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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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Solid ammonium chloride, NH4Cl, is formed by the reaction of gaseous ammonia, NH3, and hydrogen chloride, HCl. NH3(g)+HCl(g)⟶NH4
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9.41 atm is the pressure in atmospheres of the gas remaining in the flask

<h3>What is the pressure in atmospheres?</h3>

The equation NH3(g) + HCl(g) ==> NH4Cl(s) is balanced.

Divide the moles of each reactant by its coefficient in the balanced equation, and the limiting reagent is identified as the one whose value is less. With the issue we now have...

6.44 g NH3 times 1 mol NH3/17 g equals 0.3688 moles of NH3 ( 1 = 0.3688)

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NH4Cl will this reaction produce in grams

0.1764 moles of HCl multiplied by one mole of NH4Cl per mole of HCl results in 9.44 g of NH4Cl (3 sig. figs.)

the gas pressure, measured in atmospheres, that is still in the flask

NH3(g) plus HCl(g) results in NH4Cl (s)

0.3688......0.1764............0..........

Initial

-0.1764....-0.1764........+0.1764...Change

Equilibrium: 0.1924.......0...............+0.1924

There are 0.1924 moles of NH3 and no other gases in the flask. This is at a temperature of 25 °C (+273 = 298 °K) in a volume of 0.5 L. After that, we may determine the pressure by using the ideal gas law (P).

PV = nRT

P = nRT/V = 0.1924 mol, 0.0821 latm/mol, and 298 Kmol / 0.5 L

P = 9.41 atm

9.41 atm is the pressure in atmospheres of the gas remaining in the flask

To learn more about balanced equation refer to:

brainly.com/question/11904811

#SPJ1

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