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svp [43]
3 years ago
10

A) A sample of ideal gas is in a sealed container. The pressure of the gas is 725 torr, and the temperature is 18 ∘C. If the tem

perature changes to 75 ∘C with no change in volume or amount of gas, what is the new pressure, P2, of the gas inside the container? Express your answer with the appropriate units.
b) Using the same sample of gas (P1
= 725 torr, T1 = 18 ∘C ), we wish to change the pressure to 7250 torr with no accompanying change in volume or amount of gas. What temperature T2, in Celsius, is needed to reach this pressure? Express your answer with the appropriate units.
Chemistry
1 answer:
Fudgin [204]3 years ago
8 0

Answer:

a. The new pressure is 606,25 Torr.

b. -243,9°C is needed to reach the pressure of 7250 Torr.

Explanation:

Gay Lussac's law for gases says that if the volume in a gas remains constant, the pressure will be directly proportional to the temperature change.

P1 . T1 = P2. T2

(Temperature must be in K)

725 Torr . 291 K = P2 . 348 K

(725 Torr . 291 K) /348 K = P2

606,25 Torr = P2

725 Torr . 291K = 7250 Torr . T2

(725 Torr . 291K) /7250 Torr = T2

29,1 K = T2

T° K - 273 = T°C

29,1 K -273 = -243,9°C

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8 0
2 years ago
A 2.10 L vessel contains 4.65 mol of nitrous oxide (N2O) at 3.82 atm. What will be the pressure of this gas in a container that’
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Answer:

The answer to your question is 7.64 atm

Explanation:

Data

Volume 1 = V1 = 2.1 l

moles = 4.65

Pressure 1 = P1 = 3.82 atm

Volume 2 = Volume 1/2

Pressure 2 = ?

Process

1.- Calculate the new volume

Volume 2 = 2.10/2

Volume 2 = 1.05 l

2.- Use Boyle's law to find the Pressure

             P1V1 = P2V2

-Solve for P2

              P2 = P1V1 / V2

-Substitution

              P2 = (3.82)(2.1) / 1.05

-Simplification

              P2 = 8.022/1.05

-Result

              P2 = 7.64 atm

4 0
2 years ago
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