10 moles SO₂ and 15 moles O₂ were allowed to react over a suitable catalyst. 8 moles of SO₃ were formed. The remaining moles of SO₂ and O₂ respectively are -

The hydrated salt Na₂CO₃. x H₂O undergoes 63% loss in mass on heating and becomes anhydrous. The value of x is

How many gram of sulphur can be obtained by the reaction of 1 mole of SO₂ with 22.4 L of H₂S at STP?

12 L of H₂ and 11.2 L of Cl₂ are mixed and exploded. Find the composition by volume of mixture.

10 g of hydrogen and 64 g of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be:

A metal oxide has the formula Z₂O₃. It can be reduced by hydrogen to give free metal and water. 0.1596 g of the metal oxide requires 6 mg of hydrogen for complete reduction. The atomic weight of the metal is

The empirical formula of an acid is CH₂O₂, the probable molecular formula of acid may be:

The volume of chlorine at STP required to liberate all the bromine and iodine in 100 ml of 0.1 M each of KI and MBr₂ will be:

How many moles of KI are required to produce 0.4 moles of K₂HgI₄ ?

If 0.5 mol of BaCl₂ is mixed with 0.2 mole of Na₃PO₄, find the maximum amount of Ba₃(PO₄)₂ that can be formed.