let 4 moles of methanol (liquid) combust in 3 moles of gaseous oxygen to form gaseous carbon dioxide and water vapor. Suppose this occurs in a chamber of fixed volume and fixed temperature. If the original pressure is 1.0 atm, what is the final pressure in the chamber. Express your answer in atm. Enter a numerical value, do not enter units. Assume liquids take up negligible volume.

Question

Skylar Frey

Chemistry

11 June, 08:24

let 4 moles of methanol (liquid) combust in 3 moles of gaseous oxygen to form gaseous carbon dioxide and water vapor. Suppose this occurs in a chamber of fixed volume and fixed temperature. If the original pressure is 1.0 atm, what is the final pressure in the chamber. Express your answer in atm. Enter a numerical value, do not enter units. Assume liquids take up negligible volume.

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Answers (1)

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Lauren Powers · Answer 1

The final pressure is 2.0 atm

Explanation:

Step 1: Data given

Number of moles methanol = 4 mol

Number of moles oxygen = 3 mol

original pressure is 1.0 atm

Step 2: The balanced equation

2CH3OH (l) + 3O2 (g) → 2CO2 (g) + 4H2O (l)

Step 3: Calculate final pressure

For 2 moles of methanol consumed, we need 3 moles O2 to produce 2 moles CO2 and 4 moles H2O

We started with 3 moles of O2 gas.

Since methanol is not a gas, it doesn't count for the pressure.

V and T are fixed

This means the final pressure can be given by:

P2/P1 = n2/n1

with n2 = number moles of products

with n1 = number of moles of reactants

P2 = (6.0 mol*1.0 atm) / (3.0 mol)

P2 = Final pressure = 2.0 atm