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Maurinko [17]
3 years ago
10

A flask filled with oxygen is heated from 5 degrees Celsius to 30 degrees Celsius. The starting pressure was 50 kPa, what is the

final pressure? (Be sure to convert from Celsius to Kelvin, add 273 to your Celsius temperature to get the temperature to kelvin. Ex. 0 degrees Celsius id equal to 273 kelvin)
Chemistry
1 answer:
rewona [7]3 years ago
6 0

54.5kPa

Explanation:

Given parameters:

T₂ = 30°C = 30+273 = 303K

T₁ =  5°C = 5+273 = 278K

P₁ = 50kPa

Unknown:

P₂ = ?

Solution:

We can solve this problem using the combined gas law simplification and assuming that volume is constant as seen from the container:

            \frac{P_{1} }{T_{1} } =  \frac{P_{2} }{T_{2} }

Making the unknown the subject of the formula:

            P₂ = \frac{P_{1} T_{2} }{T_{1} }

             P₂ = \frac{50 x 303}{278} = 54.5kPa

Learn more:

Ideal gas brainly.com/question/9321544

#learnwithBrainly

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Answer:

In conclussion, 0.60 moles of HCOOH contains the greatest mass of O

Explanation:

Let's make some rules of three, to solve this problem:

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The question is incomplete. There's missing the image, which is shown below.

Answer:

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Explanation:

The reaction between hydrogen gas and oxygen gas to form water is:

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So, for 1 mol of O₂ is necessary 2 moles of H₂ form 2 moles of H₂O. As the images below there's 8 molecules of H₂, 4 molecules of O₂, 12 molecules in the mixture, and 8 molecules of H₂O. Thus, there are stoichiometric values.

All the images are at the same temperature and pressure, so, by the ideal gas law:

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The number of moles and molecules are related, so let's substitute it in the equation. For the H₂:

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