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3 years ago

What volume does 2.25g of nitrogen gas, N2, occupy at 273 Celsius and 1.02 atm

Chemistry

1 answer:

kotykmax [81]3 years ago

5 0

<h2><u>Answer:</u></h2>

0.126 Liters

<h2><u>Explanation:</u></h2>

V = mRT / mmP

First, convert the 2.25g of Nitrogen gas into moles. (m in the equation above)

2.25g x 1 mole / 28.0g = 0.08036 moles = m

28.0g = mm

Next, convert the 273 Celsius into Kelvin. (T in the equation above)

273 Celsius + 273.15 = 546.15K = T

R = 0.08206L*atm/mol*K

(Quick Note: The R changes depending on the Pressure Unit so do not use this number every time.)

Now, plug everything into the equation.

V = (0.08036)(0.08206)(546.15)/(28.0)(1.02)

V = 0.126 L

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3 years ago

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3 years ago

A gaseous mixture consisting of nitrogen, argon, and oxygen is in a 3.5-L vessel at 25C. Determine the number of moles of oxygen

Step2247 [10]

Answer:

Number of moles of oxygen = 0.037 mol

Explanation:

Given data:

Total pressure = 98.5 KPa

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Partial pressure of argon = 50.0 KPa

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Temperature = 25°C (25+273= 298K)

Number of moles of oxygen = ?

Solution:

Total pressure = P(N₂) + P(O₂) + P(Ar)

98.5 KPa = 22.0 KPa +P(O₂) + 50.0 KPa

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P(O₂) = 98.5 KPa - 72.0 KPa

P(O₂) = 26.5 KPa

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n = PV/RT

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3 years ago

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How many molecular of H2O and O2 are present in 8.5g of H2O2 ?

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2H2O+O2--->2H2O2

8.5 gm H2O2=0.25 mole

hence H2O is also 0.25 mole i.e.4.5 gm

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3 years ago

What volume does 2.25g of nitrogen gas, N2, occupy at 273 Celsius and 1.02 atm​

What volume does 2.25g of nitrogen gas, N2, occupy at 273 Celsius and 1.02 atm