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joja [24]
3 years ago
10

In some regions of the world, forests are cut down and then burned to create room for farmland. How might this local environment

al change affect people living on the East Coast of the United States?
A.
It could help farms to produce more crops by enriching their soil.
B.
It could contribute to rising temperatures and rising sea levels.
C.
It could raise oxygen levels in the ocean, allowing for larger populations of fish.
D.
It could reduce the amount of carbon dioxide that is released into the air.
Chemistry
2 answers:
Firdavs [7]3 years ago
8 0

Answer:It could contribute to rising temperatures and rising sea levels.

Explanation:

The forests are natural sinks for CO2. Forest trees absorb CO2 and release oxygen thereby making the air fresher. CO2 is a greenhouse gas. It is know to adversely contribute to the rising temperature of the earth. This rising temperature of the earth lead to the melting of polar ice caps and consequent rise in sea levels. For this cause, deforestation must be greatly discouraged and afforestation strongly encouraged.

UkoKoshka [18]3 years ago
6 0

The answer is D.

<u>Explanation</u>

Without trees, no carbon dioxide will be released into the air. It would not raise oxygen levels, and it wouldn’t effect rising sea levels.

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4 years ago
A bomb calorimeter has a heat capacity of 675 J/°C and contains 925 g of water. If the combustion of 0.500 mole of a hydrocarbon
ikadub [295]

<u>Answer:</u> The enthalpy of the reaction is 269.4 kJ/mol

<u>Explanation:</u>

To calculate the heat absorbed by the calorimeter, we use the equation:

q_1=c\Delta T

where,

q = heat absorbed

c = heat capacity of calorimeter = 675 J/°C

\Delta T = change in temperature = T_2-T_1=(53.88-24.26)^oC=29.62^oC

Putting values in above equation, we get:

q_1=675J/^oC\times 29.62^oC=19993.5J

To calculate the heat absorbed by water, we use the equation:

q_2=mc\Delta T

where,

q = heat absorbed

m = mass of water = 925 g

c = heat capacity of water = 4.186 J/g°C

\Delta T = change in temperature = T_2-T_1=(53.88-24.26)^oC=29.62^oC

Putting values in above equation, we get:

q_2=925g\times 4.186J/g^oC\times 29.62^oC=114690.12J

Total heat absorbed = q_1+q_2

Total heat absorbed = [19993.5+114690.12]J=134683.62J=134.7kJ

To calculate the enthalpy change of the reaction, we use the equation:

\Delta H_{rxn}=\frac{q}{n}

where,

q = amount of heat absorbed = 134.7 kJ

n = number of moles of hydrocarbon = 0.500 moles

\Delta H_{rxn} = enthalpy change of the reaction

Putting values in above equation, we get:

\Delta H_{rxn}=\frac{134.7kJ}{0.500mol}=269.4kJ/mol

Hence, the enthalpy of the reaction is 269.4 kJ/mol

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