An evaluation of R was performed, following the procedure described in this modu

Question

An evaluation of R was performed, following the procedure described in this module. The barometric pressure was 736 torr, the temperature was 295k and volume of hydrogen gas collected was 35.6 mL. The calculated value of R was 82.1 mL atm K^-1 mol^-1.

1) If the syringe volume had been incorrectly read, giving a calculated system volume of 25.6 mL, what would have been the precent error in the calculated valule of R?

2) what is the volume of one mole of hydrogen gas at 273 K and 760 torr?

3) what is the volume of one mole of oxygen gas under the same conditions?

4) What does this suggest concerning the ideal gas law?

5) show Boyle's and Charles' laws may be derived from the ideal gas law?

6) Two moles of an ideal gas originally at 380 torr amd 298 K are compressed at constant temp to 680 torr. Find the initial and final volumes.

Please I need help in these questions :)

Explanation / Answer

1 torr = 0.00131578947 atm

1. first we calculate no. of moles from the given data=

35.6*736*0.00131578947=n*82.1*295

n= 1.4e-3 moles

if 25.6 ml=

25.6*736*0.00131578947=1.4e-3*R*295

R= 59.30 mL atm K^-1 mol^-1

% error = ((59.30-82.1)/82.1)*100 = 27.76%

2. V*760*0.0013=1*82.1*273

V=22.685 litres

3. V*760*0.0013 = 1*82.1*273

V= 22.685 Litres

4. under similar conditions of temperature and pressure,equal volume of gases contain equal no. of moles.

5. boyles law(temperature is constant)

P1*V1=nRT........................1

P2*V2=nRT........................2

dividing 1 by 2,we get

P1*V1=P2*V2

charles law(at constant pressure)

P*V1=nRT1.....................1

P*V2=nRT2......................2

dividing 1 by 2,we get

V1/T1 = V2/T2

6. initial volume=

PV=nRT

380*V*0.0013=2*82.1*298

V=99.05 Litres=V1

P1*V1=P2*V2

380*99.05=680*V2

V2=55.352 Litres

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