For a first order reaction, to obtain a positive slope, we need to plot where [A] is the concentration of reactant A

Question

For a first order reaction, to obtain a positive slope, we need to plot where [A] is the concentration of reactant A (A) -log10 [A] vs t (B) -loge [A] vs t (C) log10 [A] vs log t (D)  [A] vs t

Tardigrade Admin · Accepted Answer

For a first order reaction to obtain a positive slope, a graph is plotted between -loge [A] vs. t.

Q. For a first order reaction, to obtain a positive slope, we need to plot {where [A] is the concentration of reactant A}

$- l o g_{10} [A] v s t$

$- l o g_{e} [A] v s t$

$l o g_{10} [A] v s l o g t$

$[A] v s t$

For a first order reaction to obtain a positive slope, a graph is plotted between $- l o g_{e} [A] v s . t .$

Q. For a first order reaction, to obtain a positive slope, we need to plot {where [A] is the concentration of reactant A}

−log10​[A]vst

−loge​[A]vst

log10​[A]vslogt

[A]vst

For a first order reaction to obtain a positive slope, a graph is plotted between −loge​[A]vs.t.

$- l o g_{10} [A] v s t$

$- l o g_{e} [A] v s t$

$l o g_{10} [A] v s l o g t$

$[A] v s t$

For a first order reaction to obtain a positive slope, a graph is plotted between $- l o g_{e} [A] v s . t .$