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Arturiano [62]
3 years ago
7

The Goodyear blimp we usually see hovering above our heads at a football game contains 5600 m3 of helium gas. If there are 1070

kg of gas at an absolute pressure of 1.10 105 Pa in the blimp, what is the temperature of the gas? The atomic mass of helium 4.00260 g/mol.
Chemistry
1 answer:
Alina [70]3 years ago
8 0

Answer:

277.16 K is the temperature of the gas.

Explanation:

Using ideal gas equation:

PV = nRT

where,

P = Pressure of gas = 1.10\times 10^5 Pa

V = Volume of gas = 5600 m^3

n = number of moles of gas = \frac{1,070 kg}{4.00260 g/mol}=\frac{1,070,000 g}{4.00260 g/mol}=267,326.24 mol

R = Gas constant = 8.314 J/mol.K

T = Temperature of gas = ?

Putting values in above equation, we get:

T=\frac{PV}{RT}

T=\frac{1.10\times 10^5 Pa\times 5,600 m^3}{267,326.24 mol\times 8.314 J/mol K}

T = 277.16 K

277.16 K is the temperature of the gas.

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Answer:

The final volume of the balloon is = 28.11 L

Explanation:

Initial pressure P_{1} = 1.03 atm = 104.325 K pa

Initial temperature T_{1} = 26 °c = 299 K

Initial volume V_{1} = 22.4 L

Final temperature T_{2} = 22 °c = 295 K  

Final pressure P_{2} = 0.81 atm = 82 K pa

We know that

\frac{P_{1} V_{1} }{T_{1} } = \frac{P_{2} V_{2} }{T_{2} }

Put all the values in above formula we get

\frac{(104.325)(22.4)}{299} = \frac{(82)(V_{2} )}{295}

V_{2} = 28.11 L

This is the final volume of the balloon.

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2 years ago
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2. Heating was required to get rid of the H₂O. When all moisture is gone, you weigh the sample. Afterwhich, you further heat it to get ride of the oxygen. By doing this, you would know the individual mass of each element. Then, you can solve for the empirical formula of the oxide of tin.
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