A mixture of gases containing equal weights of carbon dioxide, carbon monoxide, and ammonia exerts an overall pressure of 450.0 torr. What pressure is exerted by each gas individually??
To find the pressure exerted by each gas individually, we can use Dalton's Law of partial pressures. According to this law, the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the pressures exerted by each gas.
In this case, we have three gases with equal weights: carbon dioxide (CO2), carbon monoxide (CO), and ammonia (NH3).
Let's assume the pressure exerted by carbon dioxide is P(CO2), the pressure exerted by carbon monoxide is P(CO), and the pressure exerted by ammonia is P(NH3).
Since the weights of each gas are equal, the partial pressures of each gas will also be equal.
Therefore, we have the following equations:
P(CO2) = P(CO) = P(NH3)
The total pressure exerted by the mixture is given as 450.0 torr, so we can write:
P(CO2) + P(CO) + P(NH3) = 450.0 torr
Since all three partial pressures are equal, let's call it P:
P + P + P = 450.0 torr
3P = 450.0 torr
To find the value of P, we can divide both sides of the equation by 3:
P = 450.0 torr / 3
P ≈ 150.0 torr
So, the pressure exerted by each gas individually is approximately 150.0 torr.