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FromTheMoon [43]
3 years ago
12

At constant temperature, if a gas occupies 312 mL at a pressure of 1.60 atm, what pressure is necessary for this gas to occupy a

volume of 500 mL?
Chemistry
1 answer:
inn [45]3 years ago
5 0

Answer:

P₂ = 1.0 atm

Explanation:

Boyles Law problem => P ∝ 1/V at constant temperature (T).

Empirical equation

P ∝ 1/V => P = k(1/V) => k = P·V => for comparing two different case conditions, k₁ = k₂ => P₁V₁ = P₂V₂

Given

P₁ = 1.6 atm

V₁ = 312 ml

P₂ = ?

V₂ = 500 ml

P₁V₁ = P₂V₂ => P₂ = P₁V₁/V₂ =1.6 atm x 312 ml / 500ml = 1.0 atm

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<u>Answer:</u> The identity of the unknown acid is butanoic acid or ascorbic acid.

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The chemical equation for the reaction of NaOH and diprotic acid follows:

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Mass of L-tartaric acid = 2.002 g

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Putting values in above equation, we get:

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