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nignag [31]
2 years ago
13

They are lightning rods, and their purpose is to? A)protect the building in the event of thunder. B)protect the building in the

event of a lightning strike. C)protect the building in the event of rain.
Chemistry
1 answer:
kompoz [17]2 years ago
8 0

Answer:

Option B

Explanation:

Whenever there is a lightning strike, the enormous amount of electrical energy generated is allowed to flow through a low resistant pathway i.e through the lightning rods to the ground so that the building and its resident remains intact and safe from the adverse impacts of lightning strike. These lightning rods are placed at a certain height above the top roof of the building  Hence, option B is correct

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What type of soil is found in the desert, the tundra, the tropical forest, and the temperate
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Answer: Sandy soil

Explanation:

5 0
3 years ago
If you had .0451 moles of CaCl2, how many grams would you have?
Montano1993 [528]

Answer:

option C

Explanation:

because i took the test

8 0
2 years ago
Which of the following changes depending on the strength of the gravity field it is in?
jek_recluse [69]
I believe it’s C.) Mass. Hope I’m right.
5 0
3 years ago
Suppose that 7.25 x 10^22 atoms of a hypothetical element have a mass of 3.88 g. What would be the molar mass (g/mol) of this el
S_A_V [24]

Answer:

32.23 to 4 significant figures.

Explanation:

The molar mass of the element is the mass of 6.022 * 10^23 atoms (Avogadro's number).

So by proportion it is 6.022 * 10^23 * 3.88 / 7.25 * 10^22

= 32.23 to 4 significant figures.

4 0
3 years ago
Ascorbic acid, or vitamin C (C6H8O6, molar mass = 176 g/mol), is a naturally occurring organic compound with antioxidant propert
nydimaria [60]

Answer : 50.69 mg of ascorbic acid does not meet the daily requirement.

Solution : Given,

Molar mass of Ascorbic acid = 176 g/mole

Moles of Ascorbic acid = 2.88\times 10^{-4}moles

Formula used :

Moles=\frac{Mass}{\text{ Molar mass}}

or, \text{ Mass of ascorbic acid}=\text{ Moles of ascorbic acid}\times \text{ Molar mass of ascorbic acid}

Now put all the given values in this formula, we get the mass of ascorbic acid.

\text{ Mass of ascorbic acid}=(2.88\times 10^{-4}moles)\times (176g/mole)=0.050688g=50.69mg

Conversion : (1g=1000mg)

As per question, a healthy adult’s daily requirement of vitamin C is 70-90 mg. But calculate mass of vitamin C is 50.69 mg. So, 50.69 mg of ascorbic acid does not meet the daily requirement.

5 0
3 years ago
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