Oxygen and carbon dioxide are found under the same conditions and at the same temperature.

Oxygen and carbon dioxide are found under the same conditions and at the same temperature. Are the pressures of these gases the same?

For gas, the ideal gas equation is valid: P * V = m * R * T / M, where P is the gas pressure, V is the gas volume, m is the gas mass, R is the universal gas constant, T is the absolute temperature, M is the molar mass …
P = m * R * T / M * V.
Since the conditions are the same, the values of m, R, T, V will be the same for two gases. Only the molar mass will be different.
M (O2) = 16 * 2 = 32 g / mol is the molar mass of oxygen.
M (CO2) = 12 + 16 * 2 = 44 g / mol is the molar mass of carbon dioxide.
Therefore, the oxygen pressure will be greater than the carbon dioxide pressure under the same conditions.