samanthaxwulff
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At 125 °C, 1 mol O₂ and 2 mol H₂ in a chamber have a total pressure of 3 atm. A current is run through the chamber, combining all the molecules into H₂O at constant volume. The pressure of the chamber, in atmospheres, is now:

Respuesta :

Answer:

1.9998 atm

Explanation:

Balance the equation and then use PV=nRT to find the variable.

onyebuchinnaji

The final pressure of the chamber is 2 atm.

The given parameters;

  • Temperature of the gas, T = 125 ⁰C
  • Number of oxygen moles = 1
  • Number of hydrogen moles, = 2
  • Initial pressure of the gases, P₁ = 3 atm

The balanced chemical reaction of the given elements;

[tex]O_2 \ \ + \ 2H_2 \ \ ---> \ 2H_2O[/tex]

Initial number of moles of the gases, = 1 + 2 = 3 moles

Final number of moles of the product, = 2  moles

The final pressure of the chamber is calculated as follows;

[tex]PV = nRT\\\\\frac{P}{n} = \frac{RT}{V} \\\\\frac{P_1}{n_1} = \frac{P_2}{n_2} \\\\P_2 = \frac{P_1 n_2}{n_1} \\\\P_2 = \frac{3 \times 2}{3} \\\\P_2 = 2 \ atm[/tex]

Thus, the final pressure of the chamber is 2 atm.

Learn more about ideal gas law here: https://brainly.com/question/12873752

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