For a gaseous reaction, the rate is expressed in terms of (d P/d t) in place of (d C/d t) or (d n/d t) , where C is concentration, n is number of moles and â²Pâ² is pressure of reactant. The three are related as -

Question

For a gaseous reaction, the rate is expressed in terms of (d P/d t) in place of (d C/d t) or (d n/d t) , where C is concentration, n is number of moles and â²Pâ² is pressure of reactant. The three are related as - (A) [(d P/d t)]=(R T/V)[(d n/d t)]=[(d C/d t)] (B) (1/R T)[(d P/d t)]=(1/V)[(d n/d t)]=[(d C/d t)] (C) [(d P/d t)]=[(d n/d t)]=[(d C/d t)] (D) None of these

Tardigrade Admin · Accepted Answer

Rate=(d C/d t) C=(n/V) and C=(P/R T) (d C/d t)=(d/d t)((n/V))=(1/V)× ((d n/d t)) (d/d t)((P/R T))=(1/R T)× ((d P/d t))

Q. For a gaseous reaction, the rate is expressed in terms of $\frac{d P}{d t}$ in place of $\frac{d C}{d t}$ or $\frac{d n}{d t}$ , where $C$ is concentration, $n$ is number of moles and $' P'$ is pressure of reactant. The three are related as -

$[\frac{d P}{d t}] = \frac{RT}{V} [\frac{d n}{d t}] = [\frac{d C}{d t}]$

$\frac{1}{RT} [\frac{d P}{d t}] = \frac{1}{V} [\frac{d n}{d t}] = [\frac{d C}{d t}]$

$[\frac{d P}{d t}] = [\frac{d n}{d t}] = [\frac{d C}{d t}]$

None of these

$R a t e = \frac{d C}{d t}$

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

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

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

Q. For a gaseous reaction, the rate is expressed in terms of dtdP​ in place of dtdC​ or dtdn​ , where C is concentration, n is number of moles and ′P′ is pressure of reactant. The three are related as -

[dtdP​]=VRT​[dtdn​]=[dtdC​]

RT1​[dtdP​]=V1​[dtdn​]=[dtdC​]

[dtdP​]=[dtdn​]=[dtdC​]