at stp x ml n2 gas react completely with x ml o2 gas and form a gas a. what will be the molecular formula of a if volume is unchanged after reaction?
I think it's easier if we assign some number for x so let's use something easy like 200 ml
.........N2 + O2 ---> NyOz
I.......200.....200....0
C...-200....-200.....+ 400
E.....0...........0..........400
The problem tells us that we start off with a total volume of 400 and that the reaction is complete and that the initial volume = final volume.
Therefore, N2 + O2 ==> N2O2 but since the final volume must be twice N2 and twice O2 then N2 +O2 --> 2NO
NO is the molecular formula.
OR
....................N2 + O2 ==> NyOz
I....................x........x............0
C..................-x......-x............2x
E...........................................2x
so
.........................N2 + O2 ==> 2NO
Therefore, y and z must be 1 to make the equation balance.
To determine the molecular formula of the gas A formed in the reaction, we need to consider the stoichiometry of the reaction. The reaction equation you provided is:
N2 (g) + O2 (g) -> A (g)
Since the volume is unchanged after the reaction, it implies that the gases involved have a 1:1 ratio in terms of volume. This suggests that the coefficients in the balanced chemical equation will also be in a 1:1 ratio.
Therefore, for every x mL of N2 gas, we need x mL of O2 gas to react completely. This indicates that the reaction equation can be written as follows:
N2 (g) + O2 (g) -> A (g)
Since the volume of A is also x mL, it means that the mole ratio between N2 and A is also 1:1. Therefore, the molecular formula of the gas A will be the same as the formula for N2, which is N2.