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DaniilM [7]
3 years ago
5

A balloon that had a volume of 3.50 L at 25.0°C is placed in a hot room at 40.0°C. If the pressure remains constant at 1.00 atm,

what is the new volume of the balloon in the hot room? Use mc005-1.jpg.
Chemistry
2 answers:
Elina [12.6K]3 years ago
7 0

Using charles law, this would equal 3.68 L

belka [17]3 years ago
6 0

To solve this we assume that the gas inside the balloon is an ideal gas. Then, we can use the ideal gas equation which is expressed as PV = nRT. At a constant pressure and number of moles of the gas the ratio T/V is equal to some constant. At another set of condition of temperature, the constant is still the same. Calculations are as follows:

T1 / V1 = T2 / V2

V2 = T2 x V1 / T1

V2 = 313.15 x 3.50 / 298.15

<span>V2 = 3.68 L</span>

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Read 2 more answers
A 10.0 L sample of gas has a pressure of the 1.00 atm. If the volume increases to 15.0 L, what is the pressure of the gas ? Assu
Tanya [424]

Answer:

0.67 atm

Explanation:

From the question,

Applying Boyles law

PV = P'V'......................... Equation 1

Where P = Initial Pressure of the sample of gas, P' = Final pressure of the sample of gas, V = Initial volume of the sample of gas, V' = Final volume of the sample of gas.

make P' the subject of the equation above

P' = PV/V'.................... Equation 2

Given: P = 10.0 L, V = 1.0 atm, V' = 15.0 L

Substitute these values into equation 2

P' = (10.0×1.0)/15.0

P' = 0.67 atm

3 0
3 years ago
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