The reaction between `Cr_(2)O_(7)^(2-)` and `HNO_(2)` in an acidic medium is
`Cr_(2)O_(7)^(2-) + 5H^(o+) + 3HNO_(2) rarr 2Cr^(3+) + 3NO_(3)^(ɵ) + 4H_(2)O`.
The rate of disappearance of `Cr_(2)O_(7)^(2-)` is found to be `2.4 xx 10^(-4) mol L^(-1) s^(-1)` during measured time interval. What will be the rate of disappearance of `HNO_(2)` during the same time interval?

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

According to the Cr_(2)O_(7)^(2-)+5H^(+)+3HNO_(2) → 2Cr ^ (3+) +3NO_ (3)^(−)+4H_(2) O The rate of disappearance of Cr_(2)O_(7)^(2-) is found to be 2.4 xx10^(-4) mol L^(-1) S^(-1) find the rate of appearance of Cr^(3+) during given time interval

In the reaction the stoichiometry coefficients of Cr_(2)O_(7)^(2-) , NO_2^(-) and H^(+) respectively are Cr_(2)O_(7)^(2-) +NO_(2)^(-) +H^(+) rarr Cr^(3+) +NO_(3)^(-) +H_(2)O

In the reaction the stoichiometry coefficients of Cr_(2)O_(7)^(2-), NO_(2)^(-) and H^(+) respectively are Cr_(2)O_(7)^(2-)+NO_(2)^(-)+H^(+)rarrCr^(3+)+NO_(3)^(-)+H_(2)O

In the reaction: Cr_(2)O_(7)^(2-) + 14H^(o+) + 6I^(Ө) rarr2Cr^(3+) + 3H_(2)O + 3I_(2) Which element is reduced?

In the reaction: Cr_(2)O_(7)^(2-) + 14H^(o+) + 6I^(Ө) rarr2Cr^(3+) + 3H_(2)O + 3I_(2) Which element is reduced?