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Veseljchak [2.6K]
3 years ago
7

at a certain pressure the density of superficial carbon dioxide is 0.469. what is the mass of a 25.0 mL sample of supercritical

carbon dioxide at this pressure?
Chemistry
1 answer:
Murrr4er [49]3 years ago
7 0

Answer:

\large \boxed{\text{11.7 g}}

Explanation:

\text{Mass} = \text{25.0 mL} \times \dfrac{\text{0.469 g}}{\text{1 mL}} = \textbf{11.7 g}\\\\\text{The mass of the carbon dioxide is $\large \boxed{\textbf{11.7 g}}$}

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The number of moles of gas lost is  0.0213 mol. It can be solved with the help of Ideal gas law.

<h3>What is Ideal law ?</h3>

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Where,

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