Question

xperiment 2 Record the pairs of data for pressure (atm) and volume (mL), 2 Points Experiment Data Volume 1/Volume (mL) X-axis Pressure (atm) Y-axis (mL) 150 130 1/150-0.0067 1/130-0.0077 1.00 1.15 L30 I/ 10 /10 D.DIII 14 3.00 Law, pressure is inversely proportional to volume 1. Prepare a graph of the data, with [1/volume] (units-1/mL) on the X-axis and pressure (atm) on the Y-axis. 2. Click the graphing tool in the Latenite Lab assignment section. 3 Points 3. Draw a straight line through the data points, Does your experimental data verify Boyle's Law? Explain. 1 Point 3. What pressure would the gas sample have at a volume of 100 mL? At 250 mL? Remember P1V1-P2V2 1.0x150)-P2(100) Solve for P2 2 Points 1.0 150) P2(250) Solve for P2 2 Points 4. How do the results for butane compare with those for propane? Does each gas obey Boyle's law? 2 Points 5. What are the variables that Robert Boyle's held constant during his experiments on gases? The ideal gas law PVenRT contains all of the variables. Which two remained unchanged during this experiment? R is a constant. 2 Points Hint: Charle's Law. 1 Point 6. In a real lab situation, when the volume available to a gas is decreased, the initial change(s) would be:

Answer 1

Boyle's law 3.5 y= 149.93x R2- 1.5 OL 0.5 85 03 059 ds35 0.005 0.005 0.015 0.025

3.

Yes the experimental data verifies the boyle's law as we get the straight line curve for the plot of P vs 1/V. That too with positive slope which is expected.

P₁V₁ = P₂V₂

(1)(150) = P₂(100)

P₂ = 1.5 atm.

P₁V₁ = P₂V₂

(1)(150) = P₂(250)

P₂ = 150/250

P₂ = 0.6 atm.

4.

If we are considering each gas to be ideal gas then it does not matter which gas you choose boyle's law is applicable to that.

So in this case both the gases will obey the boyle's law.

5. PV = nRT.

R is universal gas constant.

During his experiments on gases he has taken n and T constant. That is he has taken 1 mole of gas and kept it at constant temp. conditions and observed the pressure and volume variation.

nRT = constant.

P = constant / V

So P is inversely proportional to volume.

6.

Real lab situation is constant pressure conditions that is atmospheric pressure. So constant pressure conditions are given by charle's law.

He states that under constant pressure conditions the Volume is directly proportional to temp.

If the volume of available gas decreases that means the temp of gases have fallen down or decreased.