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AnnZ [28]
3 years ago
10

To break the oxygen-oxygen bonds in a single O2 molecule, 1 × 10–18 J of energy is required. Which of the following wavelengths

of light could be used to carry out this process?
Chemistry
1 answer:
Sonbull [250]3 years ago
8 0

E = hc/(lamda)

The lamda symbol is wavelength, which this site does not have. I can represent it with an "x" instead.

Plancks constant, h = 6.626×10^-32 J·s

Speed of light, c = 3.00×10^8 m/s

The energy must be greater than or equal to 1×10^-18 J

1×10^-18 J ≤ (6.626×10^-32 J·s)*(3.0×10^8 m/s) / x

x ≤ (6.626×10^-32 J·s)*(3.0×10^8 m/s) / (1×10^-18 J)

x ≤ 1.99×10^-7 m or 199 nm

The wavelength of light must be greater than or equal to 199 nm

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Answer:

The correct answer is "11.44 ml".

Explanation:

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As we know,

⇒  Molarity=\frac{No. \ of \ moles }{Volume \ of \ solution}

or,

⇒  No. \ of \ moles=Molarity\times Volume

On putting the values, we get

⇒                         =0.2\times 1

⇒                         =0.2 \ moles

Now,

⇒  No. \ of \ moles=\frac{Mass \ taken}{Molecular \ mass}

or,

⇒  Mass \ taken=No. \ of \ moles\times Molecular \ mass

⇒                      =0.2\times 60.05

⇒                      =12.01 \ gram

hence,

⇒  Density= \frac{Mass }{Volume}

or,

⇒  Volume=\frac{Mass}{Density}

⇒                =\frac{12.01}{1.05}

⇒                =11.44 \ ml

7 0
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