how many moles of N2 (g) re present in 1.00 of N2 (g) at 100 c and 1 atm?

represent 1.00 WHAT.....

To determine the number of moles of N2 (g) present in the given conditions, you need to use the ideal gas law equation:

PV = nRT

Where:
- P is the pressure in atmospheres (1 atm),
- V is the volume in liters (given as 1.00 L),
- n is the number of moles of the gas (what we're trying to find),
- R is the ideal gas constant (0.0821 L·atm/(mol·K)),
- T is the temperature in Kelvin (100 °C + 273.15).

First, convert the temperature from Celsius to Kelvin:
T = 100 °C + 273.15 = 373.15 K

Now, rearrange the ideal gas law equation to solve for moles:
n = PV / RT

Substitute the given values into the equation:
n = (1 atm) * (1.00 L) / (0.0821 L·atm/(mol·K)) * (373.15 K)

Now, calculate the value:
n = 0.0489 mol

Therefore, there are approximately 0.0489 moles of N2 (g) present in 1.00 L of N2 (g) at 100 °C and 1 atm.