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Naily [24]
2 years ago
11

Determine the theoretical yield of H2S (in moles) if 4.0 molAl2S3 and 4.0 mol H2O are reacted according to the followingbalanced

reaction. A possibly useful molar mass is Al2S3 =150.17Al2S3(s)+6H2O(l)-->2Al(OH)3(s)+3H2S(g)
Chemistry
1 answer:
mamaluj [8]2 years ago
7 0

Answer:

The theoretical yield of the hydrogen sulfide is 68.0 grams.

Explanation:

Al_2S_3(s)+6H_2O(l)\rightarrow 2Al(OH)_3(s)+3H_2S(g)

Moles of aluminum sulfide = 4.0 mol

Moles of water = 4.0 mol

According to reaction, 6 moles of water reacts with 1 mole of aluminum sulfide,then 4 moles of water will react with :

\frac{1}{6}\times 4 mol=1.5 mol of aluminum sulfide

1.5 moles aluminum sulfide < 4 moles  aluminum sulfide

This means that water is present in limiting amount and aluminum sulfide is in excess amount.So, amount of hydrogen sulfide will depend upon moles of water.

According to reaction, 6 moles of water gives with 3 mole of hydrogen sulfide,then 4 moles of water will give :

\frac{3}{6}\times 4 mol=2.0 mol of hydrogen sulfide

Mass of hydrogen sulfide:

2.0 mol × 34 g/mol = 68.0 g

The theoretical yield of the hydrogen sulfide is 68.0 grams.

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Write a net ionic equation for the reaction that occurs when nickel(ii carbonate and excess hydrobromic acid (aq are combined.
seropon [69]
First, we write the reaction equation:
NiCO₃ + 2HBr → NiBr₂ + H₂CO₃

Now, writing this in ionic form:
NiCO₃ + 2H⁺ + 2Br⁻ → NiBr₂ + 2H⁺ + CO₃⁻²

(NiCO₃ is insoluble so it does not dissociate in to ions very readily)

Overall equation:
NiCO₃ + 2Br⁻ → NiBr₂ + CO₃⁻²
7 0
2 years ago
How did surgeon Joseph Lister kill the bacteria in urine specimens he had been studying?
stiks02 [169]

Answer:

A.He added bleach to the samples.

Explanation:

Bleach destroys the chemical composition of bacteria. Adding mold spores, freezing samples, and raising the temperature all result in physical changes, but not chemical changes, so specimens remain alive.

3 0
2 years ago
The heat of vaporization (∆Hvap) of the element mercury (Hg) is 59.0 kJ/mol. If the vapor pressure of Hg is 0.0017 torr at 25°C,
astra-53 [7]

Answer:

Tb Hg = 656.726 K

Explanation:

normal boiling point (Tb):

Clasius-Clapeyron's law:

  • Tb = [(RLn(Po)/ΔHv) + (1/To)]∧(-1)

∴ R = 8.314 J/K.mol

∴To = 25°C ≅ 298 K

∴ Po = 0.0017 torr = 2.24 E-6 atm

∴ ΔHv = 59.0 KJ/mol = 59000 J/mol

⇒ Tb = [(8.314 J/K.mol)Ln(2.24 E-6))/(59000 J/mol)) + (1/298 K)]∧(-1)

⇒ Tb = [- 1.833 E-3 K-1 + 3.355 E-3 K-1 ]∧(-1)

⇒ Tb = [1.523 E-3]∧(-1)

⇒ Tb = 656.726 K

6 0
2 years ago
1. Calculate the molarity of a sugar solution if 4 liters of the solution contains 8 moles of sugar
klio [65]

Answer:

The molarity of a sugar solution is 2 M.

Explanation:

Molarity is a concentration measure that expresses the moles of solute per liter of solution. In this case it is calculated with the simple rule of three:

4 L of solution--------8 moles of sugar

1 L of solution ------x= (1 L of solution x 8 moles of sugar)/4 L of solution

x=2 moles of sugar---> <em>The solution is 2M</em>

8 0
2 years ago
Nitrogen dioxide (NO2) cannot be obtained in a pure form in the gas phase because it exists as a mixture of NO2 and N2O4. At 16°
Pavel [41]

Answer:

PNO₂ = 0.49 atm

PN₂O₄ = 0.45 atm

Explanation:

Let's begin with the equation of ideal gas, and derivate from it an equation that  involves the density (ρ = m/V).

PV = nRT

n = m/M (m is the mass, and M the molar mass)

PV = \frac{m}{M}RT

PxM = \frac{m}{V}RT

PxM = ρRT

ρ = PxM/RT

With the density of the gas mixture, we can calculate the average of molar mass (Mavg), with the constant of the gases R = 0.082 atm.L/mol.K, and T = 16 + 273 = 289 K

2.7 = \frac{0.94xMavg}{0.082x289}

0.94Mavg = 63.9846

Mavg = 68.0687 g/mol

The molar mass of N is 14 g/mol and of O is 16 g/mol, than M_{NO2} = 46 g/mol and M_{N2O4} = 96 g/mol. Calling y the molar fraction:

Mavg = M_{NO2}y_{NO2} + M_{N2O4}y_{N2O4}

And,

y_{NO2} + y_{N2O4} = 1

y_{N2O4} = 1 - y_{NO2}

So,

68.0687 = 46y_{NO2} + 92x(1 - y_{NO2})

68.0687 - 92 = 46y_{NO2} - 92y_{NO2}

46y_{NO2} = 23.9313

y_{NO2} = 0.52

y_{N2O4} = 0.48

The partial pressure is the molar fraction multiplied by the total pressure so:

PNO₂ = 0.52x0.94 = 0.49 atm

PN₂O₄ = 0.48x0.94 = 0.45 atm

8 0
2 years ago
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