1)A completely empty 2.00 L reaction vessel is filled with ammonia gas (NH3) at a constant...

1)A completely empty 2.00 L reaction vessel is filled with ammonia gas (NH₃) at a constant temperature of 680K. The initial partial pressure of NH₃ was 9.40 atm. With time it partially decomposed according to the reaction below until equilibrium was reached:

2 N H 3 ( g ) ⟺ 3 H 2 ( g ) + N 2 ( g )

At equilibrium the total pressure inside the flask was 12.80 atm. What is the equilibrium partial pressure of all components?Use Rices table.

2)What is the Molar Solubility of copper(II) phosphate in a 0.40 M sodium phosphate solution?

The KSP of copper(II) phosphate is 1.40E–37. Use Rices table.

Solutions

Expert Solution

Use rice table to calculate the concentration in equilibrium and then put the values into equation to find the desired value.

NOTE: DEAR STUDENT IF YOU HAVE ANY QUERIES PLEASE ASK IN THE COMMENT. ALL THE BEST.

queen_honey_blossom answered 1 year ago

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