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2 years ago

On a summer day early in the moming, a balloon is filled with helium when the temperature

Chemistry

1 answer:

MAXImum [283]2 years ago

6 0

Based on the data provided;

number of moles of helium gas is 1.25 moles
pressure at peak temperature is 259.3 kPa
internal pressure is above 256 kPa, therefore, the balloon will burst.
pressure should be reduced to a value less than 256 kPa by reducing the temperature

<h3>What is the ideal has equation?</h3>

The ideal gas equation relatesthe pressure, volume, moles and temperature of a gas.

The moles of helium gas is calculated using the Ideal gas equation:

PV = nRT

n is the number of moles of gas

R is molar gas constant = 8.314 L⋅kPa/Kmol

P is pressure = 239 kPa

T is temperature = 21°C = 294 K

V is volume = 12.8 L

Therefore;

n = PV/RT

n = 239 × 12.8 / 8.314 × 294

n = 1.25 moles

The number of moles of helium gas is 1.25 moles

At peak temperature, T = 46°C = 319 K

Using P1/T1 = P2/T2

P2 = P1T2/T1

P2 = 239 × 319/294

P2 = 259.3 kPa

The pressure at peak temperature is 259.3 kPa

At 42°C, T = 315 K

Using P1/T1 = P2/T2

P2 = P1T2/T1

P2 = 239 × 315/294

P2 = 256.07 kPa

Since the internal pressure is above 256 kPa, the balloon will burst.

The pressure should be reduced to a value less than 256 kPa by reducing the temperature.

Learn more about gas ideal gas equation at: brainly.com/question/12873752

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sineoko [7]

Answer:

3. V = 0.2673 L

4. V = 2.4314 L

5. V = 0.262 L

6. V = 2.224 L

Explanation:

3. assuming ideal gas:

PV = RTn

∴ R = 0.082 atm.L/K.mol

∴ V1 = 225 L

∴ T1 = 175 K

∴ P1 = 150 KPa = 1.48038 atm

⇒ n = RT/PV

⇒ n = ((0.082 atm.L/K.mol)(175 K))/((1.48038 atm)(225 L))

⇒ n = 0.043 mol

∴ T2 = 112 K

∴ P2 = P1 = 150 KPa = 1.48038 atm

⇒ V2 = RT2n/P2

⇒ V2 = ((0.082 atm.L/K.mol)(112 K)(0.043 mol))/(1.48038 atm)

⇒ V2 = 0.2673 L

4. gas is heated at a constant pressure

∴ T1 = 180 K

∴ P = 1 atm

∴ V1 = 44.8 L

⇒ n = RT/PV

⇒ n = ((0.082 atm.L/K.mol)(180 K))/((1 atm)(44.8 L))

⇒ n = 0.3295 mol

∴ T2 = 90 K

⇒ V2 = RT2n/P

⇒ V2 = ((0.082 atm.L/K.mol)(90 K)(0.3295 mol))/(1 atm)

⇒ V2 = 2.4314 L

5. V1 = 200 L

∴ P1 = 50 KPa = 0.4935 atm

∴ T1 = 271 K

⇒ n = RT/PV

⇒ n = ((0.082 atm.L/K.mol)(271 K))/((0.4935 atm)(200 L))

⇒ n = 0.2251 mol

∴ P2 = 100 Kpa = 0.9869 atm

∴ T2 = 14 K

⇒ V2 = RT2n/P2

⇒ V2 = ((0.082 atm.L/K.mol)(14 K)(0.2251 mol))/(0.9869 atm)

⇒ V2 = 0.262 L

6.a) ∴ V1 = 24.6 L

∴ P1 = 10 atm

∴ T1 = 25°C = 298 K

⇒ n = RT/PV

⇒ n = ((0.082 atm.L/K.mol)(298 K))/((10 atm)(24.6 L))

⇒ n = 0.0993 mol

∴ T2 = 273 K

∴ P2 = 101.3 KPa = 0.9997 atm

⇒ V2 = RT2n/P2

⇒ V2 = ((0.082 atm.L/K.mol)(273 K)(0.0993 mol))/(0.9997 atm)

⇒ V2 = 2.224 L

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3 years ago

What size volumetric flask would you use to create a 1.00M solution using 166.00 g of KI?

mr Goodwill [35]

Answer:

A 1 liter volumetric flask should be used.

Explanation:

First we <u>convert 166.00 g of KI into moles</u>, using its <em>molar mass</em>:

Molar mass of KI = Molar mass of K + Molar mass of I = 166 g/mol

166.00 g ÷ 166 g/mol = 1 mol KI

Then we <u>calculate the required volume</u>, using the <em>definition of molarity</em>:

Molarity = moles / liters

Liters = moles / molarity

1 mol / 1.00 M = 1 L

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Answer:

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Explanation:

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makkiz [27]

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Answer:

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