Suppose a
500.mL
flask is filled with
1.1mol
of
CO
,
1.7mol
of
H2O
and
0.60mol
of
CO2
. The following reaction becomes possible:
+COgH2Og
+CO2gH2g
The equilibrium constant
K
for this reaction is
0.251
at the temperature of the flask.
Calculate the equilibrium molarity of
H2O
Suppose A 500 Ml Flask Is Filled With 1 1mol Of Co 1 7mol Of H2o And 0 60mol Of Co2 The Following Reaction Becomes P 1 (40.15 KiB) Viewed 40 times
Suppose a 500. mL flask is filled with 1.1 mol of CO, 1.7 mol of H₂O and 0.60 mol of CO₂. The following reaction becomes possible: CO(g) + H₂O(g) → CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 0.251 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. OM Check X 3 ? Save For Later 00 Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center B alo Ar Submit Assignment Accessibility
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