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 $2.3$ g formic acid and $4.5$ g oxalic acid is treated with conc. $H_2SO_4$. The evolved gaseous mixture is passed through $KOH$ pellets. The weight (in g) of the remaining product at STP will be

A mixture of $CO_2$ and $N_2$ gases contains 0.44 g of $CO_2$ and 0.56 g of $N_2$. The total number of moles of gases in the mixture is:

If you have 8g of He, 4g of $H_2$, and 32g of $O_2$, which sample has the highest number of molecules?

Upon treating a mixture of $0.46$ g of formic acid and $0.9$ g of oxalic acid with concentrated $H_2SO_4$, a gaseous mixture is evolved. This mixture is then passed through pellets of $KOH$. Determine the mass (in g) of the remaining product at STP.

Which of the following contains the greatest number of helium atoms?

Which has more molecules: 1 mole of glucose or 18 grams of water?

How many moles are present in 18g of water (H2O)?

Calculate the mass (in g) of the gaseous product remaining at STP when a mixture of $9.2$ g formic acid and $18$ g oxalic acid is treated with conc. $H_2SO_4$ and then passed through $KOH$ pellets.

Which of the following has the largest number of atoms?

One mole of $\;{\rm{C}}{{\rm{O}}_2}$ contains: