For gaseous reactions, the rate is often expressed in terms of d P / dt instead of dC / dt or dn / d t (where C is concentration and n is the number of mole). What is the relation among these three expressions?

Question

For gaseous reactions, the rate is often expressed in terms of d P / dt instead of dC / dt or dn / d t (where C is concentration and n is the number of mole). What is the relation among these three expressions? (A) (d C/d t)=(1/V)((d n/d t))=(1/R T)((d P/d t)) (B) (d C/d t)=((d n/d t))=((d P/d t)) (C) (d C/d t)=((d n/d t))=(1/R T)((d P/d t)) (D) (d C/d t)=(V/R T)((d n/d t))

Tardigrade Admin · Accepted Answer

C=(n/V)=(P/R T) ∴ (d C/d t)=(1/V)((d n/d t))=(1/R T)((dP/d t))

Q. For gaseous reactions, the rate is often expressed in terms of $d P / d t$ instead of $d C / d t$ or $d n / d t$ (where $C$ is concentration and $n$ is the number of mole). What is the relation among these three expressions?

$\frac{d C}{d t} = \frac{1}{V} (\frac{d n}{d t}) = \frac{1}{RT} (\frac{d P}{d t})$

$\frac{d C}{d t} = (\frac{d n}{d t}) = (\frac{d P}{d t})$

$\frac{d C}{d t} = (\frac{d n}{d t}) = \frac{1}{RT} (\frac{d P}{d t})$

$\frac{d C}{d t} = \frac{V}{RT} (\frac{d n}{d t})$

$C = \frac{n}{V} = \frac{P}{RT}$

$∴ \frac{d C}{d t} = \frac{1}{V} (\frac{d n}{d t}) = \frac{1}{RT} (\frac{d P}{d t})$

Q. For gaseous reactions, the rate is often expressed in terms of dP/dt instead of dC/dt or dn/dt (where C is concentration and n is the number of mole). What is the relation among these three expressions?

dtdC​=V1​(dtdn​)=RT1​(dtdP​)

dtdC​=(dtdn​)=(dtdP​)

dtdC​=(dtdn​)=RT1​(dtdP​)

dtdC​=RTV​(dtdn​)