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jonny [76]
3 years ago
14

How many particles are in 7.07x10^-6 moles of a substance?

Chemistry
1 answer:
Butoxors [25]3 years ago
5 0

Answer:

4.25*10^18

Explanation:

1 mole =6.023*10^23 particles

so 7.07*10^-6 mole=6.023*10^23*7.07*10^-6 particles=4.25*10^18 particles

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artcher [175]
Infrared (IR) spectroscopy uses infrared radiation to excite the molecules of a compound and generates an infrared spectrum of the energy absorbed by a molecule as a function of the frequency or wavelength of light
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3 years ago
A 0.4272 g sample of an element contains 2.241 x 10 ^21 atoms . what is the symbol of the element?
grin007 [14]

Answer:

Likely \rm In (indium.)

Explanation:

Number of atoms: N = 2.241 \times 10^{21}.

Dividing, N, the number of atoms by the Avogadro constant, N_A \approx 6.023 \times 10^{23} \; \rm mol^{-1}, would give the number of moles of atoms in this sample:

\begin{aligned} n &= \frac{N}{N_{A}} \\ &\approx \frac{2.241 \times 10^{21}}{6.023 \times 10^{23}\; \rm mol^{-1}} \approx 3.72 \times 10^{-3}\; \rm mol \end{aligned}.

The mass of that many atom is m = 0.4272\; \rm g. Estimate the average mass of one mole of atoms in this sample:

\begin{aligned}M &= \frac{m}{n} \\ &\approx \frac{0.4272\; \rm g}{3.72 \times 10^{-3}\; \rm mol} \approx 114.82\; \rm g \cdot mol^{-1}\end{aligned}.

The average mass of one mole of atoms of an element (114.82\; \rm g \cdot mol^{-1} in this example) is numerically equal to the average atomic mass of that element. Refer to a modern periodic table and look for the element with average atomic mass 114.82. Indium, \rm In, is the closest match.

5 0
3 years ago
How do the physical and chemical properties the halogens compare with those of the noble gases? ​
KonstantinChe [14]

Explanation:

To form bonds with noble gases, a lot of energy is required to form those bonds. Halogens, on the other hand, are extremely reactive. ... The halogens tend to be very reactive, while the noble gases are in no way reactive and don't bond easily, if at all.

5 0
2 years ago
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Carbon dioxide, when it is at -145 degreesC has a density of 2.54 g/L. What is the pressure in torr??
Black_prince [1.1K]

Answer: The pressure in torr is 461 torr

Explanation:

To calculate the relation of density and molar mass of a compound, we use the ideal gas equation:

PV=nRT

P = pressure

V = Volume

n = number of moles

R = gas constant = 0.0821 Latm/Kmol

T = temperature =-145^0C=(273-145)K=128K

Number of moles (n) can be written as:

n=\frac{m}{M}

where, m = given mass

M = molar mass  = 44 g/mol

PV=\frac{m}{M}RT\\\\PM=\frac{m}{V}RT

where,

\frac{m}{V}=d

where d = density = 2.54 g/L

The relation becomes:

PM=dRT  

P=\frac{dRT}{M}

P=\frac{2.54\times 0.0821\times 128}{44}=0.607atm

P=461torr    (760torr=1atm)

Thus the pressure in torr is 461 torr

5 0
3 years ago
A spring is stretched 55 cm from its testing position. If the spring's constant of proportionality is 15N / m , what is the spri
dimaraw [331]

Answer:2.27 J

Explanation:Because that’s what it was in ck12 so ion got no explanation

4 0
3 years ago
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