A 1.00-L flask was filled with 2.00 moles of gaseous SO₂ and 2.00 moles of gaseous NO2 and heated. After equilibrium was reached, It was found that 1.43 moles of gaseous NO was present. Assume that the reaction SO2(g) +NO₂(g) → SO3 (9) + NO(g) occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction. K= Submit Answer Retry Entire Group 9 more group attempts remaining
A 1.00-L flask was filled with 2.00 moles of gaseous SO₂ and 2.00 moles of gaseous NO2 and heated. After equilibrium was reached, It was found that 1.43 moles of gaseous NO was present. Assume that the reaction SO2(g) +NO₂(g) → SO3 (9) + NO(g) occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction. K= Submit Answer Retry Entire Group 9 more group attempts remaining
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Chapter1: Chemical Foundations
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A 1.00-L flask was filled with 2.00 moles of gaseous SO2 and 2.00 moles of gaseous NO₂ and heated. After equilibrium
was reached, It was found that 1.43 moles of gaseous NO was present. Assume that the reaction
SO₂(g) +NO2(g) → SO3(g) + NO(g)
F3
occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction.
K=
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Expert Solution
Step 1
Given that -
Volume of the flask = 1.00 L
Initial moles of SO2 gas = 2.00 moles
Initial moles of NO2 gas = 2.00 moles
Moles of NO gas after equilibrium reached = 1.43 moles
Now, from following equilibrium reaction, the ICE table can be written as -
| SO2(g) | +NO2(g) | <===> | SO3(g) | +NO(g) | |
| Initial | 2.00 | 2.00 | 0.00 | 0.00 | |
| Change | (2.00-1.43) | 2.00-1.43) | 1.43 | 1.43 | |
| Equilibrium | 0.57 | 0.57 | 1.43 | 1.43 |
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