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NikAS [45]
2 years ago
12

Hot air balloons are open at their lower and end. A basket is suspended from the balloon and can take several passengers as well

as the pilot. A propane burner fixed to the basket is used to heat up the air in the balloon A hot balloon has a volume of 1500 m3 and its volume does not change when the enclosed air is heated.
1) Use the ideal gas equation, pV=nRT. to calculate how many molecules of the balloon contains at a temperature of 10 °C and a pressure 10.1 KP.
2) Calculate the mass of air it contains, assuming an average M of 29.​
Chemistry
2 answers:
makkiz [27]2 years ago
6 0

Answer:

using pv=nRt

Explanation:

p= 10.1 kp

v= 1500m3

n=?

R= 8.314

T= 10 + 273= 283k

pv = nRt

10.1 *1500=n*8.314*283

n= 10.1*1500/8.314*283

n= 15150/2352.862

n= 6.44 moles

2) n= mass/ molar mass

6.44= mass/ 29

mass= 29* 6.44

mass= 186.76g

Flauer [41]2 years ago
5 0

(a) The number of molecules contained by the balloon at the given condition is 6,438.97 moles.

(b) The mass of air in the balloon is 186.73 kg.

The given parameters;

  • <em>volume of the balloon, V = 1500 m³</em>
  • <em>temperature, T = 10⁰C = 273 + 10 = 283 K</em>
  • <em>pressure, = P = 10.1 kPa = 10,100 Pa</em>

The number of molecules contained by the balloon at the given condition is calculated as follows;

PV = nRT

where;

  • <em>R is ideal gas constant = 8.314 J/mol.K</em>
  • <em>n is the number of moles air in the balloon;</em>

n = \frac{PV}{RT} \\\\n = \frac{10,100 \times 1500}{8.314 \times 283} \\\\n = 6,438.97 \ moles

The mass of air in the balloon is calculated as;

n = \frac{m}{M} \\\\m = nM\\\\m = 6,438.97\ moles \ \times \ 29 \ g/mol\\\\m = 186.73 \ kg

Learn more here:brainly.com/question/13248885

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3 years ago
CH3OH can be synthesized by the following reaction.
puteri [66]

Answer:

A: There is 43.12 Liter of H2 needed

B: There is 21.56 liter of CO needed

Explanation:

Step 1: Data given

CO(g)+2H2(g)?CH3OH(g)

For 1 mol of CO consumed, we need 2 moles of H2 to produce 1 mol of CH3OH

Molar mass of CO = 28.01 g/mol

Molar mass of H2 = 2.02 g/mol

Molar mass of CH3OH = 32.04 g/mol

Step 2: What volume of H2 gas (in L), measured at 754mmHg and 90?C, is required to synthesize 23.0g CH3OH?

Pressure = 754 mmHg = 0.992 atm

Temperature = 90°C = 363 Kelvin

mass of CH3OH produced = 23.0 grams

Step 3: Calculate moles of CH3OH

Moles CH3OH = mass CH3OH / Molar mass CH3OH

Moles CH3OH = 23.0 grams / 32.04 g/mol

Moles CH3OH = 0.718 moles

Step 4: Calculate moles of H2

For 1 mol of CO consumed, we need 2 moles of H2 to produce 1 mol of CH3OH

For 0.718 moles CH3OH produced, we have 2*0.718 moles =1.436 moles of H2 and 0.718 moles of CO

Step 5: Calculate volume of H2

p*V = n*R*T

with p = the pressure = 0.992 atm

with V the volume = TO BE DETERMINED

with n = the number of moles = 1.436 moles H2

with R = the gasconstant = 0.08206 L*atm/ K*mol

with T = the temperature = 363 Kelvin

V = (n*R*T)/p

V = (1.436*0.08206*363)/0.992

V = 43.12 L

Step 6: Calculate volume of CO

p*V = n*R*T

with p = the pressure = 0.992 atm

with V the volume = TO BE DETERMINED

with n = the number of moles = 0.718  moles CO

with R = the gasconstant = 0.08206 L*atm/ K*mol

with T = the temperature = 363 Kelvin

V = (n*R*T)/p

V = (0.718*0.08206*363)/0.992

V = 21.56 L

A: There is 43.12 Liter of H2 needed

B: There is 21.56 liter of CO needed

3 0
3 years ago
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