We are asked to write the rate law expression for the given reaction.
To do so, we shall follow these steps:
Step 1: Find the remaining pressure of oxalic acid.
Step 2: Use the integrated rate law equation for the first-order and check for the consistent value of K.
At 400 K oxalic acid decomposes according to the reaction: H2C2O4(g) → CO2(g) + HCOOH(g). In three separate experiments, the initial pressure of oxalic acid and final total pressure after 20,000 s is measured.
|P H2C2O4 at t = 0||65.8||92.1||111|
|PTotal at t = 20,000 s||93.6||131||158|
Find the rate law of the reaction.
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