calculate the density of NO3 gas at 0.970mm Hg and 35C

Take 1 liter.

calculate n in PV=nRT
then, density= mass/volume= (n*molmassNO3)/1liter.

I STILL DON'T UNDERSTAND HOW TO DO IT COULD U PLEASE EXPLAIN

What don't you understand about
PV = nRT and how that fits your problem. Or is it the density part? Please be specific.

I apologize for the confusion. Let me explain step by step how to calculate the density of NO3 gas at 0.970 mm Hg and 35°C.

1. Start with the Ideal Gas Law equation: PV = nRT.

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 in Kelvin.

2. Convert the pressure and temperature to the appropriate units.

Given:
Pressure = 0.970 mm Hg
Temperature = 35°C

To convert mm Hg to atm, divide the pressure by 760:
Pressure = 0.970 mm Hg / 760 = 0.001276 atm

To convert °C to Kelvin, add 273.15:
Temperature = 35°C + 273.15 = 308.15 K

3. Determine the number of moles (n).

We'll rearrange the Ideal Gas Law equation to solve for n:
n = PV / RT

Substituting the known values:
n = (0.001276 atm) * 1 liter / (0.0821 atm·L/mol·K * 308.15 K) = 0.0000514 moles

4. Calculate the molar mass of NO3.

The molar mass of NO3 is calculated by adding up the atomic masses of nitrogen and three oxygen atoms:
Molar mass of NO3 = (1 * Atomic mass of N) + (3 * Atomic mass of O)

Atomic mass of N = 14.01 g/mol
Atomic mass of O = 16.00 g/mol

Molar mass of NO3 = (14.01 g/mol) + (3 * 16.00 g/mol) = 62.01 g/mol

5. Calculate the density.

Density = mass / volume

We have the number of moles (0.0000514 moles) and the molar mass (62.01 g/mol). We still need to determine the volume, which is given as 1 liter in this case.

Density = (0.0000514 moles * 62.01 g/mol) / 1 liter = 0.00319 g/L

Therefore, the density of NO3 gas at 0.970 mm Hg and 35°C is approximately 0.00319 g/L.

I hope this explanation helps clarify the steps involved in calculating the density of NO3 gas. Let me know if you have any further questions.