A dull grey metallic looking substance which weighed 3.6 g was burned in air completely to produce 13.2 g of a gas with the following properties. It quinched a burning flame, and it was heavier than air g it would sink down to the bottom of a container it was also found that the same quantity of mass of oxygen (O2) Consumed by burning the 3.6 g of substance if combined with exactly 12 grams of hydrogen gas, produced 10.8g of water.

What was the mass(g) of molecular oxygen from the air that combined with the substance to produce the dense gas?

What is the ratio of the weight of oxygen burned to the weight of the dense gas produced?

Given the molecular mass of the water h2o is 18amu per molecule g or g mole what is the molecular mass of the dense gas?

What is the molar composition of the dense gas and it's chemical formula?

What is the element name and identity and atomic mass of the grey substance