NEET Chemistry MCQs

Equal masses of oxygen and ozone are present in a container at 298 K. The ratio of their partial pressures ($P_{O_2} : P_{O_3}$) is:

A mixture of 1 mol of He and 0.5 mol of SO2 is held in a container at a constant temperature of 27°C. The partial pressure of He is 2 atm. If the mixture behaves ideally, what is the density of the mixture (g/L) closest to? (Given: R = 0.082 L atm/mol K, Molar mass of He = 4 g/mol, Molar mass of SO2 = 64 g/mol)

Calculate the total pressure (in atm) exerted by a mixture of 8 g of $O_2$ and 4 g of $H_2$ confined in a 2-litre vessel at $0^0C$. (Given $R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1}$)

A container of volume 500 mL holds a mixture of 2 g of $O_2$ and 1 g of $H_2$ at $27^0C$. What is the total pressure (in atm) inside the container? (Use $R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1}$)

If 16 g of $O_2$ and 8 g of $H_2$ are present in a 4-litre container at $0^0C$, determine the total pressure (in atm) exerted by the gas mixture. (Given $R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1}$)

A mixture of 0.5 moles of $O_2$ and 1 mole of $H_2$ is contained in a 1-litre flask at 273 K. Calculate the total pressure (in atm) inside the flask. (Given $R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1}$)

Two gases, $O_2$ (1 mole) and $H_2$ (0.5 moles), are mixed in a 2-litre vessel at a temperature of 273 K. Using the ideal gas constant $R = 0.082 \, L \, atm \, mol^{-1} \, K^{-1}$, find the total pressure (in atm) exerted by the mixture.

Which of the following equations does NOT correctly represent Dalton's Law of Partial Pressures for a mixture of three gases A, B, and C, where $p$ is the total pressure?

A mixture of nitrogen and oxygen gases exerts a total pressure of 1.2 atm. If the partial pressure of nitrogen is 0.8 atm, what is the partial pressure of oxygen according to Dalton's Law?

If the partial pressures of gases in a mixture are 20 kPa, 30 kPa, and 50 kPa, what is the total pressure exerted by the mixture according to Dalton's Law?