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monitta
4 years ago
15

Nitrogen gas (N₂) reacts with hydrogen gas (H₂) to form ammonia (NH₃). At 200°C in a closed container, 1.0 atm of nitrogen gas i

s mixed with 2.0 atm of hydrogen gas. At equilibrium, the total pressure is 1.9 atm. Calculate the partial pressure of hydrogen gas at equilibrium.
Chemistry
1 answer:
Pie4 years ago
8 0

Answer:

The partial pressure of hydrogen gas at equilibrium is 1.26 atm

Explanation:

Let's use the molar fraction to solve this:

Molar fraction = Moles of gas / Total moles

Molar fraction = Gas pressure / Total pressure

Without equilibrium, we can think that the total system pressure is the sum of the partial pressures of each gas.

1 atm N₂ + 2 atm H₂ = 3 atm

Molar fraction for H₂ = 2 atm / 3atm → 0.66

Let's replace the molar fraction in equilibrium

Gas pressure / 1.9 atm = 0.66

Gas pressure = 1.26atm

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In the given question according to the information the process of polymerization is an addition polymerization.

<h3>What is polymerization?</h3>

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In the polymerization of polyethene the small repeating molecule is ethene and in this process product formed due to the addition process to the double bond of the ethene.

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Hence given process is an addition polymerisation.

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<h3>Further explanation</h3>

Given

the structure of the alkanes

Required

match the image to the name

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General formula:

\large {\boxed {\bold {C_nH_2n + 2}}}

If we look at the picture, we define the black atom as Carbon and the branch is Hydrogen

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