How much heat must be added to 1.0kg of steam at 100 degrees Celsius to convert it to steam at 110 degrees Celsius?

How much heat must be added to 1.0 kg of water at 100 degrees Celsius to convert it to steam at 100 degrees Celsius?

What type of solution is formed when steam from boiling water evaporates

into the air?Explain

To determine the amount of heat needed to convert a substance from one temperature to another, we can use the formula:

Q = m * c * ΔT

Where:
Q is the heat needed,
m is the mass of the substance,
c is the specific heat capacity of the substance, and
ΔT is the change in temperature.

For steam at 100 degrees Celsius to steam at 110 degrees Celsius:
m = 1.0 kg
c = 2.03 kJ/kg°C (specific heat capacity of steam)
ΔT = 110°C - 100°C = 10°C

Using the formula, we can calculate the heat needed:

Q = 1.0 kg * 2.03 kJ/kg°C * 10°C
Q = 20.3 kJ

Therefore, 20.3 kJ of heat must be added to 1.0 kg of steam at 100 degrees Celsius to convert it to steam at 110 degrees Celsius.

For water at 100 degrees Celsius to steam at 100 degrees Celsius:
m = 1.0 kg
c = 4.18 kJ/kg°C (specific heat capacity of water)
ΔT = 100°C (no change in temperature)

Using the formula, we can calculate the heat needed:

Q = 1.0 kg * 4.18 kJ/kg°C * 100°C
Q = 418 kJ

Therefore, 418 kJ of heat must be added to 1.0 kg of water at 100 degrees Celsius to convert it to steam at 100 degrees Celsius.

To calculate the heat required to convert water at a certain temperature to steam at another temperature, we need to consider the concept of specific heat capacity and the heat of vaporization.

The specific heat capacity (C) is the amount of heat energy required to raise the temperature of a substance by 1 degree Celsius. For water, the specific heat capacity is approximately 4.186 J/g°C.

So, for the first question:
1. Determine the temperature change: 110°C - 100°C = 10°C.
2. Calculate the heat required to raise the temperature of 1.0 kg of steam by 10°C:
Heat = Mass × Specific Heat Capacity × Temperature Change
Heat = 1.0 kg × 4.186 J/g°C × 10°C
Heat = 41.86 kJ

Therefore, 41.86 kJ of heat must be added to 1.0 kg of steam at 100°C to convert it to steam at 110°C.

For the second question:
To convert 1.0 kg of water at 100°C to steam at 100°C, we need to consider the heat of vaporization. The heat of vaporization is the amount of heat energy required to convert 1 gram of a substance from a liquid to a gas without changing the temperature. For water, the heat of vaporization is approximately 2260 J/g.

1. Calculate the heat required to vaporize 1.0 kg of water:
Heat = Mass × Heat of Vaporization
Heat = 1.0 kg × 2260 J/g
Heat = 2260 kJ

Therefore, 2260 kJ of heat must be added to 1.0 kg of water at 100°C to convert it to steam at 100°C.

To convert steam at 100 to steam at 110, it is

q = mass steam x specific heat steam x (Tfinal-Tinitial) = ??

To convert WATER at 100 C to steam at 100 C it is
q = mass H2O x heat vaporization of H2O.