Calculate the average atomic mass of hydrogen using the following data:

45.4 L of dinitrogen reacted with 22.7 L of dioxygen and 45.4 L of nitrous oxide was formed. The reaction is given below:

2N₂(g) + O₂(g) → 2N₂O(g)

Which law is being obeyed in this experiment? Write the statement of the law?

If two elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element, are in whole number ratio

(a) Is this statement true?

(b) If yes, according to which law?

(c) Give one example related to this law.

Hydrogen gas is prepared in the laboratory by reacting dilute HCl with granulated zinc. Following reaction takes place.

Zn + 2HCl → ZnCl₂ + H₂

Calculate the volume of hydrogen gas liberated at STP when 32.65 g of zinc reacts with HCl. 1 mol of a gas occupies 22.7 L volume at STP; atomic mass of Zn = 65.3 u.

The density of 3 molal solution of NaOH is 1.110 g mL–1. Calculate the molarity of the solution.