Question 1 A 350 mL glass bulb is filled with an unknown gas with a mass of 0.225 g fills, a pressure of 733 mmHg and a temperature of 22 °C. Is this gas argon (Ar), methane
X (CH4), nitrogen monoxide (NO), or carbon monoxide (CO)?

Methane

Explanation:

Step 1: Convert the volume to L

We will use the relationship 1 L = 1000 mL.

350 mL × 1 L/1000 mL = 0.350 L

Step 2: Convert the pressure to atm

We will use the relationship 1 atm = 760 mmHg.

733 mmHg × 1 atm/760 mmHg = 0.964  atm

Step 3: Convert the temperature to Kelvin

We will use the following expression.

K = °C + 273.15 = 22 + 273.15 = 295 K

Step 4: Calculate the moles of the gas

We will use the ideal gas equation

P × V = n × R ×T

n = P × V/R ×T

n = 0.964 atm × 0.350 L/0.0821 atm.L/mol.K ×295 K

n = 0.0139 mol

Step 5: Calculate the molar mass of the gas

0.0139 moles have a mass of 0.225 g. The molar mass of the gas is:

0.225 g / 0.0139 mol = 16.2 g/mol

From the options, methane is the gas with a molar mass of about 16.2 g/mol.

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.

i just learnt this recently but i need to look through my notes again