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3 years ago

Significant Figures For 7.06 × 10^5 ÷ 5.3 × 10^-2

Chemistry

1 answer:

Kay [80]3 years ago

4 0

Answer:

$\boxed{\text{two}}$

Explanation:

In multiplication and division problems, your answer can have no more significant figures than the number with the fewest significant figures.

$\dfrac{7.06 \times 10^{5}}{5.3 \times 10^{-2}}= 1.332 075 472 \times 10^{7}$ (by my calculator)

There are three significant figures in 7.06 and two in 2.3.

You must round to $\boxed{\textbf{two}}$ significant figures and report the answer as 1.3 × 1.0⁷.

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Ultraviolet radiation and radiation of shorter wavelengths can damage biological molecules because they carry enough energy to b

Lelechka [254]

Answer:

343.98 nm is the longest wavelength of radiation with enough energy to break carbon–carbon bonds.

Explanation:

A typical carbon–carbon bond requires 348 kJ/mol=348000 J/mol

Energy required to breakl sigle C-C bond:E

$E=\frac{348000 J/mol}{6.022\times 10^{23} mol^{-1}}=5.7788\times 10^{-19} J$

$E=\frac{h\times c}{\lambda}$

where,

E = energy of photon

h = Planck's constant = $6.626\times 10^{-34}Js$

c = speed of light = $3\times 10^8m/s$

$\lambda$ = wavelength of the radiation

Now put all the given values in the above formula, we get the energy of the photons.

$\lambda =\frac{(6.63\times 10^{-34}Js)\times (3\times 10^8m/s)}{5.7788\times 10^{-19} J}$

$\lambda =3.4398\\times 10^{-7}m=343.98 nm$

$1 m = 10^{9} nm$

343.98 nm is the longest wavelength of radiation with enough energy to break carbon–carbon bonds.

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3 years ago

And ironic bonds what happens to electrons? No

iren [92.7K]

Answer:

metals donate electrons to nonsmetals

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3 years ago

How many moles are in 7.46 x 1025 particles of iron

sladkih [1.3K]

Answer:

1 mole of iron =6.023×10^23 particles

1 particles of iron=1/6.023×10^23 mole

7.46×10^25 particles =1/6.023×10^23×7.46×10^25

=1.238×10^48 mole is a required answer.

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2 years ago

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rusak2 [61]

Answer:

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