= 17. A chemical reaction involves the combination of 0.200 mol of hydrogen and 0.200 mol of nitrogen in a rigid 2.00 L container at 773 K, represented by the following equation: 3H₂(g) + N₂(g) → 2NH3(g). At equilibrium the system contains 0.050 mol of ammonia. Use an ICE table to determine the equilibrium concentrations of hydrogen and nitrogen.

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17. A chemical reaction involves the combination of 0.200 mol of hydrogen and 0.200 mol of nitrogen in a
rigid 2.00 L container at 773 K, represented by the following equation: 3H₂(g) + N₂(g) → 2NH3(g). At
equilibrium the system contains 0.050 mol of ammonia. Use an ICE table to determine the equilibrium
concentrations of hydrogen and nitrogen.
Transcribed Image Text:17. A chemical reaction involves the combination of 0.200 mol of hydrogen and 0.200 mol of nitrogen in a rigid 2.00 L container at 773 K, represented by the following equation: 3H₂(g) + N₂(g) → 2NH3(g). At equilibrium the system contains 0.050 mol of ammonia. Use an ICE table to determine the equilibrium concentrations of hydrogen and nitrogen.
Expert Solution
Step 1

Given equilibrium reaction is 

3H2(g) + N2(g)  2NH3(g) 

Initially 0.200 mol of H2 and 0.200 mol of N2 are combined in a 2.00 L container

Equilibrium moles of NH3 = 0.050 mol 

We need to find equilibrium concentrations of H2 and I2 using ICE table 

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