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musickatia [10]
2 years ago
10

The pressure of a sample of argon gas was increased from 3.14 atm to 7.98 at a constant temperature. If the final volume of argo

n sample was 14.2 L what what’s the initial volume of the argon sample? Assume ideal behavior
Chemistry
1 answer:
noname [10]2 years ago
8 0

Answer:

<h2>36.09 L</h2>

Explanation:

The initial volume can be found by using the formula for Boyle's law which is

P_1V_1 = P_2V_2

where

P1 is the initial pressure

P2 is the final pressure

V1 is the initial volume

V2 is the final volume.

Since we're finding the initial volume

V_1 =  \frac{P_2V_2}{P_1}  \\

We have

V_1 =  \frac{7.98 \times 14.2}{3.14} =   \frac{113.316}{3.14}  \\  = 36.0878...

We have the final answer as

<h3>36.09 L</h3>

Hope this helps you

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Mercury chloride is a commercial fungicide. If the molar mass is 470 g/mol and the percent composition is 85.0% Hg and 15.0% Cl,
ElenaW [278]
Data: molar mass 470 g/mol

Percent composition:

Hg = 85.0%
Cl = 15.0%

Solution:

1)  Convert % to molar ratios

A. Base: 100 g

=> Hg = 85.0 g / 200.59 g/mol = 0.4235 mol

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B. divide by the higher number and round to whole number

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2) Find the mass of the empirical formula:

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3) Determine how many times is the empirical mass contained in the molecular mass:

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Answers:

Empirical formula HgCl
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3 years ago
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Calculate the work (kJ) done during a reaction in which the internal volume expands from 20 L to 43 L against an outside pressur
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Answer:

\large \boxed{\text{-10.0 kJ}}

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2. Convert litre-atmospheres to joules

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