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Gnesinka [82]
3 years ago
13

A reaction between liquid reactants takes place at - 11.0 degree C in a sealed, evacuated vessel with a measured volume of 45.0

L. Measurements show that the reaction produced 35. g of chlorine pentafluoride gas. Calculate the pressure of chlorine pentafluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid of reactants. Be sure your answer has the correct number of significant digits.
Chemistry
1 answer:
Sati [7]3 years ago
4 0

Explanation:

The given data is as follows.

       T = 11^{o}C = (11 + 273) K = 284 K,     V = 45.0 L

      m = 35 g

As molar mass of chlorine pentafluoride is 130.445 g/mol. Hence, number of moles of chlorine pentafluoride are as follows.

      No. of moles = \frac{mass}{\text{molar mass}}

                             = \frac{35 g}{130.445 g/mol}

                             = 0.268 mol

Now, using the ideal gas equation we will find the pressure as follows.

                          PV = nRT

       P \times 45.0 L = 0.268 mol \times 0.082 L atm/mol K \times  284 K

                       P = 0.139 atm

Thus, we can conclude that pressure of chlorine pentafluoride gas in the given reaction vessel after the reaction is 0.139 atm.

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Answer:

8

Explanation:

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8 0
3 years ago
Whoever awser correct I will give you Brainly
vivado [14]

Answer:

Option A.

2Na + 2H2O —> 2NaOH + H2

Explanation:

To know which option is correct, we shall do a head count of the number of atoms present on both side to see which of them is balanced. This is illustrated below below:

For Option A:

2Na + 2H2O —> 2NaOH + H2

Reactant >>>>>>> Product

2 Na >>>>>>>>>>> 2 Na

4 H >>>>>>>>>>>> 4 H

2 O >>>>>>>>>>>> 2 O

Thus, the above equation is balanced.

For Option B:

2Na + 2H2O —> NaOH + H2

Reactant >>>>>>> Product

2 Na >>>>>>>>>>> 1 Na

4 H >>>>>>>>>>>> 3 H

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Thus, the above equation is not balanced.

For Option C:

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Reactant >>>>>>> Product

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2 H >>>>>>>>>>>> 4 H

1 O >>>>>>>>>>>> 2 O

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For Option D:

Na + 2H2O —> NaOH + 2H2

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Thus, the above equation is not balanced.

From the illustrations made above, only option A is balanced.

7 0
3 years ago
We have 1700 Tonnes of Amoniac every day. How many tonnes of 63% Nitrogen soda we can get?
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First the ammonia is oxidized:
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Then for the absorption of the nitrogen oxides.
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Lastly, the N2O4 is further oxidized into Nitric acid.
3N2O4 + 2H2O = 4HNO3 + 2NO

Then run stoichiometry through these equations.
The first equation produces roughly 271,722,938 grams of NO
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Convert the exact number back into tons, and your answer is: 419.332775 tons.

Rounded, I'm going to say that's 419.33 tons.
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Also, it seems that commercially, Nitric Acid is commonly made by bubbling NO2 into water, rather than using ammonia.
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Answer:

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Answer:

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