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Good day.
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The topic is about dalton's law of partial pressure, which states that the partial pressure of all the gases make up the total pressure.
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In this problem, we are given with carbon monoxide, oxygen gas, and carbon dioxide, which is formed from the reaction of the said two gases.
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So first, let us establish balanced chemical equation for the reaction between carbon monoxide, and oxygen gas, which is two moles of carbon monoxide reacts with one more of oxygen gas to form two most of carbon dioxide.
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Suppose initially we have x most or in terms of partial pressure, we have xatm of carbon monoxide and we have yatm of carbon dioxide.
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And before the start of the reaction, we have no carbon dioxide that's formed.
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As the reaction proceeds, the amount of the gases or their partial pressure change.
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Suppose our atm of oxygen gas is consumed, so we say negative r.
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So from the balance equation, for every one mole of oxygen gas, we have to most of carbon monoxide.
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So the change in carbon monoxide will be minus 2r.
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So this minus sign here indicates that the partial pressure or the amount in general decreases as the reaction goes on.
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And since carbon dioxide is a product, it is produced.
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And from the balance equation again, one more of oxygen gas produces two most of carbon dioxide.
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So the change in the amount of carbon dioxide will be 2r.
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At the end of the reaction, what we will get is simply the sum of the sum of the the initial and then the change.
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So at the end of the reaction we expect x minus 2r atm of carbon monoxide, y minus r atm for carbon for oxygen gas, and 2r atm for carbon dioxide...