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worty [1.4K]
2 years ago
7

A 46.2 L sample of gas exerts 237.4 mm Hg pressure at 139.2 ºC. What volume does the gas have at 702.4 mm Hg and 63.4 ºC?

Chemistry
1 answer:
zvonat [6]2 years ago
5 0

7.111 L is the volume of gas with 702.4 mm Hg and 63.4 ºC.

<h3>What is an ideal gas equation?</h3>

The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

Given data:

V_1=46.2 L

P_1=237.4 mm Hg

T_1=139.2 ºC

V_2=?

P_2=702.4 mm Hg

T_2=63.4 ºC

Using the given below formula:

\frac{V_1 X P_1}{T_1} = \frac{V_1 X P_1}{T_2}

\frac{46.2 L X 237.4 \;mm Hg}{139.2} = \frac{V_2 X 702.4 mm Hg}{63.4 ºC}

V_2 = 7.111 L

Hence, 7.111 L is the volume of gas with 702.4 mm Hg and 63.4 ºC.

Learn more about the ideal gas here:

brainly.com/question/27691721

#SPJ1

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13mL

Explanation:

Step 1:

The balanced equation for the reaction. This is given below:

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From the balanced equation above, we obtained the following data:

Mole ratio of the acid (nA) = 1

Mole ratio of the base (nB) = 1

Step 2:

Data obtained from the question.

This includes the following:

Molarity of the acid (Ma) = 6M

Volume of the acid (Va) =?

Volume of the base (Vb) = 39mL

Molarity of the base (Mb) = 2M

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Determination of the volume of the acid.

Using the equation:

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MaVa/MbVb = nA/nB

6 x Va / 2 x 39 = 1/1

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Divide both side by 6

Va = (2 x 39)/6

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