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?

You didn't show your work so I don't know what you're doing wrong. Perhaps nothing more than punching the wrong button?

PV = nRT
7.74kPa x 0.0103L = n*8.314*298K
n = 3.22E-5 moles

To find the value of N (number of moles), we can use the ideal gas equation:

PV = nRT

Where:
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.

First, we need to convert the pressure (P) from pascals (Pa) to atmospheres (atm), since the ideal gas constant (R) is often given in terms of atm.

1 atm = 101325 Pa

So, converting P from Pa to atm:
P = 7.74 * 10^3 Pa / 101325 Pa/atm = 0.0763 atm

Next, we need to convert the volume (V) from milliliters (mL) to liters (L), as the ideal gas equation requires volume in liters.
1 L = 1000 mL

So, converting V from mL to L:
V = 10.3 mL / 1000 mL/L = 0.0103 L

Now, let's convert the temperature (T) from Celsius (°C) to Kelvin (K), which is the unit required for temperature in the ideal gas equation.

T(K) = T(°C) + 273.15
T(K) = 25°C + 273.15 = 298.15 K

Now, let's substitute the values into the ideal gas equation:

(0.0763 atm) * (0.0103 L) = n * (0.0821 L atm/mol K) * (298.15 K)

Simplifying, we get:

0.0007869 atm L = 0.024378 n

Next, solve for n:

n = (0.0007869 atm L) / (0.024378)

n ≈ 0.0322 moles

Therefore, the correct value for N (number of moles) is approximately 0.0322 moles, not 3.20e-4 moles.