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3 years ago

How would increased chlorofluorocarbons (CFCs) in the atmosphere affect the growth of vegetation throughout the world?

2 answers:

7 0

Chlorofluorocarbons are a class of organic compounds that were used as propellants in the late 20th century. The problem with CFC's is that they attack the ozone layer, breaking it down. The weakened ozone layer is not able to stop UV light from reaching the earth, so the amount of UV light reaching the earth increases. This results in increased temperatures, and the death of vegetation.

Therefore, the answer is B.

ankoles [38]3 years ago

4 0

Ultraviolet light will increase on earth's surface. It will "raise" temperatures and decrease plant populations. Actually UV rays do not increase temperature, that's wrong.

They cause mutations in several organisms as they modify their DNA. They also cause skin cancer in humans and also cataracts and sunburns.

But they don't increase temperature. That's carbon dioxide accumulation.

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what the type of solid materials are typically hard, have high melting pionts and poor electrical conductivities

Virty [35]

Answer:

Ionic solids

Explanation: Ionic solids—Made up of positive and negative ions and held together by electrostatic attractions. They're characterized by very high melting points and brittleness and are poor conductors in the solid state. An example of an ionic solid is table salt, NaCl.

7 0

3 years ago

Read 2 more answers

If one gram of sulphur dioxide contains x molecules what will be the number of molecules in 1g of methane

evablogger [386]

The ratio of molecules in sulphur dioxide and methane will be the same as the ratio of their moles. So, first of all we should find out the number of moles of sulphur dioxide in 1 gram of sulphur dioxide in 1 gram of sulphur dioxide, and the number of moles of methane in 1 gram of methane. This can be done as follows :

(i) The molecular formula of sulphur dioxide is $SO_{2}$

So, $1$ mole of $SO_{2}$ = $Mass$ $of$ $2'O'$

$=32+2*16$

$= 64$ grams

Now, $64g$ of sulphur dioxide $= 1$ mole

So, $1g$ of sulphur dioxide = $\frac{1}{64}$ mole

Thus, we have $\frac{1}{64}$ mole of sulphur dioxide and it contains molecules in it. Now, since equal moles of all the substance contain equal number of molecules, therefore, $\frac{1}{64}$ mole of methane will also contain x molecules of methane.

(ii) Molecular formula of methan is $CH_{4}$

So, 1 mole of $CH_{4}$ = Mass of C + Mass of 4 H

$=12+4*12$

Now, 16g of methane = 1 mole

So, 1 g of mathane = $\frac{1}{16}$ mole

We know that:

$\frac{1}{64}$ mole of methane contains = x molecules

So, $\frac{1}{16}$ mole of contains will contain = $\frac{x*64}{16}$ molecules

= $4x$ molecules

7 0

2 years ago

Balance the equation

Damm [24]

Answer:

Explanation:

8 0

3 years ago

What is the charge of an electron?

Mandarinka [93]

The charge of a electron is negative charge equal to
-1.602 176 565(35) X 10-19 coulombs

8 0

3 years ago

(22 points) Gas conversion problems #4-7 pls I have no idea how to solve this and i’ve tried but i don’t get it :(

vova2212 [387]

Answer:

See attached

Explanation:

The empirical gas laws relate the effect of one gas-law variable upon another. The gas-law variables include Pressure (P), Volume(V), Temperature(T) and mass (n). When two of the four variables are related holding the other two constant, the relationships are called 'The Empirical Gas Laws'.

These include

Boyles Law* => P ∝ 1/V; Temp & mass remain constant => P₁·V₁ = P₂V₂

(NOTE => Boyles Law is the only 'inverse' empirical relationship)

Charles Law => V ∝ T; Press & mass remain constant => V₁/T₁ = V₂/T₂

Gay-Lussac Law => P ∝ T; Vol & mass remain constant => P₁/T₁ = P₂/T₂

Avogadro's Law => n ∝ V; Press & Temp remain constant => n₁/V₁ = n₂/V₂

Combined Law => All variables in play => P₁V₁/n₁T₁ = P₂V₂/n₂T₂

*Note => <u>Convert all Temperature values to Kelvin</u> when working with Empirical Gas Laws. If a different dimension is needed, convert after working with Kelvin values. => ( K = °C + 273 )

__________________

Standards of the Gas Laws at 0°C(273K) STP

(Std Intn'l System) Other common equivalent unit values

Pressure 1 Atm 760mmHg, 101.325Kpa, 760 Torr, 14.2 lbs/in²

Volume 1 Liter

mass 1 mole

Temperature 0°C(=273K) K = °C + 273

___________________

4. ?Atm = 758.7mmHg

758.8mmHg = 758.7mmHg x (1Atm/760mmHg) = 0.9983 Atm

5. ?Kpa = 760.00mmHg x (1 Atm/760.00mmHg) x 101.325Kpa/1Atm)

= 101.325Kpa

6. Boyles Law => Decrease Pressure => Increase Volume (of gas) in bag.

P₁ = 101.325Kpa => P₂ = 99.82Kpa

P₁V₁ = P₂V₂ => V₂ = P₁V₁/P₂ = V₁(101.325Kpa/99.82Kpa) = 1.015·V₁ => That is, the volume of gas in bag will expand to 1.015 x that at sea level. The bag may burst if not elastic.

7. ?Kpa = 2.56Atm

2.56Atm = 2.56Atm x 101.325Kpa/1Atm = 259.392Kpa

6 0

3 years ago