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  • Consider the reaction: 2X 4Y + Z In the reaction Y is being formed at the rate of <i

Consider the reaction:
2X \rightarrow 4Y + Z
In the reaction Y is being formed at the rate of 0.05 \mathrm{molL}^{-1} \mathrm{~s}^{-1}. Calculate overall rate of reaction.

Option: 1

0.0125 \mathrm{molL}^{-1} \mathrm{~s}^{-1}


Option: 2

0.1 \mathrm{molL}^{-1} \mathrm{~s}^{-1}


Option: 3

0.05 \mathrm{molL}^{-1} \mathrm{~s}^{-1}


Option: 4

0.025 \mathrm{molL}^{-1} \mathrm{~s}^{-1}


Answers (1)

best_answer

For a given reaction, if:
aA + bB \rightarrow cC + dD


Overall rate r can be expressed as:
\mathrm{ r=\frac{-1}{a} \times \frac{d[A]}{d t}=\frac{-1}{b} \times \frac{d[B]}{d t}=\frac{+1}{c} \times \frac{d[C]}{d t}=\frac{+1 d[D]}{d d t} }

where:
\mathrm{ -\frac{d[A]}{d t}= \\ }  Rate of disappearance of A.
\mathrm{ -\frac{d[B]}{d t}= }  Rate of disappearance of B.

\mathrm{ +\frac{d[C]}{d t}= }  Rate of Formation of C.

\mathrm{ +\frac{d[D]}{d t}= }  Rate of Formation of D.

Given:
2X \rightarrow 4Y + Z 
\mathrm{ +\frac{d[Y]}{d t}=\text { Rate of formation of } Y=0.05 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}}

Overall rate (r) =\mathrm{ \frac{1}{4} \times} Rate of formation of Y
\mathrm{ r=\frac{1}{4} \times 0.05=0.0125 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} }

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