How was the ideal gas equation, $PV = nRT$, derived?

Md Ariful Islam

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Md Ariful Islam

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You can also derive it 'logically' from 'first principles' - deduce the shape of the following sketch graphs, for instance: volume vs pressure, thermodynamic temperature (in K) vs pressure, volume vs thermodynamic temperature (in K) and number of moles vs pressure. If you use each to deduce the relationship between the different variables, you will find that pressure is proportional to number of moles and to temperature and inversely proportional to volume. Putting this all together, pressure equals a constant times n, times T over V. The constant is found, again experimentally, and is called R, the Universal Gas Constant.

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We have a lab assignment that we haven't had a lecture on yet. It's the Pv=nRT. I had to graph 50 plus atm measurements & K temps on Excel. We are supposed to answer "$ of moles of the gas in the 250mL sealed flask." I do not know where to go next?

So, $PV=nRT$ is the Ideal Gas Law where "P" is the pressure (in the question it should state it. Maybe it says "at STP" or SATP" or just use each...

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Considering the ideal gas law PV=nRT, what is P directly proportional to what variable?

The equation looks like this $PV = nRT$, where $P$ - the pressure of the gas; $V$ - its volume; $n$ - the number of moles of gas; $R$...

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What units are used in the equation pv=nrt?

For the $PV=nRT$ the unit of each term is the following: $P " in "color(green)(atm)$ $V" in "color(red)(L)$ $n" in "color(orange)(mol)$ $R" in" (color(red)(L)*color(green)(atm))/(color(blue)(K)*color(orange)(mol))$ $T" in "color(blue)(K)$

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How would you solve the equation PV = nRT for R?

$"PV=nRT"$ Isolate $"R"$ by dividing both sides of the equation by $("nT")$. $(PV)/(nT)=(cancelnRcancelT)/(cancelncancelT)$ Switch sides. $R=(PV)/(nT)$

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Considering the ideal gas law PV = nRT, what is P directly proportional to?

First, make sure that you have a clear understanding of what directly proportional actually means. In order for two quantities to be directly proportional, you need one to increase...

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How would you derive the ideal gas law PV= nRT using Avogadros law, Boyles law, and Charles law?

According to , $color(red)(v prop1/p" "$when $" "color(green)(T" & "n$ constant. According to Charle's Law, $color(red)(v prop T" "$when $" "color(green)(p" "&" "n$ constant....

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In the equation PV=nRT, what does the R and n stand for?

And thus $n$ is equal to the number of gaseous particles....i.e. which we express in units of moles. And $R$ is the universal gas constant. There are several expressions for...

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I've found the number of moles of each gas (H2 and H2O) using PV = nRT. Now. I need to find the theoretical yield of H at STP. Can you refresh my memory on how to do that? Is it different with gases?

SIDE NOTE In order to make sure that other students can benefit from this as well, I'll solve the problem completely. If you already found the number of moles of...

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In the ideal gas law equation, $PV=nRT$, what is the value of the variable $'R'$?

Chemists typically deal with $"litre"$ quantities of gases, and typically measure $"pressure"$ in units of $"atmospheres"$. Of course, both physicists and chemists tend to use $"degrees Kelvin"$ as units of...

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An ideal gas at constant temperature is confined In an airtight cylinder, and a piston pushes down on the gas in the cylinder. Assuming the gas behaves as an ideal gas during the compression, what effect will this have on the pressure of the ideal gas?

You are compressing a gas. Is the volume going to increase? Is it going to decrease? If you compress the volume of a gas what is going to happen to...

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