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andrezito [222]
2 years ago
8

The O2 produced from the decomposition of the 1.0 L sample of H2O2 is collected in a previously evacuated 10.0 L flask at 300. K

What is the approximate pressure in the flask after 400 s
Chemistry
1 answer:
Sergio [31]2 years ago
7 0

The full question can be seen below:

2H_{2}O_2_{(aq)} --> 2H_{2}O_{(l)}+O_{2}_{g}

The decomposition of H_{2}O_{aq} is represented by the equation above.

A student monitored the decomposition of a 1.0 L sample of H_{2}O_2_(_{aq}_) at a constant temperature of 300K and recorded the concentration of H_{2}O_2 as function of time. The results are given in the table below:

                                    Time (s)      H_{2}O_2

                                    0                 2.7

                                    200            2.1

                                    400            1.7

                                    600            1.4

The O_2_(_{g}_) produced from the decomposition of the 1.0 L sample of H_{2}O_2_(_{aq}_) is collected in a previously evacuated 10.0 L flask at 300 K. What is the approximate pressure in the flask after 400 s?

(For estimation purpose, assume that 1.0 mole of gas in 1.0 L exerts a pressure of 24 atm at 300 K).

Answer:

1.2 atm

Explanation:

Considering all assumptions as stated above;

                       2H_{2}O_2_{(aq)} --> 2H_{2}O_{(l)}+O_{2}_{g}

Initial               2.7 mole               ---             ---

Change          -1.0                        ---             +\frac{1.0}{2}

Equilibrium     1.7 mole                ---             0.5 mole

To determine the concentration of O₂; we need to convert the moles to concentration for O₂ = \frac{0.5}{volume in the flask}

                                  = \frac{0.5 mol}{10.0 L}

                                  = 0.05 \frac{mol}{L}

Thus, based on the assumption that "1.0 mole of gas in 1.0 L exerts a pressure of 24 atm"

∴ 0.05\frac{mol}{L} will give rise to = 0.05 \frac{mol}{L} × 24

                                           = 1.2 atm

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