The reaction between `Cr_(2)O_(7)^(2-) and HCO_(2)` in an acidic medium is : `Cr_(2)O_(7)^(2)+5H^(+)+2HNO_(2)rarr2 Cr^(3+)+3NO_(3)^(-)+4H_(2)O` The ra

Question

The reaction between `Cr_(2)O_(7)^(2-) and HCO_(2)` in an acidic medium is : `Cr_(2)O_(7)^(2)+5H^(+)+2HNO_(2)rarr2 Cr^(3+)+3NO_(3)^(-)+4H_(2)O` The ra

The reaction between `Cr_(2)O_(7)^(2-) and HCO_(2)` in an acidic medium is :
`Cr_(2)O_(7)^(2)+5H^(+)+2HNO_(2)rarr2 Cr^(3+)+3NO_(3)^(-)+4H_(2)O`
The rate of disappearance of `Cr_(2)O+_(7)^(2-)` is found to be `2.4xx10^(-4)"mol" L^(-1)s^(-1)` during a meausred time interval. Find the rate of disppearanceo of `HNO_(2)` and the rate of appearance of `Cr^(3+)` during this time interval

Monjur Alahi

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2025-01-04 04:42

1 Answers

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Salim Ahmed Kawsar · Accepted Answer · 2023-02-05T15:29:48+06:00

The equality in this case is :
`-(Delta[Cr_(2)O_(7)^(2-)])/(Deltat)=-(1)/(3)(Delta[HNO_(2)])/(Deltat)=(1)/(2)(Delta[Cr^(3+)])/(Deltat)`
It is given than,
`-(Delta[Cr_(2)O_(7)^(2-)])/(Deltat)=2.4xx10^(-4)"mol"L^(-1)s^(-1)`
So, `(Delta[HNO_(2)])/(Deltat)=3xx2.4xx10^(4)=7.2xx10^(-4)"mol"L^(-1)s^(-1)`
and `(Delta[Cr^(3+)])/(Deltat)=2xx2.4xx10^(-4)=4.8xx10^(-4)"mol" L^(-1)s^(-1)`