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postnew [5]
3 years ago
10

The equilibrium: 2 NO2(g) \Longleftrightarrow⇔ N2O4(g) has Kc = 4.7 at 100ºC. What is true about the rates of the forwar

d (ratefor) and reverse (raterev) reactions initially and at equilibrium if an empty container is filled with just NO2?
Initial: forward rate < reverse rate Equilibrium: forward rate > reverse rate
Initial: forward rate > reverse rate Equilibrium: forward rate > reverse rate
Initial: forward rate > reverse rate Equilibrium: forward rate = reverse rate
Initial: forward rate = reverse rate Equilibrium: forward rate = reverse rate
Chemistry
1 answer:
Sergeeva-Olga [200]3 years ago
7 0

Answer:

  • Initial: forward rate > reverse rate
  • Equilibrium: forward rate = reverse rate

Explanation:

2NO₂(g) → N₂O₄(g)   Kc=4.7

The definition of <em>equilibrium</em> is when the forward rate and the reverse rate are <em>equal</em>.

Because in the initial state there's only NO₂, there's no possibility for the reverse reaction (from N₂O₄ to NO₂). Thus the forward rate will be larger than the reverse rate.

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See whole explanation to understand

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The combustion of propane may be described by the chemical equation C 3 H 8 ( g ) + 5 O 2 ( g ) ⟶ 3 CO 2 ( g ) + 4 H 2 O ( g ) C
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Answer: 72 grams of O_2(g) are needed to completely burn 19.7 g C_3H_8(g)

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To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Putting in the values we get:

\text{Number of moles}=\frac{19.7g}{44g/mol}=0.45moles

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7 0
3 years ago
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