Estimate the molar volume of CO2 at 500 K and 100 atm by treating it as a van der Waals gas? a = 3.610 dmoatmm

A breathing mixture used by deep-sea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at a barometric pressure of 101.4 kPa, if PHe  = 82.5 kPa and  PCO2  = 0.4 kPa?

In a container of 80 I at 50 ° C under vacuum, 7 g of N2, 16 g of O2 and 3.03 g of H2 are introduced. Calculate the partial pressure of each gas, the total pressure, and the composition of the mixture in mole percent.

When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete - the lime absorbs CO₂ from the air and turns back into hard, durable limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 550. L and heated to 520.0 °C. When the amount of CaCO3 has stopped changing, it is found that 8.46 kg have disappeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 520.0 °C. Round your answer to 2 significant digits. P Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K does not match the accepted value. 0 X

Calculate the pressure, in atmospheres, of 2.40 molesmoles of helium gas in a 10.0-LL container at 21 ∘C∘C. Express your answer with the appropriate units.

Describe what happens to the average kinetic energy of ideal gas molecules when the conditions are changed as follows:(a) The pressure of the gas is increased by reducing the volume at constant temperature.(b) The pressure of the gas is increased by increasing the temperature at constant volume.(c) The average velocity of the molecules is increased by a factor of 2.

When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete the lime absorbs CO₂ from the air and turns back into hard, durable 2 limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 400. L and heated to 740.0 °C. When the amount of CaCO3 has stopped changing, it is found that 3.37 kg have disappeared. P 00. Calculate the pressure equilibrium constant K this experiment suggests for the equilibrium between CaCO3 and CaO at 740.0 °C. Round your answer to 2 significant digits. Ar Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K does not match the accepted value. р K₁ = 0 x10 р x Ś ? Explanation Check 0 81 K © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility