We’re being asked how many infrared photons with a wavelength of 1.5 × 10–6 m are needed to warm up 175 g of water from 25.0 ˚C to 40.0 ˚C.
For this problem, we need to do the following steps:
Step 1: Calculate the energy needed to warm up the water.
Step 2: Calculate the energy of an infrared photon.
Step 3: Calculate the number of photons needed.
Photons of infrared radiation are responsible for much of the warmth we feel when holding our hands before a fire. These photons will also warm other objects. How many infrared photons with a wavelength of 1.5 × 10−6 m must be absorbed by the water to warm a cup of water (175 g) from 25.0 °C to 40 °C?
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the The Energy of Light concept. You can view video lessons to learn The Energy of Light. Or if you need more The Energy of Light practice, you can also practice The Energy of Light practice problems.
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Our tutors rated the difficulty ofPhotons of infrared radiation are responsible for much of th...as medium difficulty.
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Our expert Chemistry tutor, Sabrina took 6 minutes and 44 seconds to solve this problem. You can follow their steps in the video explanation above.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor West's class at UGA.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.