A) Write an equation to relate the rate of consumption of hydrogen to the rate of formation of hydrogen chloride.

Question

Hydrogen reacts with chloride according to the following balanced equation: H₂ +Cl₂→2HCl.

B) Suppose the rate of consumption of hydrogen in this reaction is 5.9x10⁴ M/s. Calculate the corresponding rate of formation of hydrogen chloride.

Answer 1

A) -∆[H₂]/∆t = +1/2∆[HCl]/∆t

B) 9.5x10⁴ M/s = 1/2 x

x = 1.9x10⁵ M/s

Answer 2

Based on the balanced chemical equation, when one mole of hydrogen is consumed, two moles of hydrogen chloride is formed. Therefore to relate the rate of consumption of H₂ and the rate of formation of HCl, we have

-2d[H₂]/dt = d[HCl]/dt. The rate of H₂ is negative since it's being consumed and changed into HCl.

Lastly, substitute the rate of consumption for hydrogen (5.9 x 10⁴ M/s) into the equation