A 4-liter container at 25 degrees Celsius contains 2.0 grams of He gas. What is the pressure inside the container?

3.06 atm

Explanation:

Using general gas law equation as follows:

PV = nRT

Where;

P = pressure (atm)

V = volume (litres)

n = number of moles (mol)

R = gas law constant (0.0821 Latm/molK

T = temperature (K)

According to the information provided in this question, V = 4L, T = 25°C = 25 + 273 = 298K, n = ?

Mass of He gas = 2.0g

Using mole = mass ÷ molar mass

Molar Mass of He = 4g/mol

mole = 2/4

mole = 0.5mol

Using PV = nRT

P = nRT/V

P = 0.5 × 0.0821 × 298 ÷ 4

P = 12.233 ÷ 4

P = 3.06 atm

Hence, the pressure inside the container is 3.06atm.

- lead + phosphoric acid = hydrogen + lead(ii) phosphate

c. electrical charges of ionic bonds.