The total pressure of a container that has $N H_{3} (g)$ $NH_3(g)$ exerting a pressure of 346 torr, $N_{2} (g)$ $N_2(g)$ exerting a pressure of 225 torr, and $H_{2} O (g)$ $H_2O (g)$ exerting a pressure of 55 torr?

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The total pressure of a container that has $N H_{3} (g)$ $NH_3(g)$ exerting a pressure of 346 torr, $N_{2} (g)$ $N_2(g)$ exerting a pressure of 225 torr, and $H_{2} O (g)$ $H_2O (g)$ exerting a pressure of 55 torr?

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Answer 1 · 2017-04-20T14:40:30

This is simply the sum of the individual partial pressures...........

Explanation:

And thus.......................

$P_{total} = P_{ammonia} + P_{dinitrogen} + P_{water vapour}$ $P_"total"=P_"ammonia"+P_"dinitrogen"+P_"water vapour"$

$= (346 + 225 + 55)$ $=(346+225+55)$ $m m \cdot H g$ $mm*Hg$ $= 626 \cdot Torr$ $=626*"Torr"$ .

How many atmospheres is this?

Can you think of a way to estimate the temperature at which this experiment was performed? I can think of [one.](https://en.wikipedia.org/wiki/Vapour_pressure_of_water)

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The total pressure of a container that has $N H_{3} (g)$ $NH_3(g)$ exerting a pressure of 346 torr, $N_{2} (g)$ $N_2(g)$ exerting a pressure of 225 torr, and $H_{2} O (g)$ $H_2O (g)$ exerting a pressure of 55 torr?

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The total pressure of a container that has NH3(g)NH_3(g) exerting a pressure of 346 torr, N2(g)N_2(g) exerting a pressure of 225 torr, and H2O(g)H_2O (g) exerting a pressure of 55 torr?

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The total pressure of a container that has $N H_{3} (g)$ $NH_3(g)$ exerting a pressure of 346 torr, $N_{2} (g)$ $N_2(g)$ exerting a pressure of 225 torr, and $H_{2} O (g)$ $H_2O (g)$ exerting a pressure of 55 torr?