Calculate the number of moles of HI that are at equilibrium with 1.42 mol of H₂ and 1.42 mol of 12 in a 3.50 L flask at 439°C.
H₂(g) + 1₂ (9)
2 HI(g)
mol
Kc
= 67.3 at 439°C

Question

ryannorfleet15p79e9n ryannorfleet15p79e9n

02-10-2022
Chemistry

Answered

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Calculate the number of moles of HI that are at equilibrium with 1.42 mol of H₂ and 1.42 mol of 12 in a 3.50 L flask at 439°C.
H₂(g) + 1₂ (9)
2 HI(g)
mol
Kc
= 67.3 at 439°C

Sagot :

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Calculate the number of moles of HI that are at equilibrium with 1.42 mol of H₂ and 1.42 mol of 12 in a 3.50 L flask at 439°C. H₂(g) + 1₂ (9) 2 HI(g) mol Kc = 67.3 at 439°C

Sagot :

Other Questions

Calculate the number of moles of HI that are at equilibrium with 1.42 mol of H₂ and 1.42 mol of 12 in a 3.50 L flask at 439°C.
H₂(g) + 1₂ (9)
2 HI(g)
mol
Kc
= 67.3 at 439°C