# Question c5cb2

Apr 16, 2017

By the problem the following gaseous reaction is occuring in closed, rigid vessel at constant temperature.

$W \left(g\right) + X \left(g\right) \to Y \left(g\right) + Z \left(g\right)$

The stoichiometric ratio of number of moles of reactants and prducts is

$W \left(g\right) : X \left(g\right) : Y \left(g\right) : Z \left(g\right) = 1 : 1 : 1 : 1$

The volume and temperature remaining constant the partial pressures of the component gases are proportional to their number of moles.

The initial partial pressures of $W \left(g\right) \mathmr{and} X \left(g\right)$ are 1.2 atm and 1.6 atm respectively.
And the initial partial pressures of $Y \left(g\right) \mathmr{and} Z \left(g\right)$ are 0 atm.

If the partial pressure of $W \left(g\right)$ is decreased to 1atm then the 0.2atm decrease is due to its taking part in the reaction.
So the decrease in pressure of $X \left(g\right)$ will also be 0.2 atm.

But pressures of each of Y(g) and Z(g) # will be inreased to 0.2atm as the interacting mole ratio is $1 : 1 : 1 : 1$