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Byju's Answer

Standard XII

Chemistry

Compressibility Factor

For the ideal...

Question

For the ideal gaseous reaction, the rate is generally expressed in terms of $\frac{d P}{d t}$ instead of $\frac{d C}{d t}$ or $\frac{d n}{d t}$ (where $C = n / v$ is concentration and $n$ is the number of moles). What is the relation among these three expressions if $T$ and $V$ are constant?

\frac{d C}{d t} = \frac{d n}{d t} = \frac{d P}{d t}

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\frac{d C}{d t} = \frac{1}{V} \frac{d n}{d t} = \frac{1}{R T} (\frac{d P}{d T})

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R T \frac{d C}{d t} = \frac{d n}{d t} = \frac{d P}{d t}

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None of these

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Solution

The correct option is B $\frac{d C}{d t} = \frac{1}{V} \frac{d n}{d t} = \frac{1}{R T} (\frac{d P}{d T})$
$C = \frac{n}{V} = \frac{P}{R T} ∴ \frac{d C}{d t} = \frac{1}{V} \frac{d n}{d t} = \frac{1}{R T} (\frac{d P}{d t})$
Since $T$ and $V$ are constants.

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Similar questions

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

Q. For a gaseous reaction,

A (g) ⟶

Product, which one of the following is correct relation among

\frac{d P}{d t}, \frac{d n}{d t}

and

\frac{d c}{d t}

?
(

\frac{d P}{d t} =

Rate of reaction in

a t m

{s e c}^{- 1}

;

\frac{d c}{d t} =

Rate of reaction in molarity

{s e c}^{- 1}

;

\frac{d n}{d t} =

Rate of reaction in

m o l

{s e c}^{- 1}

)

Q. For a gaseous reaction, the rate is expressed interms of

\frac{d P}{d t}

in place of

\frac{d C}{d t}

\frac{d n}{d t}

, where

C

is concentration,

n

is number of moles and

^{'} P^{'}

ispressure of reactant. The three are related as:

Q. Which is correct relation in between

\frac{d c}{d t}, \frac{d n}{d t}

and

\frac{d P}{d t}

, where c, n, P, represents concentration, mole and pressure terms for gaseous phase reactant

A (g) \to p r o d u c t

Consider the chemical reaction,
$N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)$
The rate of this reaction can be expressed in terms of time derivatives of concentration of $N_{2} (g), H_{2} (g) o r N H_{3} (g)$ . Identify the correct relationship amongst the rate expressions.

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For the ideal gaseous reaction, the rate is generally expressed in terms of dPdt instead of dCdt or dndt (where C=n/v is concentration and n is the number of moles). What is the relation among these three expressions if T and V are constant?

The correct option is B dCdt=1Vdndt=1RT(dPdT)C=nV=PRT ∴dCdt=1Vdndt=1RT(dPdt) Since T and V are constants.

For the ideal gaseous reaction, the rate is generally expressed in terms of $\frac{d P}{d t}$ instead of $\frac{d C}{d t}$ or $\frac{d n}{d t}$ (where $C = n / v$ is concentration and $n$ is the number of moles). What is the relation among these three expressions if $T$ and $V$ are constant?

The correct option is B $\frac{d C}{d t} = \frac{1}{V} \frac{d n}{d t} = \frac{1}{R T} (\frac{d P}{d T})$
$C = \frac{n}{V} = \frac{P}{R T} ∴ \frac{d C}{d t} = \frac{1}{V} \frac{d n}{d t} = \frac{1}{R T} (\frac{d P}{d t})$
Since $T$ and $V$ are constants.