Compelete the following table for an ideal gas.
P= 7.74*10^3 Pa
V= 10.3 mL
N= ?
T= 25°C
I'm getting 3.20e-4, but my online homework says its wrong, what am I doing wrong?
To find the value of N, the number of moles of the ideal gas, you can use the ideal gas law equation:
PV = nRT
Where:
P = pressure in Pascal (Pa)
V = volume in liters (L)
n = number of moles (N)
R = ideal gas constant (8.314 J/(mol·K))
T = temperature in Kelvin (K)
However, in your given data, the volume is provided in milliliters (mL), so it needs to be converted to liters before using it in the equation. Also, the temperature needs to be converted from Celsius (°C) to Kelvin (K) as the ideal gas law requires temperature in Kelvin.
First, let's convert the volume from mL to L:
10.3 mL = 10.3 / 1000 L = 0.0103 L
Next, let's convert the temperature from Celsius to Kelvin:
T (K) = T (°C) + 273.15
T (K) = 25 + 273.15 = 298.15 K
Now you can plug in the values into the ideal gas law equation:
(7.74 * 10^3 Pa) * (0.0103 L) = n * (8.314 J/(mol·K)) * (298.15 K)
Simplifying the equation:
n = (7.74 * 10^3 * 0.0103) / (8.314 * 298.15)
Calculating the value of n:
n ≈ 0.033831
So, the number of moles of the ideal gas is approximately 0.033831 mol.
It seems like there was an error in your calculation or conversion. Double-check your work and ensure that you've used the correct units for the volume and temperature.