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Cloud [144]
3 years ago
6

if the temperature of 20.0 L of gas were increased to twice the initial value, while the pressure is held constant what would be

the volume of the gas at the new temperature
Chemistry
1 answer:
Kay [80]3 years ago
7 0

Answer:

40 L

Explanation:

From the question given above, the following data were obtained:

Initial volume (V₁) = 20 L

Initial temperature (T₁) = T

Final temperature (T₂) = 2T

Pressure (P) = constant

Final volume (V₂) =?

The new (i.e final) volume of the gas can be obtained as follow:

V₁/T₁ = V₂/T₂

20/T = V₂/2T

Cross multiply

T × V₂ = 20 × 2T

T × V₂ = 40T

Divide both side by T

V₂ = 40T /T

V₂ = 40 L

Therefore, the new volume of the gas is 40 L

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2 years ago
Calculate the volume which 1.00 mole of a gas occupies at 1 atm and 298K?
elena-14-01-66 [18.8K]

Answer:

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Explanation:

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Calculate the following quantity: molarity of a solution prepared by diluting 45.45 mL of 0.0404 M ammonium sulfate to 550.00 mL
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Answer:

M_2=3.34x10^{-3}M

Explanation:

Hello!

In this case, since a dilution process implies that the moles of the solute remain the same before and after the addition of diluting water, we can write:

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Thus, since we know the volume and concentration of the initial sample, we compute the resulting concentration as shown below:

M_2=\frac{M_2V_2}{V_1} =\frac{45.45mL*0.0404M}{550.00mL}\\\\M_2=3.34x10^{-3}M

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5 0
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Explanation:

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