Consider the decomposition of N 2 O 5 as shown in the following equation to answer the next three questions:
2 N 2 O 5 (g) → 4 NO 2 (g) + O 2 (g)
1. If the rate of decomposition of N 2 O 5 at a particular instant in a reaction vessel is 4.2 x 10 -7 M/s, what is the rate of appearance of NO 2 and O 2 respectively?
2. The reaction shown above has been determined to be first order with respect to N 2 O 5 . If 0.0250 moles of N 2 O 5 are charged into a 2.00 L vessel, how many moles will remain after 150 seconds if the rate constant is 6.82 x 10 -3 s -1 (at 70 o C)?
3. What is the half-life for this reaction at 70 o C?
