrees Fahrenheit.

### The specific heat of water

At standard temperature and pressure (STP), water has a specific heat of 4.184 joules per gram (J/g). This means that it takes 4.184 joules of heat to raise the temperature of one gram of water by one degree Celsius. For a 200 gram sample of water, this would mean that it would take 836.8 joules of heat to raise the temperature by one degree Celsius.

### The molar heat of fusion of water

The molar heat of fusion of water is 333.55 J/mol. This means that, to completely melt a 200 gram sample of h2os at stp, you would need to supply 66.71 kJ of heat.

### The molar heat of vaporization of water

The molar heat of vaporization (∆Hvap) of water is the amount of heat required to completely vaporize one mole of liquid water at its boiling point (100°C) and standard pressure (1 atm). This value is often expressed in units of J/mol or kJ/mol. The ∆Hvap of water is about 40.7 kJ/mol, which means that it takes about 40.7 kJ of energy to convert 1 mol of liquid water into 1 mol of water vapor.

## Conclusion

In order to completely melt a 200 gram sample of water at standard temperature and pressure, 4.184 joules of heat energy would be required.