In a first-order decomposition reaction. 20.8% of a compound decomposes in 7.8 min. how long (in min) does it take for 88.2% of the compound to decompose?

t = 71.47 min

Explanation:

Using integrated rate law for first order kinetics as:

Where,  

is the concentration at time t

is the initial concentration

Given:

20.8 % is decomposed which means that 0.208 of is decomposed. So,

= 1 - 0.208 = 0.792

t = 7.8 min

k = 0.0299 min⁻¹

Also,

Given:

88.2 % is decomposed which means that 0.882 of is decomposed. So,

= 1 - 0.882 = 0.118

t = ?

t = 71.47 min

56 moles of   lieter in chemistry

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