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disa [49]
3 years ago
9

ICK

Chemistry
1 answer:
Lesechka [4]3 years ago
4 0

Answer:

The new volume, after increasing the pressure to 785 torr, will be 1.22 L

Explanation:

Step 1: Data given

Volume of neon sign is 1.51 L

Pressure of the neon gas = 635 torr

The pressure increases to 785 torr

Step 2: Calculate the volume

P1*V1 = P2*V2

⇒with P1 = the initial pressure of the gas = 635 torr

⇒with V1 = the initial volume of the gas = 1.51 L

⇒with P2 = the increased pressure = 785 torr

⇒with V2 = the new volume = TO BE DETERMINED

635 torr * 1.51 L = 785 torr * V2

V2 = (635 torr * 1.51 L ) / 785 torr

V2 = 1.22 L

The new volume, after increasing the pressure to 785 torr, will be 1.22 L

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A sample of a vapor occupies a volume of 500 mL at 65°C. If pressure remains constant, what is the volume of the gas at standard
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Answer:

403 mL

Explanation:

First, I will assume that the mole is 1, because you are not specifing this.

Now, with the innitial data, we need to get the pressure:

T = 65+273 = 338 K

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Now if:

PV = nRT

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Let's calculate the P:

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The standard temperature is 0° C or 273 K so, the volume is:

V = 1 * 0.082 * 273 / 55.432

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8 0
3 years ago
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Answer:

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A single C-C or C-H bond is in a tetrahedral geometry, the carbon atom is bonded to four species with a bond angle of 109°.

A C=C bond is trigonal planar with a bond angle of 120°.

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Answer:

I hope it helps u

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