How much hydrogen (H2) gas is needed to fill an 80.0 L tank to a pressure of 150 atm at 27°C​

PV = nRT

P - pressure - 150.0 atm x 101 325 Pa/atm = 15 198 750 Pa

V - volume  - 80 x 10⁻³ m³

n - number of moles

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

T - temperature in K - 27 °C + 273 = 300 K

substituting the values in the equation

15 198 750 Pa  x 80 x 10⁻³ m³ = n x 8.314 Jmol⁻¹K⁻¹ x 300 K

n = 487.5 mol

molar mass of CO₂ is 44 g/mol

mass of CO₂ - 44 g/mol x 487.5 mol = 21 450 g

mass of CO₂ required is 21.450 kg

Explanation:

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

24

answer; 4 electrons;