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Reika [66]
2 years ago
6

How minimising the use of cars can help save the ozone layer​

Chemistry
1 answer:
fgiga [73]2 years ago
6 0

Answer:

minimizing the use of cars can help save the ozone layer by ​Minimizing the amount of gasoline which damages the ozone layer.

therefore the ozone layer is preserved.

have a nice day.

You might be interested in
2.822 mol of nickel has _________ atoms of nickel.<br><br> (Enter just the number for this one.)
Irina-Kira [14]

Hello!

To find the number of atoms in 2.822 moles of nickel, we need to multiply it by Avogadro's number. Avogadro's number is 6.02 x 10^23 atoms.

2.822 moles x (6.02 x 10^23) ≈ 1.698844 x 10^24

Therefore, there are about 1.70 x 10^24 atoms (according to the number of significant figures) in 2.822 moles of nickel.

6 0
3 years ago
If you have a 4.6 L of gas in a piston at a pressure of 1.2 atm and compress 2p the gas until its volume is 2.6 L, what will the
Nesterboy [21]

Answer:

2.12atm

Explanation:

Boyle's Law: P1V1 = P2V2

Manipulate to solve for unknown: P2 = P1V1/V2

Substitute values:  P2=(1.2atm)(4.6L)/2.6L

P2 = 2.1230769atm

Round to 3 sig figs to get 2.12atm

3 0
3 years ago
What is the mass of Al₂O3 that will contain 10 kg of aluminium?​
Oksanka [162]

Answer:

1 mole of Al2O3 = 102 grams

1 mole of Al2 = 54 grams

102 grams of Al2O3 contains = 54 gram of Al2

10kg of Al2O3 contains = (54/102)*10000g Al2

= 5294.11 g Al2 or 5.29411 kg

5 0
2 years ago
Read 2 more answers
What does the principle of faunal succession state?
svetoff [14.1K]

Answer:

Explanation:

about 7000

3 0
3 years ago
Read 2 more answers
1) How many molecules are there in 985 mL of nitrogen at 0.0° C and 1.00 x 10-6 mm Hg?
RSB [31]

Answer : The number of molecules present in nitrogen gas are, 3.48\times 10^{13}

Explanation :

First we have to calculate the moles of nitrogen gas by using ideal gas equation.

PV=nRT

where,

P = Pressure of N_2 gas = 1.00\times 10^{-6}mmHg=1.32\times 10^{-9}atm      (1 atm = 760 mmHg)

V = Volume of N_2 gas = 985 mL = 0.982 L    (1 L = 1000 mL)

n = number of moles N_2 = ?

R = Gas constant = 0.0821L.atm/mol.K

T = Temperature of N_2 gas = 0.0^oC=273+0.0=273K

Now put all the given values in above equation, we get:

(1.32\times 10^{-9}atm)\times 0.982L=n\times (0.0821L.atm/mol.K)\times 273K

n=5.78\times 10^{-11}mol

Now we have to calculate the number of molecules present in nitrogen gas.

As we know that 1 mole of substance contains 6.022\times 10^{23} number of molecules.

As, 1 mole of N_2 gas contains 6.022\times 10^{23} number of molecules

So, 5.78\times 10^{-11} mole of N_2 gas contains (5.78\times 10^{-11})\times (6.022\times 10^{23})=3.48\times 10^{13} number of molecules

Therefore, the number of molecules present in nitrogen gas are, 3.48\times 10^{13}

8 0
3 years ago
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