Chemistry, 15.02.2020 10:44 ineedhelpireallydo

15.1 L N2 at 25 °C and 125 kPa and 44.3 L O2 at 25 °C and 125 kPa were transferred to a tank with a volume of 6.25 L. What is the total pressure at 51 °C?

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Answer from: mandy9386

The total pressure of the gas mixture which were transferred to a tank of 6.25 L at 51 °C is 1291.7 KPa

We'll begin by calculating the number of mole of N₂ and O₂ which was transferred. This can be obtained as follow:

For N₂:

Volume (V) = 15.1 L

Temperature (T) = 25 °C = 25 + 273 = 298 K

Pressure (P) = 125 KPa

Gas constant (R) = 8.314 L.KPa/Kmol

Number of mole (n) =?

PV = nRT

125 × 15.1 = n × 8.314 × 298

1887.5 = n × 2477.572

Divide both side by 2477.572

n = 1887.5 / 2477.572

n = 0.762 mole For O₂:

Volume (V) = 44.3 L

Temperature (T) = 25 °C = 25 + 273 = 298 K

Pressure (P) = 125 KPa

Gas constant (R) = 8.314 L.KPa/Kmol

Number of mole (n) =?

PV = nRT

125 × 44.3 = n × 8.314 × 298

5537.5 = n × 2477.572

Divide both side by 2477.572

n = 5537.5 / 2477.572

n = 2.235 molesNext, we shall determine the total mole of the mixture.

Mole of N₂ = 0.762 mole

Mole of O₂ = 2.235 moles

Total mole = 0.762 + 2.235

Total mole = 2.997 moles Finally, we shall determine the total pressure at 51 °C. This can be obtained as follow:

Volume (V) = 6.25 L

Temperature (T) = 51 °C = 51 + 273 = 324 K

Gas constant (R) = 8.314 L.KPa/Kmol

Total of mole (n) = 2.997 moles

Total Pressure (P) =?

PV = nRT

P × 6.25 = 2.997 × 8.314 × 324

P × 6.25 = 8073.126792

Divide both side by 6.25

P = 8073.126792 / 6.25

P = 1291.7 KPa

Therefore, the total pressure of the gas mixture at 51 °C is 1291.7 KPa

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Answer from: pandaho

The total pressure of the mixture in the tank of volume 6.25 litres at 51°C is 1291.85 kPa.

Explanation:

For N2,

Pressure(P₁)=125 kPa

Volume(V₁)=15·1 L

Temperature (T₁)=25°C=25+273 K=298 K

Similarly, for Oxygen,

Pressure(P₂)= 125 kPa

Volume(V₂)= 44.3 L

Temperature(T₂)=25°C= 298 K

Then, for the mixture,

Volumeof the mixture( V)= 6.25 L

Pressure(P)=?

Temperature (T)= 51°C = 51+273 K=324 K

Then, By Combined gas laws,

$\frac{P_{1} V_{1} }{T_{1} } +\frac{P_{2} V_{2} }{T_{2} } =\frac{PV}{T}$

or, $\frac{15.1*125}{298} +\frac{44.3*125}{298} =\frac{P*6.25}{324}$

or, $6.34+18.58=\frac{P*6.25}{324}$

or, $P=\frac{24.92*324}{6.25}$

∴P=1291.85 kPa

So the total pressure of the mixture in the tank of volume 6.25 litres at 51°C is 1291.85 kPa.

Answer from: Quest

You use the atomic number to find out how many protons and neutrons there are in the atom. you use the atomic mass to find out how many protons and electrons there are in the atom.

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15.1 L N2 at 25 °C and 125 kPa and 44.3 L O2 at 25 °C and 125 kPa were transferred to a tank with a...

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