Question

PLEASE VERY URGENTTT WILL GIVE MEDAALSS !!

0.144gg of an aluminum compound X react with an excess of water, to produce a gas. This gas burns completely in O2 to form H2O and 72cm^3 of CO2 only. The volume of CO2 was measured at room temperature and pressure,

What could be the forumula of X?
(C=12.0, Al=27.0 ; 1 mole of any gas occupies 24 dm^3 at room temperature and pressure.

???

Answer 1

Well first you need to write out a balanced chemical reactions.

This question is describing two chemical reactions

You also know that you produced,

72cm^3 of CO2 in the second reaction, and that 1 mole of any gas occupies 24 cm^3, so you can find the amount of moles of CO2 produced in the second reaction.

You should then be able to work backwards to find the moles of the almunium product reacted.

Use the formula,

Moles = Grams/molecular mass
or
n*Moles = n*Grams/molecular mass

where n is some integer (because you cannot balance the first reaction because you dont really know what X is), although assume it is a 1 to 1 reaction first so set n=1

to find molecular mass of the Aluminum compound from that you should be able to deduce the identity of X (the aluminum compound) reacted in the first reaction.

q

Answer 2

I'm pretty sure I know what the answer is without even doing the math lol

Answer 3

If you have any questions on solving this problem please feel free to ask

Answer 4

@Australopithecus can you do it step wise please, i cant really follow what you posted above. I will appreciate it :)