4 NH3 (g) + 5 O2 (g) = 4 NO (g) + 6 H2O (g)A sample of NH3 is added to an initially evacuated 2.00 L flask at 125 C, until the pressure if 415 torr. O2 is then added to the flask until the total initial pressure ( before reaction) is 875 torr. Assuming the reaction goes to completion, find the partial pressure of all gases in the mixture, after the reaction is complete.

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Asked Nov 15, 2019
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4 NH3 (g) + 5 O2 (g) = 4 NO (g) + 6 H2O (g)
A sample of NH3 is added to an initially evacuated 2.00 L flask at 125 C, until the pressure if 415 torr. O2 is then added to the flask until the total initial pressure ( before reaction) is 875 torr. Assuming the reaction goes to completion, find the partial pressure of all gases in the mixture, after the reaction is complete.

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Expert Answer

Step 1

Given that,

Partial pressure of NH3= 415torr

Partial pressure of O2 = (875-415) torr

                                   = 460 torr

Step 2

The given reaction is

4 NO 6H20
4NH3502
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4 NO 6H20 4NH3502

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Step 3

As per the reaction

4 moles of NH3 reacts with 5 moles of O2

B...

P(O2)
= 1.1
P(NH)
according to the reaction the mole ratio is
mole(02)
mole(NH
5
4
1.25
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P(O2) = 1.1 P(NH) according to the reaction the mole ratio is mole(02) mole(NH 5 4 1.25

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