Chemistry, 16.03.2020 22:22 fordalolz1553

Problem Page Question Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a flask with of ammonia gas and of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be . Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to significant digits. Clears your work. Undoes your last action. Provides information about entering answers.

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Answer from: xaniawashington

The question is incomplete, here is the complete question:

Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 500 mL flask with 4.8 atm of ammonia gas and 1.9 atm of oxygen gas at 33 degress Celsius.

He then raises the temperature, and when the mixture has come to equilibrium measures the partial pressure of nitrogen gas to be 0.63 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture.

Round your answer to 3 significant digits. Clears your work. Undoes your last action. Provides information about entering answers.

The value of pressure equilibrium constant for the given reaction is 0.132

Explanation:

We are given:

Initial partial pressure of ammonia gas = 4.8 atm

Initial partial pressure of oxygen gas = 1.9 atm

Equilibrium partial pressure of nitrogen gas = 0.63 atm

The chemical equation for the reaction of ammonia and oxygen gas follows:

$4NH_3(g)+3O_2(g)\rightarrow 2N_2(g)+6H_2O(g)$

Initial: 4.8 1.9

At eqllm: 4.8-4x 1.9-3x 2x 6x

Evaluating the value of 'x'

$\Rightarrow 2x=0.63\\\\x=0.315$

So, equilibrium partial pressure of ammonia gas = (4.8 - 4x) = [4.8 - 4(0.315)] = 3.54 atm

Equilibrium partial pressure of oxygen gas = (1.9 - 3x) = [1.9 - 3(0.315)] = 0.955 atm

Equilibrium partial pressure of water vapor = 6x = (6 × 0.315) = 1.89 atm

The expression of K_p for above equation follows:

$K_p=\frac{(p_{H_2O})^6\times (p_{N_2})^2}{(p_{NH_3})^4\times (p_{O_2})^3}$

Putting values in above equation, we get:

$K_p=\frac{(0.63)^2\times (1.89)^6}{(3.54)^4\times (0.955)^3}\\\\K_p=0.132$

Hence, the value of pressure equilibrium constant for the given reaction is 0.132

Answer from: Quest

If a hydrogen atom is neutral, it must also have one electron. an oxygen atom (o) has an atomic number of eight (8). this means a neutral oxygen atom has eight protons and eight electrons. the element actium (ac) has an atomic number of 89, so it has 89 protons and 89 electrons in a neutral atom

Answer from: Quest

What do you mean by that? like the contents? the thc level?

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