Question

a compound x of a metal reacts with dilute hydrochloric acid a gas comes out with effervescence and it is extinguishes a burning candle it also turns lime water milky identify the gas evolved when excess of this gas is passed into lime water the milkiness disappears explain the observation and give equation involved

Please tell the right answer. ​

Answer 1

Answer:

The gas thus formed is an effervescent carbon dioxide gas when calcium carbonate reacts with hydrochloric acid. The carbon dioxide gas also acts as an extinguisher for fires. Hence, the burning candle is extinguished. The metal compound A, therefore, constitutes calcium carbonate.

Hence metal compound A is CaCO3

The Gas evolved is CO2

Answer 2

Explanation:

When a metal compound A on reacting with hydrochloric acid shows effervescence which shows the evolution of carbon dioxide gas and it is confirmed by putting off the candle flame.

So metal compound A is a carbonate of calcium which on reacting with HCl gives calcium chloride and carbon dioxide as gas along with water.

CaCO

3

(s) + 2HCl(aq) → CaCl

2

(s) + CO

2

(g) + H

2

O(l)