Hydrogen iodide decomposes according to the reaction 2 HI(g) ⇌ H2(g) + I2(g) A sealed 1.50−L container initially holds 0.00623 mol of H2, 0.00414 mol of I2, and 0.0244 mol of HI at 703 K. When equilibrium is reached, the concentration of H2(g) is 0.00467 M. What are the concentrations of HI(g) and I2(g)? [I2]eq M [HI]eq
Hydrogen iodide decomposes according to the reaction
2 HI(g) ⇌ H2(g) + I2(g)
A sealed 1.50−L container initially holds 0.00623 mol of H2, 0.00414 mol of I2, and 0.0244 mol of HI at 703 K. When equilibrium is reached, the concentration of H2(g) is 0.00467 M. What are the concentrations of HI(g) and I2(g)?
[I2]eq
M
[HI]eq
M
Given reaction
2 HI(g) ⇌ H2(g) + I2(g)
No. of moles 0.0244mol 0.00623mol 0.00414mol
Volume 1.5L 1.5L 1.5L
[initial] 0.016267M 0.004153M 0.00276 (mol/L)
Charge -2x x x
Equilibrium (0.016267-2x) (x+ 0.004153) (x+ 0.00276)
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