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?
See your post above.
To complete the table for an ideal gas, you need to use the ideal gas law formula, which states:
PV = nRT
Where:
P = pressure (in Pascal, Pa)
V = volume (in cubic meters, m³)
n = number of moles
R = ideal gas constant (8.314 J/(mol·K))
T = temperature (in Kelvin, K)
In your case, you have the pressure (P = 7.74*10^3 Pa) and volume (V = 10.3 mL), but the volume needs to be converted to cubic meters and the temperature needs to be converted to Kelvin.
First, convert the volume from milliliters to cubic meters:
V = 10.3 mL = 10.3 * 10^(-6) m³
Next, convert the temperature from Celsius to Kelvin:
T = 25°C + 273.15 = 298.15 K
Now, we can plug in the values into the ideal gas law formula to solve for the number of moles (n):
n = (PV) / (RT)
n = (7.74*10^3 Pa * 10.3 * 10^(-6) m³) / (8.314 J/(mol·K) * 298.15 K)
By doing the calculations, you should get an answer of approximately 3.16 x 10^(-4) mol, which is equivalent to 3.16 x 10^(-2) mmol or 316 μmol.
Since your answer of 3.20 x 10^(-4) is very close to the correct answer, it's possible that the difference is due to rounding or significant figure rules. Make sure to check the instructions or guidelines in your online homework to determine how many significant figures or decimal places are required in your answer.