4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
a. Calculate the average rate of reaction with respect to NH3 .b. Calculate the average rate at which H2O is being formed.c. Calculate the average rate at which O2 is being consumed.
For the reaction below, initially 3.5 mol of NH3 are placed in a 4.0 L reaction chamber. After 3.0 minutes only 1.6 moles of NH3 remain. ?
2020-07-10 12:02 am
回答 (1)
2020-07-10 1:34 am
a.
Decrease in concentration of NH₃ in 3 min
= [(3.5 - 1.6) mol] / (4 L)
= 0.475 M
Average rate of reaction at which NH₃ is being consumed
= (0.475 M) / (3 min)
= 0.16 M/min (to 2 sig. fig.)
====
b.
According to the equation, mole ratio NH₃ : H₂O = 4 : 6
Average rate of reaction at which H₂O is being formed
= (0.16 M/min) × (6/4)
= 0.24 M/min
====
c)
According to the equation, mole ratio NH₃ : O₂ = 4 : 5
Average rate of reaction at which O₂ is being consumed
= (0.16 M/min) × (5/4)
= 0.20 M/min
Decrease in concentration of NH₃ in 3 min
= [(3.5 - 1.6) mol] / (4 L)
= 0.475 M
Average rate of reaction at which NH₃ is being consumed
= (0.475 M) / (3 min)
= 0.16 M/min (to 2 sig. fig.)
====
b.
According to the equation, mole ratio NH₃ : H₂O = 4 : 6
Average rate of reaction at which H₂O is being formed
= (0.16 M/min) × (6/4)
= 0.24 M/min
====
c)
According to the equation, mole ratio NH₃ : O₂ = 4 : 5
Average rate of reaction at which O₂ is being consumed
= (0.16 M/min) × (5/4)
= 0.20 M/min
收錄日期: 2021-04-18 18:33:17
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