What pressure will 2.6 x 1023 molecules of h2 exert in a 3.9 l container at 45°c?

We can use the ideal gas law equation to find the pressure

PV = nRT

where;

P - pressure

V - volume - 3.9 x 10⁻³ m³

R - universal gas constant - 8.314 Jmol⁻¹K⁻¹

T - temperature - 45 °C + 273 = 318 K

n - number of moles

there are 6.022 x 10²³ molecules in 1 mol of H₂

Therefore when theres 2.6 x 10²³ H₂ molecules - 1 / (6.022 x 10²³) x 2.6 x 10²³

Number of H₂ moles - 0.43 mol

substituting these values in the equation,

P x 3.9 x 10⁻³ m³ = 0.43 mol x 8.314 Jmol⁻¹K⁻¹ x 318 K

P = 291.5 kPa