Consider the reaction
`3I_(aq)^(-) +S_2O_(8(aq))^(2-) rarr I_(3(aq))^(-)+2SO_(4(aq))^(2-)`
At a particular time t, `(d[SO_4^(2-)])/(dt) = 2.2xx10^(-2) M//s` What are the values of
`-(d[S_2O_8^(2-)])/(dt)` at the same time?

Consider the reaction 3I_(aq)^(-) +S_2O_(8(aq))^(2-) rarr I_(3(aq))^(-)+2SO_(4(aq))^(2-) At a particular time t, (d[SO_4^(2-)])/(dt) = 2.2xx10^(-2) M//s What are the values of (d[I_3^-])/(dt) at the same time?

Consider the reaction 3I_(aq)^(-) +S_2O_(8(aq))^(2-) rarr I_(3(aq))^(-) +2SO_(4(aq))^(2-) At a particular time t, (d[SO_4^(2-)])/(dt) = 2.2xx10^(-2) M//s What are the values of -(d[I^-])/(dt) at the same time?

Consider the following redox reaction Mg_((S)) +Sn_((aq))^(2+) rarr Mg_((aq))^(2+)+Sn_((s)) : Write the cell formula.

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For the reaction, 3I^(o-)(aq) + S_2O_8^(2(o-))(aq)rarr I_3^(o-) (aq) + 2 SO_4^(2(o-))(aq) Calculate the rate of formation of I_3^(o-) , the rates of consumption of I^- and S_2O_8^(2(o-)) and' the overall rate of reaction if the rate of formation of SO_4^(2(o-)) is 0.022M/s

Balance the following equation stepwise. NaOH_((aq))+H_2SO_(4(aq))rarrNa_2SO_(4(aq))+H_2O_((l))

Balance the following equation stepwise. SO_(2(g))+H_2S_((aq))rarrS_((s))+H_2O_((l))

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Consider the reaction 2N_(2) O_(5(g) ) to 4NO_(2(g)) +O_(2(g)) in liquid bromine If -(d[N_(2)O_(5) ])/(dt)=0.02 M s^(-1) then NO_(2) is formed at _______.

Consider the reaction 2NO_(g)+O_(2(g))rarr 2NO_(2(g)) . If (d[NO_2])/(dt) = 0.052M//s then -(d[O_2])/(dt) will be