For the reaction $H^{+}+Br{O}_3^{-}+3B{r}^{-}\to 5B{r}_2+H_{2}O$ which of the following relation correctly represents the consumption & formation of reactants and product:

Q. For a reaction, $2N{H}_3⟶N_2+3H_2$, it is observed that:

Q. For a gaseous reaction, $A\left(g\right)⟶$ Product, which one of the following is correct relation among $\frac{dP}{dt},\frac{dn}{dt}$ and $\frac{dc}{dt}$?
($\frac{dP}{dt}=$ Rate of reaction in $atm$ ${sec}^{-1}$; $\frac{dc}{dt}=$ Rate of reaction in molarity ${sec}^{-1}$; $\frac{dn}{dt}=$ Rate of reaction in $mol$ ${sec}^{-1}$)

Q. For a reaction: $xA+yB\to zC$, if $-\frac{d\left[A\right]}{dt}=-\frac{d\left[B\right]}{dt}=1.5\frac{d\left[C\right]}{dt}$; then $x,y$ and $z$ are:

Q. In the following reaction, how is the rate of appearance of product related to the rate of disappearance of the reactant?
$Br{O}_3^{-}\left(aq\right)+5B{r}^{-1}\left(aq\right)+6H^{+}\to 3B{r}_2\left(l\right)+2H_{2}O\left(l\right)$

Q. For the reaction, \(BrO_3^-(aq)+5Br^-(aq)+6H^+ \to 3Br_2(l)+3H_2O(l)\), the rate equation can be expressed in two ways
\(\dfrac{d[Br_2]}{dt}= k [Br^-][BrO_3][H^+]^2\) and
\(-\dfrac{d[Br^-]}{dt}= k ' [Br^-][BrO_3][H^+]^2\)
Here, k and k' are related as