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Mastering Chem Partial Pressure Q?
Assignment 1 Exercise 20.9
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Exercise 20.9
In the reaction A(g)→2B(g)+C(g),
the total pressure increases while the partial pressure of A(g) decreases. The initial pressure of A(g) in a vessel of constant volume is 6.600×10^3 mmHg .
Thru ICE diagram I found the total pressure after the reaction as gone to competion is Pt= 1.980x 10^-4 mmHg.
However what will be the total gas pressure when the partial pressure of A(g) drops to 7.60x10^-2 mmHg?
Pt= ?
How would I go about this???
1 Answer
- Roger the MoleLv 74 years ago
(6.600 × 10^3 mmHg) - (7.60x10^-2 mmHg) = 6599.924 mmHg A reacted
(6599.924 mmHg A) x (3 mol products / 1 mol reactant) = 19799.772 mmHg products
(19799.772 mmHg products) + (7.60 x 10^-2 mmHg) = 19799.848 mmHg total
But when you round off correctly the answer is the same as if all the A had been consumed.
This is not surprising since all of "7.60x10^-2 mmHg" is outside the significant-digit limit of "6.600×10^3 mmHg" in the first place.
Supposing all the given number have been copied correctly, your answer for the total volume ought to be
1.980 x 10^+4 mmHg.
