The apparatus in which standard solution is prepared is known as :

According to the Haber-Bosch process, the molar ratio of hydrogen to ammonia is:

What is the mass of 0.2 moles of oxygen atoms?

1 mol of $C{H_4}$ contains

Two elements, R and S, combine to form $RS_2$ and $R_2S_3$. If 10 g of $RS_2$ contains 0.1 mole and 9 g of $R_2S_3$ contains 0.05 mole, find the atomic weights of R and S.

The total number of electrons in 18 ml of water (density = 1/gml

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:

A 0.50 $M$ solution of $KI$ reacts with excess of ${{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}$ and ${\rm{KI}}{{\rm{O}}_3}$ solutions according to the equation, $6{{\rm{H}}^ + } + 5{{\rm{I}}^ - } + {\rm{IO}}_3^ - o 3{{\rm{I}}_2} + 3{{\rm{H}}_2}{\rm{O}}$. Which of the following statements is true?

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

A compound contains 28% nitrogen and 72% of a metal by weight. Three atoms of metal combine with two atoms of nitrogen. If the atomic weight of nitrogen is 14, the atomic weight of the metal is:

If Avogadro's number were $6.022 imes 10^{15} \, mol^{-1}$, what would be the mass of one mole of water (H$_2$O)? (Atomic masses: H = 1 u, O = 16 u)