a. How many moles of N2 are present in a 1.00 qt flask that has a pressure of 425 torr at a temperature of 35°C?

What is the mass in this na2?

It would be much simpler to change quart to liters first, then torr to kpa

PV=nRT

n= PV/RT Temps in Kelvins, V in liters, P in kpa

I did that but I keep getting the wrong answer

Why don't you show your work and let us find the error? You can play hide and seek with these problems all day long.

1L=1.06qt

1.00 / 1.06 = 0.94339623

425 torr = 56.7 kpa

35= 308.15 k

56.7/0.0821*308.15 = 212814.921

Your numbers don't look all that bad except you are using the wrong R. The value of 0.08206 is used with p in atm. When you use kPa R is 8.314. I would have used 0.946 for 1 qt to L (the easy way to do the conversion is to go to Google, type in "1.00 quart to" without the quotation marks and hit the enter key. Up pops 0.946 L).

I used what you said but I'm still getting the wrong answer. I'm sorry I really struggle in chemistry

To find the number of moles of N2 present in the flask, we can use the ideal gas law equation:

PV = nRT

Where:
P is the pressure (in kPa)
V is the volume (in liters)
n is the number of moles
R is the ideal gas constant (0.0821 L·atm/mol·K or 8.3145 J/mol·K)
T is the temperature (in Kelvins)

You mentioned that you converted the volume from quart to liters and the pressure from torr to kPa, which is a good approach. Let's assume you have the correct conversions.

To find the number of moles, we rearrange the ideal gas law equation to solve for n:

n = PV / RT

Here's how you can calculate it:

Step 1: Convert the volume from quart to liters (1 quart = 0.946353 liters).
Step 2: Convert the pressure from torr to kPa (divide by 7.50062).
Step 3: Convert the temperature from Celsius to Kelvin (add 273.15).

Let's assume the volume after conversion is V = 0.946353 liters, the pressure after conversion is P = 425 torr / 7.50062 = 56.67 kPa, and the temperature after conversion is T = 35°C + 273.15 = 308.15 K.

Now substitute the values into the equation:

n = (56.67 kPa) * (0.946353 L) / [(0.0821 L·atm / mol·K) * (308.15 K)]

Calculating this expression, you will find the number of moles of N2 in the flask.

To find the mass of N2, you need to know the molar mass of N2, which is approximately 28.0134 g/mol (two nitrogen atoms).

Multiply the number of moles of N2 by the molar mass to get the mass:

Mass of N2 = Number of moles of N2 * Molar mass of N2 (28.0134 g/mol)

Evaluate this expression using the number of moles you calculated, and you will get the mass of N2 present in the flask.