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  • For the reaction: <img alt="\mathrm{2SO_{2}+O_{2}\rightarrow 2SO_{3}}" src="https://entrancecorner.oncodecogs.com/gif.latex?%5Cmathrm%7B2SO_%7B2%7D&plus;O_%7B2%7D%5Crightarrow%20

For the reaction:

\mathrm{2SO_{2}+O_{2}\rightarrow 2SO_{3}}
if the rate of disappearance of O2 is 8 g/sec,then rate of appearance  of SO3 (in g/sec)  will be:

Option: 1

40


Option: 2

4


Option: 3

16


Option: 4

10


Answers (1)

best_answer

For the reaction

\mathrm{2SO_2 + O_2 \longrightarrow 2SO_3}

Rate of reaction =

 \mathrm{Rate\ of \ Reaction = -\frac{1}{2}\frac{\mathrm{d} \left [ SO_{2} \right ]}{\mathrm{d} t}=-\frac{\mathrm{d} \left [ O_{2} \right ]}{\mathrm{d} t}=\frac{1}{2}\frac{\mathrm{d} \left [ SO_{3} \right ]}{\mathrm{d} t}}

\mathrm { Given, \frac{ d \left[ O _{2}\right]}{ d t}=8\ \frac{g}{sec}=\frac{1}{4} \frac{mol}{sec}}

\\\mathrm{Now, \frac{\mathrm{d} \left [ O_{2} \right ]}{\mathrm{d} t}=\frac{1}{2}\frac{\mathrm{d} \left [ SO_{3} \right ]}{\mathrm{d} t}}\\\\ \mathrm{So, \ \frac{\mathrm{d} \left [ SO_{3} \right ]}{\mathrm{d} t}=2\times\frac{\mathrm{d} \left [ O_{2} \right ]}{\mathrm{d} t}}

\mathrm{ Hence, \frac{ d \left[S O_{3}\right]}{ d t}=\left( 2 \times \frac{1}{4}\right ) \frac{mol}{sec}= 40\ \frac{g}{sec}}
 

 

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