Based on exposure time and place, the Sun's radiation may have harmful or beneficial effects.
<h3>What is solar radiation?</h3>
Solar radiation refers to the radiation from the Sun in the form heat, light and other forms of radiation.
The radiation from the Sun may have harmful or beneficial effects.
The effects of the Sun's radiation can be classified as BE, HE or SP as follows:
- BE- UV rays can help treat some health conditions. It creates Vitamin D
- SP- Use sunblock lotion with SPF 15 during hot days.
- BE- With the presence of sunlight, farmers can dry their crops.
- HE- UV rays can damage the tissue in your eyes.
- BE- Research says that sunlight helps moods.
- HE- Too much exposure from the sun can cause skin cancer.
- SP- Use sunglasses when you stay under the sun.
- SP- Wear a wide- brimmed hat on sunny days.
- BE- Humans can do recreational activities on a sunny day.
- SP- Wear sunglasses that filter UV light.
- HE- Prolonged exposure to the sun’s heat makes your skin age faster than normal.
- HE- Too much heat from the sun can cause heat stroke and loss of water.
- BE- Sunlight helps strengthen your immune system.
- BE- The vitamin D made thanks to the sun plays a big role in bone health.
- SP- Avoid sun in the middle of the day, from about 10 a.m. to 3 p.m.
Learn more about Sun's radiation at: brainly.com/question/921530
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Answer:
1.62 × 10²⁴ atoms are in 52.3 g of lithium hypochlorite.
Explanation:
To find the amount of atoms that are in 52.3 g of lithium hypochlorite, we must first find the amount of moles. We do this by dividing by the molar mass of lithium hypochlorite.
52.3 g ÷ 58.4 g/mol = 0.896 mol
Next we must find the amount of formula units, we do this be multiplying by Avagadro's number.
0.896 mol × 6.02 × 10²³ = 5.39 × 10²³ f.u.
Now to get the amount of atoms we can multiply the amount of formula units by the amout of atoms in one formula unit.
5.39 × 10²³ f.u. × 3 atom/f.u. = 1.62 × 10²⁴ atoms
1.62 × 10²⁴ atoms are in 52.3 g of lithium hypochlorite.
Start by converting mg to g. There is .001g in every miligram, so there is 0.4g in this sample.
Then find the molar mass of ibuprofen (C13H18O2) which is 206.3g/mol
Then divide grams by the molar mass to get moles of C13H18O2: (0.4g)/(206.3g/mol) = 1.94x10^-3mol C13H18O2
Then multiply moles by Avogadro's number to get molecules: (1.94x10^-3mol)/(6.02x10^23) = 1.17x10^21 molecules of ibuprofen (C13H18O2)
