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Arte-miy333 [17]
3 years ago
13

What volume will 2.50 mol of hydrogen (H2) occupy at -20.0 °C and 1.5 atm?

Chemistry
1 answer:
svet-max [94.6K]3 years ago
5 0

Answer:

v = 34.62 L

Explanation:

Given data:

Moles of H₂ = 2.50 mol

Temperature of gas = -20.0°C

Pressure of gas = 1.5 atm

Volume of gas = ?

Solution:

Formula:

PV = nRT

P= Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K  

T = temperature in kelvin

Now we will convert the temperature.

-20 + 273 = 253 K

Now we will put the values in formula.

1.5 atm × v = 2.50 mol ×0.0821 atm.L/ mol.K  ×  253 K

1.5 atm × v = 51.93 atm.L

v = 51.93 atm.L/1.5 atm

v = 34.62 L

The volume of hydrogen is 34.62 L.

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What kind of product is formed when a ketone reacts with a grignard reagent followed by protonation?
svet-max [94.6K]

c. a tertiary alcohol; when a ketone reacts with a grignard reagent followed by protonation a tertiary alcohol is formed.

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2 years ago
What is the volume occupied by 4.20 miles of oxygen gas (O2) at STP
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To find volume, derive the equation, it becomes V=nRT/P. Substitute the values. V= 4.20 mol( 0.08205L.atm/mol.K)(273.15K) / 1 atm = 94.13 L. The mole units, atm and K will be cancelled out and L will be the remaining unit which is for volume.

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