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Lena [83]
2 years ago
14

During the day, the temperature of the sand in a desert rises as the sand is heated by the sun. After the sun sets, the sand coo

ls. What happens to the heat energy in the sand as it cools?
Chemistry
2 answers:
Aleksandr [31]2 years ago
8 0
D) It is transferred to the air via the process of radiation.
abruzzese [7]2 years ago
8 0

Answer:

Deserts are the regions that cover little or no vegetation and there is no rainfall. Deserts are very hot in the day time and cold during the night time. It is because during the day time the sun heats up the sand, as a result of which the sand becomes very hot increasing the temperature. This increasing temperature in the desert is also because of the absence of rainfall and vegetation cover.

Thus, the desert area is rich in heat energy during the day time. But at night, the sand releases its heat energy back into the atmosphere through infrared radiation because the dry air cannot hold the heat anymore. This release of the heat energy allows the sands to cool, thereby dropping the temperature.

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Can soft drinks be part of a healthy diet?
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Answer:

yes, but its better to drink water

Explanation:

6 0
2 years ago
Consider the reaction; Mg + O2 → MgO Calculate the mass of magnesium oxide possible if 2.5 g Mg reacts with 5.0 g O2?
MAXImum [283]

Answer:

4.15g

Explanation:

Balance the reaction:

2Mg + O2 = 2MgO

Find limiting reactant from the two, by dividing miles with coefficient

2.5/24.3 = 0.103 moles/2 = 0.0515

5/16 = 0.31 moles/2 = 0.156

0.0515 is small than 0.156, so limiting reactant is Mg

Compare the ratio of Mg with MgO

Ratio is 2:2

So same moles = 0.103 moles

Mass = moles x molar mass of MgO

Mass = 0.103 x 40.3

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7 0
1 year ago
For the reaction ? Fe+? H2o ⇀↽? Fe3o4+? H2 , a maximum of how many grams of fe3o4 could be formed from 354 g of fe and 839 g of
Evgesh-ka [11]

The given reaction is:

3Fe + 4H2O → Fe3O4 + 4H2

Given:

Mass of Fe = 354 g

Mass of H2O = 839 g

Calculation:

Step 1 : Find the limiting reagent

Molar mass of Fe = 56 g/mol

Molar mass of H2O = 18 g/mol

# moles of Fe = mass of Fe/molar mass Fe  = 354/56 = 6.321 moles

# moles of H2O = mass of h2O/molar mass of H2O = 839/18 = 46.611 moles

Since moles of Fe is less than H2O;  Fe is the limiting reagent.

Step 2: Calculate moles of Fe3O4 formed

As per reaction stoichiometry:

3 moles of Fe form 1 mole of Fe3O4

Therefore, 6.321 moles of Fe = 6.321 * 1/ 3 = 2.107 moles of Fe3O4

Step 4: calculate the mass of Fe3O4 formed

Molar mass of Fe3O4 = 232 g/mol

# moles = 2.107 moles

Mass of Fe3O4 = moles * molar mass

= 2.107 moles * 232 g/mol = 488.8 g (489 g approx)

 


7 0
3 years ago
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stealth61 [152]

Answer:

The goal of Science is to expand knowledge.

Explanation:

3 0
3 years ago
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inysia [295]
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