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IceJOKER [234]
3 years ago
5

A container of what volume would be required to store 60.0 moles of a gas at a pressure of 20.0 atm and a temperature of 50.0 Ce

lsius? 12.3 L 79.6 L 8060 L 1250 L
Chemistry
1 answer:
belka [17]3 years ago
7 0

Answer:

The answer to your question is:  79.6 L

Explanation:

Data:

n = 60 moles

Pressure = P = 20.0 atm

Temperature = T = 50°C

Volume = V = ?

Convert temperature to Kelvin

      °K = 273 + 50

      °K = 323

Formula  (ideal gas law)

               PV = nRT        solve for V

              V = nRT / P

             V = (60)(0.08206)(323) / 20        Substitution

            V = 1590.32 /20                    

             V = 79.6 L

               

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(a): 2,300 kilograms

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(c): 2.3 × 10^-5 kilograms

(d): 155 kilograms

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1. Based on the observed performance of the air bag models and the amounts of sodium bicarbonate and acetic acid (vinegar) neede
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Sodium bicarbonate and acetic acid are not good substitute for sodium azide in airbags since the require more mass and produce less gas.

<h3>Which is the better chemical for an airbag?</h3>

The chemical equation for the production of nitrogen gas from sodium azide is given below:

  • NaN₃ → 2 Na + 3 N₂

1 mole or 66 go of sodium azide produces 3 moles or 67.2 L of nitrogen gas.

The equation for the production of carbon dioxide from sodium bicarbonate and acetic acid is given below:

  • Na₂CO₃ + CH₃COOH → CH₃COONa + CO₂ + H₂O

1 mole, 106 g of Na₂CO₃ and 1 mole, 82 g of CH₃COOH are required to produce 1 mole or 22.4 L of CO₂.

The mass of sodium azide required is less than that of sodium bicarbonate and acetic acid required. Also, sodium azide produces a greater volume of gas. Therefore, sodium bicarbonate and acetic acid are not good substitute for sodium azide in airbags.

In conclusion, sodium azide is a better choice in airbags.

Learn more about airbags at: brainly.com/question/14954949

#SPJ1

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