If 2.0 moles of a gas (ideal behavior) at 25°C and 1.5 atm pressure react with excess oxygen, what will be the final pressure of the gas if the reaction produces two moles of a different gas and the volume remains constant?
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According to the ideal gas law, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
Since the volume remains constant, the equation can be simplified to P = nRT/V.
We want to find the final pressure, so we need to solve for P.
Let's assume that the initial pressure is given by P1 and the final pressure is given by P2.
We are given:
Initial moles of gas (n1) = 2.0 moles
Initial pressure (P1) = 1.5 atm
Final moles of gas (n2) = 2 moles
Since the volume remains constant, V1 = V2.
We have the equation for the initial pressure P1:
P1 = (n1 * R * T) / V
And the equation for the final pressure P2:
P2 = (n2 * R * T) / V
Since the temperature remains constant, the gas constant R remains constant as well.
We can solve for P2 by rearranging the equation:
P2 = (n2 / n1) * P1
Substituting the known values:
P2 = (2 moles / 2.0 moles) * 1.5 atm
P2 = 1.5 atm
Therefore, the final pressure of the gas is 1.5 atm.
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