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shusha [124]
3 years ago
6

g Determine the value of the equilibrium constant for this reaction if an initial concentration of N2O4(g) of 0.040 mol/L is red

uced to 0.0055 mol/L at equilibrium. There is no NO2(g) present at the start of the reaction.
Chemistry
1 answer:
jeyben [28]3 years ago
7 0

Answer:

Explanation:

N₂O₄(g) ⇄ 2 NO₂

N₂O₄ reacted = .04 - .0055 = .0345 mole

NO₂ formed = 2 x .0345 = .069 moles

equilibrium constant = [ NO₂ ] ² / [ N₂O₄]

= .069² / .0055

= 0.865 .

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2 years ago
Consider the following isotopic abundance data for argon (Ar) and silicon (Si):
pshichka [43]

Answer:

Explanation:

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= 35.96755 x .00337 + 37.96272 x .00063 + 39.96240 x .99600

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= 16.76 x 10²³ .

c )

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42Ar = 41.95

2 )

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7 0
3 years ago
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