A 44.1 L sample of nitrogen gas at a pressure of 88.3 kPa is placed into a container of equal
volume that already holds hydrogen gas at a pressure of 125.6 kPa.
! What is the partial pressure of the nitrogen in the new container?
! What is the total pressure in the new container
I don't know what you mean by "equal volume".
To determine the partial pressure of nitrogen in the new container, as well as the total pressure in the new container, we can use the concept of Dalton's Law of Partial Pressures.
1. Dalton's Law of Partial Pressures states that the total pressure exerted by a mixture of ideal gases is equal to the sum of the pressures exerted by each individual gas. Mathematically, it can be represented as:
P_total = P_1 + P_2 + P_3 + ... + P_n
2. In this case, we have nitrogen gas and hydrogen gas in the new container. We know the initial pressure of nitrogen gas (P_nitrogen = 88.3 kPa) and the initial pressure of hydrogen gas (P_hydrogen = 125.6 kPa). Both gases are in separate containers of equal volume.
3. Since the volumes of the two containers are equal, when they are combined, each gas will occupy half of the total volume (22.05 L each).
4. To find the partial pressure of nitrogen in the new container, we can use the ideal gas law equation:
PV = nRT
Rearranging the equation, we get:
P = (n/V) * RT
5. Since the volume and temperature remain constant and the amount of nitrogen gas is constant, the ratio (n/V) for nitrogen will remain the same.
6. Hence, the partial pressure of nitrogen in the new container can be calculated as:
P_nitrogen_new = (n/V) * RT
7. To find the total pressure in the new container, we will add the partial pressures of nitrogen and hydrogen gas:
P_total_new = P_nitrogen_new + P_hydrogen
8. Plugging in the given values:
V_nitrogen = 44.1 L (volume of nitrogen gas)
V_hydrogen = 44.1 L (since both gases occupy equal volumes)
P_nitrogen_new = (n/V_nitrogen) * RT
P_total_new = P_nitrogen_new + P_hydrogen
9. To find the values of n and R, we need additional information, such as the number of moles of nitrogen gas and the ideal gas constant (R = 8.314 J/(mol*K)).
Without this information, it is not possible to calculate the partial pressure of nitrogen in the new container or the total pressure in the new container.