How much heat is required to raise the temperature of 53.5g of water from its melting point to its boiling point?

q = mass H2O x specific heat H2O x (Tfinal - Tinitial)

To determine the heat required to raise the temperature of water from its melting point to its boiling point, we need to consider two steps:

1. Heating the water from the melting point (0°C) to its boiling point (100°C)
2. Phase change from the liquid phase to the gas phase (boiling)

Let's calculate the heat required for each step:

Step 1: Heating the water from 0°C to 100°C
The specific heat capacity of water is approximately 4.184 J/g°C.

Heat (Q) = mass (m) × specific heat capacity (c) × temperature change (ΔT)

ΔT = final temperature - initial temperature = 100°C - 0°C = 100°C

Q1 = m × c × ΔT
= 53.5 g × 4.184 J/g°C × 100°C
= 223,898 J (rounded to the nearest whole number)

Step 2: Phase change (water to steam)
The heat of vaporization of water is approximately 2260 J/g.

Q2 = m × heat of vaporization
= 53.5 g × 2260 J/g
= 120,710 J (rounded to the nearest whole number)

Total heat required = Q1 + Q2
= 223,898 J + 120,710 J
= 344,608 J

Therefore, approximately 344,608 J of heat is required to raise the temperature of 53.5 g of water from its melting point to its boiling point.

To answer this question, we first need to know the specific heat capacity of water. The specific heat capacity is the amount of heat energy required to raise the temperature of a substance by a certain amount.

For water, the specific heat capacity is approximately 4.18 J/g°C (joules per gram per degree Celsius). This means that it takes 4.18 joules of heat energy to raise the temperature of 1 gram of water by 1 degree Celsius.

Next, we need to determine the temperature difference between the melting point and boiling point of water. Water's melting point is 0°C (32°F) and its boiling point is 100°C (212°F). So, the temperature difference is 100°C - 0°C = 100°C.

Now, we can calculate the amount of heat required to raise the temperature of 53.5 grams of water from its melting point to its boiling point using the formula:

Heat energy = mass × specific heat capacity × temperature difference

Substituting the values into the formula:

Heat energy = 53.5 g × 4.18 J/g°C × 100°C

Calculating this gives us:

Heat energy = 22381 J (joules)

Therefore, approximately 22381 joules of heat energy is required to raise the temperature of 53.5 grams of water from its melting point to its boiling point.