N O_{2} required for a reaction is produced by the decomposition of N_{2} O_{5} in C C l_{4} as per the equation 2 N_{2} O_{5}(g)\to 4 N O_{2}(g)+O_{2}(g) The initial concentration of N_{2} O_{5} is 3.00 mol L^{-1} and it is 2.75 mol L^{-1} after 30 minutes the rate of formation of N O_{2} is [12 Apr 2019 Shift 2]

Correct Answer is : 1.667×10−3molL−1min−1

2.083 \times 10^{-3} \mol \L^{-1} \min^{-1}

8.333 \times 10^{-3} \mol \L^{-1} \min^{-1}

4.167 \times 10^{-3} \mol \L^{-1} \min^{-1}

1.667 \times 10^{-3} \mol \L^{-1} \min^{-1}

Chemical Kinetics Part 1

Section: Chemistry

Question : 37 of 100

Marks: +1, -0

NO2 required for a reaction is produced by the decomposition of N2O5 in CCl4 as per the equation 2N2O5(g)→4NO2(g)+O2(g) The initial concentration of N2O5 is 3.00 mol L−1 and it is 2.75 mol L−1 after 30 minutes the rate of formation of NO2 is

[12 Apr 2019 Shift 2]

2.083×10−3‌mol‌L−1‌min−1
8.333×10−3‌mol‌L−1‌min−1
4.167×10−3‌mol‌L−1‌min−1
1.667×10−3‌mol‌L−1‌min−1

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