We developed each of the eponymous, historical gas laws by starting with the Ide

Question

We developed each of the eponymous, historical gas laws by starting with the Ideal Gas equation. By recognizing which variable are being held constant and which variables are changing you can develop each of the historical gas laws (and skip memorizing four separate equations). Each solution you for these problems looked like a one-step unit conversion, too. The Combined Gas Law is a similar to the historical gas laws. If you have a "sample" of gas (constant n), the product of pressure and volume divided by temperature is a constant. As a result, you can calculate changes in pressure or volume when an isolated sample of gas is compressed or cooled. Either calculation is essentially a multi-step unit conversion P_f = P_i times V_i/V_f times T_f/T_i and V_f = V_i times P_i/P_f times T_f/T_i Solve each of the following problems using this type of set up. A pure gas sample with a partial pressure of 165 mm Hg occupies a volume of 135 mL at a temperature of 22.5 degree C. What is the gas sample's pressure when it is transferred into a flask with volume of 252 mL and cooled to 0.0 degree C.

Explanation / Answer

Question 1

apply ideal gas law

initially

P1 = 165 mm Hg, V = 135 mL, T = 22.5°C = 295.5 K

find P2 when

V2 = 252 mL, T2 = 0°C = 273 K

Apply Ideal gas Law ratios

P1V1/T1 = P2V2/T2

P2 = P1*V1/V2 * T2/T1

P2 = 165*135/252 * 273 / (295.5)

P2 = 81.662 mm Hg

the pressure drops since Volume is increased

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.