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tatyana61 [14]
3 years ago
11

A 1.50 liter flask at a temperature of 25°C contains a mixture of 0.158 moles of methane, 0.09 moles of ethane, and 0.044 moles

of butane. What is the total pressure of the mixture inside the flask?
Physics
1 answer:
Julli [10]3 years ago
7 0
Applying the general gas equation : PV=nRT
V = 1.50 litres
R = <span>0.08205746 L atm/K mol
T = </span><span>25°C = 25+273 = 298 K
n = </span>0.158 moles+0.09 moles+<span> 0.044 moles = 0.292 moles
</span><span>Re arranging the equation:
P = nRT / V = (0.158 + 0.09 + 0.044) mol x (0.08205746 L atm/K mol)
 x (25 + 273)K / (1.50 L)
= 4.76 atm
= 482 kPa
= 3617 mmHg</span>
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Hi there!

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<u>vA + vA´ = 4 vB´</u>

<u />

The change in momentum of glider A (ΔpA) is calculated as follows:

ΔpA = final momentum - initial momentum

ΔpA =  -mA · vA´ - mA · vA = -mA (vA + vA´) = -4mA · vB´

The change in momentum of glider B (ΔpB) is calculated as follows:

ΔpB = final momentum - initial momentum

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