Question
If a sample of 200 g of water must be boiled and the heat of vaporization of water is 2260 J/g, how much
heat is needed to cause this entire sample to boil into steam?
Answers below:
56800 J
411000 J
452000 J
395900 J
heat is needed to cause this entire sample to boil into steam?
Answers below:
56800 J
411000 J
452000 J
395900 J
Answers
GPT-4o mini
To find out how much heat is needed to boil the entire sample of water, you can use the formula:
\[
Q = m \cdot L
\]
where:
- \( Q \) is the heat required,
- \( m \) is the mass of the water, and
- \( L \) is the heat of vaporization.
In your case:
- \( m = 200 \, \text{g} \)
- \( L = 2260 \, \text{J/g} \)
Now, substituting the values into the formula:
\[
Q = 200 \, \text{g} \times 2260 \, \text{J/g}
\]
Calculating this gives:
\[
Q = 452000 \, \text{J}
\]
So, the amount of heat needed to boil the entire sample of water is \( 452000 \, \text{J} \).
The answer is \( 452000 \, \text{J} \).
\[
Q = m \cdot L
\]
where:
- \( Q \) is the heat required,
- \( m \) is the mass of the water, and
- \( L \) is the heat of vaporization.
In your case:
- \( m = 200 \, \text{g} \)
- \( L = 2260 \, \text{J/g} \)
Now, substituting the values into the formula:
\[
Q = 200 \, \text{g} \times 2260 \, \text{J/g}
\]
Calculating this gives:
\[
Q = 452000 \, \text{J}
\]
So, the amount of heat needed to boil the entire sample of water is \( 452000 \, \text{J} \).
The answer is \( 452000 \, \text{J} \).