# college chem

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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 -

The slope will be nRT. You will have to use the ideal gas law to derive this.

• college chem -

Thank you but I am not sure what you mean by derive it

• college chem -

I am still very confused

• college chem -

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 -

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.