A mixture of 90.0 grams of CH4 and 10.0 grams of argon has a pressure of 250 torr under conditions of constant temperature and volume. The partial pressure of CH4 in tore is?

the partial pressure of methane CH₄ is 239.4 torr.

Explanation:

Given;

molar mass of methane, CH₄ = 90.0 g

molar mass of argon, Ar = 10.0 g

total pressure of the gases, Pt = 250 torr

number of moles of methane CH₄;

number of moles of Ar;

The mole fraction of methane XCH₄ is calculated as;

Apply Dalton's law of partial pressure, to determine the partial pressure of methane CH₄;

Therefore, the partial pressure of methane CH₄ is 239.4 torr.

b. examine and describe cells

answer seismograph;