10 grams of argon and 20.0 g of the neon are placed in a 1200.0 ml container at 25 degrees C. The partial pressure of neon is?
n Ne = grams/molar mass
Then PV = nRT and solve for P.
To find the partial pressure of neon (P_neon), we need to use the ideal gas law equation: PV = nRT, where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
First, let's calculate the number of moles of argon and neon using their respective masses and molar masses:
Molar mass of argon (Ar) = 39.95 g/mol
Molar mass of neon (Ne) = 20.18 g/mol
Number of moles of argon (n_ar):
n_ar = mass_ar / molar mass_ar
n_ar = 10 g / 39.95 g/mol
n_ar ≈ 0.25 mol
Number of moles of neon (n_neon):
n_neon = mass_neon / molar mass_neon
n_neon = 20.0 g / 20.18 g/mol
n_neon ≈ 0.99 mol
Next, we need to convert the volume from milliliters (ml) to liters (L):
V = 1200.0 ml = 1200.0 / 1000 L = 1.2 L
Given that the temperature is 25°C, we need to convert it to Kelvin (K):
T = 25°C + 273.15 = 298.15 K
Now, let's find the partial pressure of neon:
P_neon = (n_neon * R * T) / V
The ideal gas constant (R) is approximately 0.0821 L·atm/(mol·K). Substituting the known values into the equation:
P_neon = (0.99 mol * 0.0821 L·atm/(mol·K) * 298.15 K) / 1.2 L
P_neon ≈ 20.2 atm
Therefore, the partial pressure of neon is approximately 20.2 atm in the given conditions.
To find the partial pressure of neon in the container, we can use the ideal gas law, which states:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles of gas
R = ideal gas constant
T = temperature
First, we need to calculate the number of moles of neon gas. We can use the formula:
n = mass / molar mass
The molar mass of neon is approximately 20.18 g/mol. Therefore, the number of moles of neon is:
n(neon) = 20.0 g / 20.18 g/mol
Next, we need to convert the volume of the container to liters. Since 1 L = 1000 mL, the volume is:
V = 1200.0 mL / 1000 mL/L
Now, let's plug the values into the ideal gas law equation:
(P(neon))(V) = (n(neon))(R)(T)
We are solving for P(neon), so rearranging the equation yields:
P(neon) = (n(neon))(R)(T) / V
Here are the known values:
n(neon) = 20.0 g / 20.18 g/mol
R = 0.0821 L·atm/(mol·K)
T = 25 °C + 273.15 K (conversion to Kelvin)
V = 1200.0 mL / 1000 mL/L
Now, calculate P(neon) using these values.