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3 years ago

Determine the density of chlorine gas at 22C and 1.00 atm pressure

1 answer:

3 0

T = 22.0 + 273.15 =295.15 K
Molar mass Cl2 = 70.906 g/mol
d = molar mass x p / RT = 70.906 x 1.00 / 0.0821 x 295.15 = 2.93 g/L
Hope this isn't to much? If it doesn't help you know where to find me :)

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What volume would a sample of gas occupy in LITERS at 0.985 atmospheres and a volume of 3.65 liters if the pressure were raised

musickatia [10]

Answer:

3.18 L

Explanation:

Step 1: Given data

Initial pressure (P₁): 0.985 atm

Initial volume (V₁): 3.65 L

Final pressure (P₂): 861.0 mmHg

Final volume (V₂): ?

Step 2: Convert P₁ to mmHg

We will use the conversion factor 1 atm = 760 mmHg.

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Step 3: Calculate the final volume of the gas

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3 years ago

3.0 cm x 4.0 cm x 1.0 cm [?]cm^3

CaHeK987 [17]

Explanation:

Hi there!!

you asked to multiply these all right,

you can simply multiply it ,

=3cm × 4 cm × 1cm

= 12cm^2×1cm (4×3=12)

= 12cm^3 (12×1=12)

Therefore, theanswer is 12 cm^3.

Hope it helps..

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3 years ago