Which of the following plots is correct for a zero-order reaction?

If doubling the initial concentration of reactant doubles $t_{1/2}$ of reaction,the order of reaction is

The rate constant,$k$ of a zero order reaction $2 NH_{3(g)} \xrightarrow[1130 \ K]{Pt} N_{2(g)} + 3 H_{2(g)}$ is $y \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$. The rate of formation of hydrogen (in $mol \ L^{-1} \ s^{-1}$) is

The rate constant of a zero-order reaction is $0.2 \ mol \ m^{-3} \ h^{-1}$. If the concentration of the reactant after $30 \ minutes$ is $0.05 \ mol \ m^{-3}$,then its initial concentration will be ....... $mol \ m^{-3}$.

For a zero order reaction,the plot of concentration $(a - x)$ $vs$ time is linear with

What is the half-life time of a reaction? Derive the equation of half-life time $(t_{1/2})$ for a zero-order reaction.