For the reaction 2 {\N}_2 {\O}_5( {\g}) \to 4 {\NO}_2( {\g})+ {\O}_2( {\g}) \text{, } the rate of formation of {\NO}_2( {\g}) is 2.8 \times 10^{-3} {\M} { s}^{-1}. Calculate the rate of disappearance of {\N}_2 {\O}_5( {\g})

CBSE Class 12 Chemistry 2018 Solved Paper - Question 7

Question : 7 of 26

Marks: +1, -0

For the reaction

2 {\N}_2 {\O}_5( {\g}) → 4 {\NO}_2( {\g})+ {\O}_2( {\g}) \;\text ", "\;

the rate of formation of

{\NO}_2( {\g})

2.8 × 10^{-3} {\M} {\ s}^{-1}

.
Calculate the rate of disappearance of

{\N}_2 {\O}_5( {\g})

Solution:

\;\text " Rate "\;\;=\;{1}/{4} \;{∆ N {\O}_2}/{∆(t)}=\;{1}/{2} \;{∆ ( {\N}_2 {\O}_5) }/{∆(t)}

\;{1}/{4} (2.8 × 10^{-3}) \;=-\;{1}/{2} \;{∆ ( {\N}_2 {\O}_5) }/{∆(t)}

Rate of disappearance of

{\N}_2 {\O}_5

(-\;{∆ N_2 O_5}/{∆(t)}) 1.4 × 10^{-3} {\M} \/ {\ s}

(Deduct half mark if unit is wrong or not written)

Go to Question:

Prev Question

Next Question