Question

Can someone walk me through step by step with this question:

A rigid vessel at constant temperature initially contains 0.600 atm nitrogen gas and 0.600 atm hydrogen gas. If these gases react to form ammonia and the reaction goes to completion, which choice is closest to the final total pressure after the reaction?

Answer 1

What are the choices?

Answer 2

0.800 atm, 0.167 atm, 0.950 atm, 1.52 atm

Answer 3

First write the chemical reaction:

N2 + 3H2 --> 2NH3
nitrogen gas hydrogen gas ammonia

The total pressure = the sum of the partial pressures of gases in the system (the rigid vessel). This is because matter is neither created nor destroyed.

0.60atm + 0.60atm = 1.2atm

Answer 4

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Answer 5

If partial pressure of N2 and H2 are the same, you will have the same number of moles of each. Based on N2 + 3H2 ---> 2NH3 you will have more N2 that can react. All H2 will react so its partial pressure at the end = 0 atm. Only 1/3 of N2 can react so 2/3 of N2 will be left at the end. This will have a partial pressure of 0.4atm. If each mole N2 makes 2 moles NH3, based on a partial pressure of N2 reacting of 1/3 atm. the partial pressure of NH3 made will be 2/3 atm. Total pressure at end will be 2/3 atm for N2 and 2/3 atm for NH3 making 1 1/3 atm. total pressure. Starting total pressure was 1.2 atm.

Answer 6

Does this make sense? I believe the answer is 0.8atm