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Alex777 [14]
3 years ago
5

Explain how to convert a mass of compound A to a mass of compound D in words with no equations using the following reaction 2A +

4B -> C + 3D​
Chemistry
1 answer:
leonid [27]3 years ago
8 0

Answer:

Explanation:

The given reaction equation is:

                2A + 4B → C + 3D

We know the mass of compound A in the reaction above. We are to find the mass of compound D.

We simply work from the known mass to calculate the mass of the unkown compound D

Using the mole concept, we can find the unknown mass.

Procedures

  • We first find the molar mass of the compound A from the atomic units of the constituent elements.
  • We then use the molar mass of A to calculate its number of moles using the expression below:  

            Number of moles of A = \frac{mass of A}{molar mass of A}

  • Using the known number of moles of A, we can work out the number of moles of D.

           From the balanced equation of the reaction, it is shown that:

         2 moles of compound A was used up to produced 3 moles of D

  Then \frac{3}{2} x number of moles of A would give the number of moles of D

  • Now that we know the number of moles of D, we can find its mass using the expression below:

             Mass of D = number of moles of D x molar mass of D

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kondaur [170]

Answer: The most likely partial pressures are 98.7MPa for NO₂ and 101.3MPa for N₂O₄

Explanation: To determine the partial pressures of each gas after the increase of pressure, it can be used the equilibrium constant Kp.

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P(N₂O₄) = 200 - P(NO₂)

Kp = \frac{P(N_{2}O_{4} )}{P(NO_{2} ^{2}) }

0.0104 = \frac{200 - P(NO_{2})  }{[P(NO_{2} )]^{2}}

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P(N₂O₄) = 200 - P(NO₂)

P(N₂O₄) = 200 - 98.7

P(N₂O₄) = 101.3

The partial pressures are P(NO_{2} ) = 98.7 MPa and P(N₂O₄) = 101.3 MPa

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