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Paladinen [302]
3 years ago
11

What volume of nitrogen gas at STP would react with 37.2 g of magnesium to produce magnesium nitride

Chemistry
1 answer:
anastassius [24]3 years ago
6 0

Answer:

11.58 L of N₂

Explanation:

We'll begin by calculating the number of mole in 37.2 g of magnesium. This can be obtained as follow:

Mass of Mg = 37.2 g

Molar mass of Mg = 24 g/mol

Mole of Mg =?

Mole = mass /Molar mass

Mole of Mg = 37.2 / 24

Mole of Mg = 1.55 moles

Next, we shall write the balanced equation for the reaction. This is illustrated below:

3Mg + N₂ —> Mg₃N₂

From the balanced equation above,

3 moles of Mg reacted with 1 mole of N₂.

Therefore, 1.55 moles of Mg will react with = (1.55 × 1)/3 = 0.517 mole of N₂

Thus, 0.517 mole of N₂ is need for the reaction.

Finally, we shall determine the volume of N₂ needed for the reaction as follow:

Recall:

1 mole of a gas occupies 22.4 L at STP.

1 mole of N₂ occupied 22.4 L at STP.

Therefore, 0.517 mole of N₂ will occupy = 0.517 × 22.4 = 11.58 L at STP

Thus, 11.58 L of N₂ is needed for the reaction.

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the normal boiling point of ethanol is 78.3 and its molar heat of vaporization is 393. Calculate the vapor pressure of ethanol a
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<u>0.12 atm</u><u> </u><u>vapor pressure</u><u> of ethanol at 45.0 C.</u>

What is vapor pressure in science definition?

  • Vapour pressure is a measure of the tendency of a material to change into the gaseous or vapour state, and it increases with temperature.
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We will use the Clausius-Clapeyron equation,

ln(P2/P1) = dHvap/R[1/T1-1/T2]

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T1 = 30 oC = 30 + 273 = 303 K

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Feed values,

ln(1/P1) = 39300/8.314[1/303 - 1/351.3]

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thus, the vapor pressure at 30° C is 0.12 atm.

Learn more about vapor pressure

brainly.com/question/2510654

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8 0
1 year ago
The activation energy for the gas phase isomerization of cyclopropane is 272 kJ. (CH2)3CH3CH=CH2 The rate constant at 718 K is 2
NikAS [45]

The answer is:

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The explanation:

According to Arrhenius equation:

ln(k₁/k₂) = Ea/R (1/T₂ - 1/T₁)

when K is the rate constant

and Ea is the activation energy

R is the ideal gas constant

T1 & T2 is a temperature at kelvin

when we have:

Ea = 272 KJ = 272000 J

R is the ideal gas constant 8.3145 J/Kmol

K1 = 2.3 x 10^-5 1/s    K2 = ?? that is we need to calculate

T1 = 718 K     T2 =753 K

So by substitution:

ln(k₁/k₂) = Ea/R (1/T₂ - 1/T₁)

㏑(2.3X10^-5/K2) = [272000/8.314](1/753-1/718)

∴ K2 = 1.9 x 10^-4 1/s

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3 years ago
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