PLEASE HELP! According to the equation, how many liters of oxygen gas at STP are produced when 2.00 moles of potassium chlorate decomposes? a. 134 L

b. 67.2 L

c. 22.4 L

d. 11.2 L

PLEASE HELP! According to the equation, how many liters of oxygen gas at STP are produced when 2.00

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Ответ:

Karamatullah

24.12.2020

Chemistry

Answer : The concentration of H_3O^+ at equilibrium is, 0.015 M

Solution :

The balanced equilibrium reaction will be,

$HA+H_2O\rightleftharpoons H_3O^++A^-$

The expression for dissociation constant of weak aciod will be,

$k_a=\frac{[H_3O^+]\times [A^-]}{[HA]}$

where,

k_a = dissociation constant of weak acid

Let the concentration of H_3O^+ and A^- be 'x'

Now put all the given values in this expression, we get

$4.6\times 10^{-4}=\frac{(x)\times (x)}{0.50}$

x=0.015M

The concentration of H_3O^+ = A^- = x = 0.015 M

Therefore, the concentration of H_3O^+ at equilibrium is, 0.015 M

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PLEASE HELP! According to the equation, how many liters of oxygen gas at STP are produced when 2.00 moles of potassium chlorate decomposes? a. 134 Lb. 67.2 Lc. 22.4 Ld. 11.2 L