Consider a 980-mL container at 133 °C in which the pressure of nitrogen oxide is 0.394x106 Pa.

a) What mass of nitrogen oxide (in g) is present in this container?
b) How many molecules is this?
(a)----g
(b)-----molecules

Use PV = nRT

Remember P is in atm and T in Kelvin. Solve for n = number of moles.
Then moles = grams/molar mass. Solve for grams. For b), remember there are 6.022 x 10^23 molecules in a mole.

To determine the mass of nitrogen oxide present in the container, you need to use the ideal gas law equation:

PV = nRT

Where:
P = pressure (in Pa)
V = volume (in m³)
n = number of moles
R = gas constant (8.314 J/(mol·K))
T = temperature (in Kelvin)

To find the number of molecules, you can use Avogadro's number, which states that there are 6.022 × 10^23 molecules in one mole of any substance.

Let's solve the problem step by step:

a) To find the mass of nitrogen oxide in grams, we first need to calculate the number of moles by rearranging the ideal gas law equation:

n = PV / RT

Convert the temperature from Celsius to Kelvin:
T (K) = 133 °C + 273.15 = 406.15 K

Now, substitute the given values into the equation:
n = (0.394 × 10^6 Pa) × (0.980 L) / (8.314 J/(mol·K)) × (406.15 K)

Note: The volume needs to be converted to cubic meters (m³) and the pressure to Pascals (Pa) for consistency in units.

Next, you can calculate the moles of nitrogen oxide.

Now, to find the mass, you need to multiply the number of moles by the molar mass of nitrogen oxide (NOx). Without specifying the exact compound, we cannot provide an accurate molar mass. However, you can look up the molar mass of the specific compound you're considering using a periodic table or another reference source.

b) To determine the number of molecules, multiply the number of moles by Avogadro's number (6.022 × 10^23 molecules/mol):

Number of molecules = n × (6.022 × 10^23 molecules/mol)

Now you should have the answers for both (a) and (b).