Question

Calculate the average reaction rate of Cl2 consumed using the following information. H2 + Cl2 yields 2 HCl A table with three columns and 3 rows. The first column is titled Time. The second is titled the concentration of H subscript two (molar). The third column is titled the concentration of Cl subscript two (molar). The first row shows 0.00 under time, 0.0505 under H subscript two and 0.0875 under Cl subscript two. The second row shows 10.0 under Time, 0.0255 under H subscript two and 0.0625 under Cl subscript two. 6.81 × 10-1 mol/(L × s) 5.82 × 10-2 mol/(L × s) 7.50 × 10-2 mol/(L × s) 2.50 × 10-3 mol/(L × s)

Answer 1

Answer : Option D) 2.50 X $10^{-3}$ Mol/(L s)

Explanation: While calculating the average reaction rate for the given reaction in terms of Cl;

$H_{2} + Cl_{2} ----\ \textgreater \ 2HCl$.

using the rate equation which is;

$\frac{-1}{1}$$\frac{delta [Cl]}{delta t}$ = 

$\frac{- 0.0875 - 0.0625}{10s - 0s}$ = 2.50 X $10^{-3}$ Mol/(L s)