how much thermal energy is needed to raise 500.0g of H2O at 50.0*C to steam at 100.0*C? step by step solution and answer!!???!!

answer? You have to be kidding. Are you taking a quiz and want to turn it in? Goodness.
Find the heat in each of the following.
heat the water from 50 to 100C
change the water to steam at 100C

add both those.

To calculate the amount of thermal energy required to raise 500.0g of H2O from 50.0°C to steam at 100.0°C, we need to consider two steps: heating the water from 50.0°C to 100.0°C, and then changing the water to steam at 100.0°C.

Step 1: Heating the water from 50.0°C to 100.0°C
To calculate the energy needed to heat the water, we can use the equation:

q = m * c * ΔT

Where:
q is the heat energy (in Joules),
m is the mass of the water (500.0g),
c is the specific heat capacity of water (4.184 J/g°C),
ΔT is the change in temperature (100.0°C - 50.0°C = 50.0°C).

Plugging in the values, we have:

q1 = 500.0g * 4.184 J/g°C * 50.0°C
q1 = 104,600 J

So, it requires 104,600 Joules of energy to heat the water from 50.0°C to 100.0°C.

Step 2: Changing the water to steam at 100.0°C
To calculate the energy needed to change the water to steam, we need to use the formula:

q = m * ΔHvap

Where:
q is the heat energy (in Joules),
m is the mass of the water (500.0g),
ΔHvap is the heat of vaporization of water (2260 J/g).

Plugging in the values, we have:

q2 = 500.0g * 2260 J/g
q2 = 1,130,000 J

So, it requires 1,130,000 Joules of energy to change the water to steam at 100.0°C.

Now, we can find the total thermal energy required by adding the results from steps 1 and 2:

Total thermal energy = q1 + q2
Total thermal energy = 104,600 J + 1,130,000 J
Total thermal energy = 1,234,600 J

Hence, the total thermal energy needed to raise 500.0g of H2O from 50.0°C to steam at 100.0°C is 1,234,600 Joules.