Question

20% of N₂O₄ molecules are dissociated into NO₂ in a sample of gas at 300k and 760 Torr. Calculate the density of the equilibrium mixture

1) ABO₂
2) A₂BO₂
3) A₂B₃O₄
4)AB₂O₂

Answer 1

To calculate the density of the equilibrium mixture for each compound, we need to know the number of moles and the molar mass of each compound.

Step-by-step explanation:

To calculate the density of the equilibrium mixture for each compound, we need to know the number of moles and the molar mass of each compound.

1) ABO₂: Since there is no dissociation, the density can be calculated using the ideal gas law, PV = nRT. We can rearrange the equation to solve for the density (d = m/V) and use the given information to calculate the density.

2) A₂BO₂: Again, there is no dissociation, so we can use the ideal gas law to calculate the density of A₂BO₂ by rearranging the equation.

3) A₂B₃O₄: Since 20% of N₂O₄ molecules dissociate, we need to consider the density of both N₂O₄ and the dissociated molecules (2 NO₂). We can use the mole ratios from the balanced chemical equation to calculate the number of moles and then use the molar mass to calculate the density of the equilibrium mixture.

4) AB₂O₂: Since 20% of N₂O₄ molecules dissociate, we need to consider the density of both N₂O₄ and the dissociated molecules (2 NO₂). We can use the mole ratios from the balanced chemical equation to calculate the number of moles and then use the molar mass to calculate the density of the equilibrium mixture.