Question

4.0 L of He(g), 6.0 L of N2(g), and 10. L of Ar(g), all at 0°C and 1.0 atm, are pumped into an evacuated 8.0 L rigid container, the final pressure in the container at 0°C is _____

A) 4 atm
B) 7 atm
C) 9 atm
D) 3 atm

Answer 1

The final pressure in the container at 0°C can be found using the ideal gas law equation, PV = nRT. By calculating the number of moles for each gas and summing them, you can then determine the final pressure. In this case, the final pressure is 8 atm.

Step-by-step explanation:

To find the final pressure in the container, we can use the ideal gas law equation: PV = nRT. Here, 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 container is rigid, the volume remains constant at 8.0 L.

We can find the number of moles for each gas using the equation n = PV/RT. Plugging in the values for He(g): nHe = (1.0 atm * 4.0 L) / (0.0821 * 273 K) = 0.073 moles. Similarly, for N2(g): nN2 = (1.0 atm * 6.0 L) / (0.0821 * 273 K) = 0.11 moles. And for Ar(g): nAr = (1.0 atm * 10.0 L) / (0.0821 * 273 K) = 0.183 moles.

Now, we can calculate the total moles of gas in the container: nTotal = nHe + nN2 + nAr = 0.073 + 0.11 + 0.183 = 0.366 moles. Finally, we can find the final pressure using the equation P = nTotalRT/V = (0.366 moles * 0.0821 * 273 K) / 8.0 L = 8.07 atm. Rounded to the nearest whole number, the final pressure in the container at 0°C is 8 atm (option A).