In the following reaction: $xA \to yB$,$\log \left[ -\frac{d[A]}{dt} \right] = \log \left[ \frac{d[B]}{dt} \right] + \log 2$,where the negative sign indicates the rate of disappearance of the reactant. Thus,$x : y$ is:

At $298 \ K$ the value of $-\frac{\Delta[Br^{-}]}{\Delta t}$ for the reaction$5Br^-{_{\text{(aq)}}} + BrO_3^-{_{\text{(aq)}}} + 6H^+{_{\text{(aq)}}} \rightarrow 3Br_{2\text{(aq)}} + 3H_2O_{\text{(l)}}$ is $x \ mol \ L^{-1} \ min^{-1}$. What is the rate (in $mol \ L^{-1} \ min^{-1}$) of this reaction?

For the reaction $4NH_3 + 5O_2 \to 4NO + 6H_2O$,if the rate of disappearance of $NH_3$ is $3.6 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$,what is the rate of formation of $H_2O$?

The rate of a reaction that does not involve gases is not dependent on:

For a general chemical reaction $2A + 3B \rightarrow \text{Products}$,if the rate of disappearance of $A$ is $r_1$ and that of $B$ is $r_2$,then the relationship between $r_1$ and $r_2$ is:

For the chemical reaction: $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the rate of reaction can be expressed in terms of the concentration of $N_{2(g)}$,$H_{2(g)}$,or $NH_{3(g)}$ with respect to time. Identify the correct relationship between these rates.