Posted by k on Friday, February 1, 2013 at 12:09am.
A researcher explores the ideal gas equation. He measures the pressure of a system at different temperatures ( keeping the volume and moles of the gas constant) and creates a plot of P versus T. What is the slope of the line that results if the volume is 1.0L when 1.0 mol of gas is used in the exploration?

college chem  Devron, Friday, February 1, 2013 at 2:57am
The slope will be nRT. You will have to use the ideal gas law to derive this.

college chem  k, Friday, February 1, 2013 at 7:07am
Thank you but I am not sure what you mean by derive it

college chem  k, Friday, February 1, 2013 at 10:28am
I am still very confused

college chem  Devron, Friday, February 1, 2013 at 5:39pm
Slope intercept form is y=mx+b. The gas law is PV=nRT. The graph is a plot of P vs. T, so we will isolate P on one side of the equal sign and let that be Y and 1/V is our x, since plotting P vs 1/V is the only way to obtain a straight line.
Rearrange, P=nRT/V + 0 is our equation, and since 1/V is our x, then m is equal to nRT our slope. What I did was derive the equation of the line.

college chem  Devron, Saturday, February 2, 2013 at 4:45am
I apologize. Everything that I told you was correct except for the X axis. The X axis is T not V, so starting to where I misstated, slope intercept form is y=mx+b. The gas law is PV=nRT. The graph is a plot of P vs. T, so we will isolate P on one side of the equal sign and let that be Y and T is our x, since plotting P vs T obtains a straight line, rearranging causes the equation of the line to be P=(nR/V)T+ b, where the slope is equal to nR/V, P =Y, and T=X. Once again I apologize, it was late when I was looking at this and it was early when I replied.
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