On a summer day early in the moming, a balloon is filled with helium when the temperature
is 21°C, but the temperature will reach a peak of 46°C later in the day. The balloon holds 12.8 L of helium gas at a starting pressure of 239 kPa. The balloon will burst when the internal pressure (Pb) reaches 256 kPa. Answer the following questions and show your
work

1. How many moles of helium gas are in the balloon?
2. What will the gas pressure be in the balloon at the peak temperature?
3. Will the balloons burst when the temperature reaches 42 degrees Celsius? Explain.
4. To what pressure should the helium gas pressure be reduced to avoid bursting the balloon? (Assume no significant volume change of the balloon)

Any help I’d great! Equations are not my strong suit

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

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:

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.

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