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bronzecod748Lv1
28 Sep 2019
The equilibrium constant for HI decomposition at 500 °C is5.8Ã10-3.
2HI(g) <=> H2(g) + I2(g)
At that temperature reactants and products are gaseous. (There isno change in the total number of moles, so Kc = Kp.)
A sample of 0.40 mol of HI is placed in a 1.00 L vessel which isthen heated to 500 °C. When equilibrium is reached, what is themolar concentration of H2? (Give units).
The equilibrium constant for HI decomposition at 500 °C is5.8Ã10-3.
2HI(g) <=> H2(g) + I2(g)
At that temperature reactants and products are gaseous. (There isno change in the total number of moles, so Kc = Kp.)
A sample of 0.40 mol of HI is placed in a 1.00 L vessel which isthen heated to 500 °C. When equilibrium is reached, what is themolar concentration of H2? (Give units).
2HI(g) <=> H2(g) + I2(g)
At that temperature reactants and products are gaseous. (There isno change in the total number of moles, so Kc = Kp.)
A sample of 0.40 mol of HI is placed in a 1.00 L vessel which isthen heated to 500 °C. When equilibrium is reached, what is themolar concentration of H2? (Give units).
Irving HeathcoteLv2
28 Sep 2019
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