Volume of a gaseous hydrocarbon is 1.12 L at STP. When it is completely burnt in air, 2.2g of `CO_(2)` & 1.8g of water are formed. Find the volume of oxygen required at STP and also mass of the compound taken. Give the molecular formula of hydrocarbon.

A sample of gaseous hydrocarbon occupying 1.12 litre at NTP, when completely burnt in air produced 2.2 g CO_2 and 1.8 g H_2O Calculated the weight of hydrocarbon taken and the volume of O_2 at NTP required for its combustion.

What is the volume of 11g of CO_(2) at STP?

An oil of relative density 1.2 and volume 1 litre is poured in water find the mass of the oil

10 mL of a gaseous hydrocarbon is completely combusted with 60 mL of oxygen by passing electric spark. The volume of the gaseous mixture thus yielded on cooling becomes 46 mL, iff the vapour density of the compound is 15, what will be its molecular formula? [All volumes were measured under the same conditions of temperature and pressure.]

Volume of 4.4 g of CO_2 at STP is-

Volume of CO_2 produced at STP from 1 mole of calcium carbonate is-

A gaseous hydrocarbon gives upon combustion 0.72g water and 3.08g CO_(2) . The empirical formula of the hydrocarbon-

The volume of CO_2 at STP from the combustion of 12 g carbon will be-

An organic compound contains C, H and O as its constituents. On heating in absence of air, 3.10g of this compound, produces 1.24g of carbon. But if 0.5 g of the compound is burnt in presence of air, 0.3 g of H_(2)O is formed. 0.05 gram-mole of the compound contains 4.8g of oxygen. what is the molecular formula off the compound?