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bekas [8.4K]
3 years ago
7

Enter your answer in the provided box. On a certain winter day in Utah, the average atmospheric pressure is 718 torr. What is th

e molar density (in mol/L) of the air if the temperature is −29°C?
Chemistry
1 answer:
AnnZ [28]3 years ago
7 0

Answer:

The correct answer is 0.047 mol/L

Explanation:

The atmospheric air is a mixture of gases. We can assume an ideal behavior of the gas and use the ideal gas equation:

PV= nRT

where P is the pressure, V is the volume, n is the number of moles, R is a constant (0.082 L.atm/K.mol) and T is the temperature in K.

We have to first convert the pressure from Torr to atm:

760 Torr= 1 atm

⇒ 718 Torr x 1 atm/760 Torr = 0.945 atm

Then, we convert the temperature from ºC to K:

0ºC = 273 K

⇒ -29ºC+273= 244 K

Finally, we introduce the data in the equation and calculate de densitiy, which is the moles per liters of gas (n/V):

PV = nRT

n/V= P/RT

n/V = (0.945 atm)/(0.082 L.atm/K.mol x 244 K) = 0.047 mol/L

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1 year ago
An unknown amount of mercury (II) oxide was decomposed in the lab. Mercury metal was formed and 5.20 L of oxygen was released at
Yakvenalex [24]

Answer:

  • <u>68.3g</u>

Explanation:

<u>1. Word equation:</u>

  • <em>mercury(II) oxide → mercury + oxygen </em>

<u>2. Balanced molecular equation:</u>

  • 2HgO → 2Hg + O₂(g)

<u>3. Mole ratio</u>

Write the ratio of the coefficients of the substances that are object of the problem:

       2molHgO/1molO_2

<u>4. Calculate the number of moles of O₂(g)</u>

Use the equation for ideal gases:

          pV=nRT\\\\\\n=\dfrac{pV}{RT}\\\\\\n=\dfrac{0.970atm\times5.20L}{0.08206atm.L/K.mol\times 390.0K}\\\\\\n=0.1576mol

<u>5. Calculate the number of moles of HgO</u>

         \dfrac{2molHgO}{1molO_2}\times 0.1576molO_2=0.315molHgO

<u>6. Convert to mass</u>

  • mass = # moles × molar mass

  • molar mass of HgO: 216.591g/mol

  • mass = 0.315mol × 216.591g/mol = 68.3g

7 0
2 years ago
Which material gives the soil its high fertility?
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Answer:

Explanation:

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2 years ago
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