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REY [17]
3 years ago
11

Gallium (Ga) consists of two naturally occurring isotopes with masses of 68.926 and 70.925 amu.

Chemistry
1 answer:
almond37 [142]3 years ago
5 0

Answer:

Part A. p, n = 31, 38.

Part B. p, n = 31, 40.

Part C. ^{69}_{31}Ga,\ ^{71}_{31}Ga

Explanation:

Hello,

Part A.

In this case, since the atomic number for gallium is 31, we can say that the first isotope has also 31 protons and the neutrons are computed by using its molar mass as a whole number (69):

neutrons=mass-protons=69-31=38

Thus, result is p, n = 31, 38.

Part B.

In this case, since the atomic number for gallium is 31, we can say that the second isotopes has also 31 protons and the neutrons are computed by using its molar mass as a whole number (71):

neutrons=mass-protons=71-31=40

Thus, result is p, n = 31, 40.

Part C.

Finally, the isotopes as shown as:

^{69}_{31}Ga,\ ^{71}_{31}Ga

Best regards.

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How many molecules are in 7.62 L of CH4, at 87.5°C and 722 torr
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Answer: There are 1.469 \times 10^{23} molecules present in 7.62 L of CH_4 at 87.5^{o}C and 722 torr.

Explanation:

Given : Volume = 7.62 L

Temperature = 87.5^{o}C = (87.5 + 273) K = 360.5 K

Pressure = 722 torr

1 torr = 0.00131579

Converting torr into atm as follows.

722 torr = 722 torr \times \frac{0.00131579 atm}{1 torr}\\= 0.95 atm

Therefore, using the ideal gas equation the number of moles are calculated as follows.

PV = nRT

where,

P = pressure

V = volume

n = number of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into above formula as follows.

PV = nRT\\0.95 atm \times 7.62 L = n \times 0.0821 L atm/mol K \times 360.5 K\\n = \frac{0.95 atm \times 7.62 L}{0.0821 L atm/mol K \times 360.5 K}\\= \frac{7.239}{29.59705}\\= 0.244 mol

According to the mole concept, 1 mole of every substance contains 6.022 \times 10^{23} atoms. Hence, number of atoms or molecules present in 0.244 mol are calculated as follows.

0.244 mol \times 6.022 \times 10^{23}\\= 1.469 \times 10^{23}

Thus, we can conclude that there are 1.469 \times 10^{23} molecules present in 7.62 L of CH_4 at 87.5^{o}C and 722 torr.

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3 years ago
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