Use the kinetic-molecular theory to explain why gas pressure increases if the te

Question

Use the kinetic-molecular theory to explain why gas pressure increases if the temperature is raised and the volume is kept constant. Explain in 1 - 2 sentences. What is the ideal gas law? What do the different variables represent? What is the effect of pressure (e.g. increased or decreased atmospheric pressure) on a liquid's boiling point? Explain in 1-2 Sentences. The atmospheric pressure on the top of Mt. Everest an altitude of 29,035 ft, is only 265 mmHg. What is the partial pressure of oxygen in the lungs at this altitude, assuming that the mole fraction ot O: in air is 21 %? Report your value in units of mm Hg. What, is the difference between an amorous and a engine so.id? Exp.ain in 1-2 sentence.

Explanation / Answer

3) As temperature increases energy of the gas molecules increases and the collision frequency of the molecules with the walls of the vessel also increases. The increase in the number of collisions increases the gas pressure

4) Ideal gas law states that PV = nRT

P = Pressure

V = Volume

n = number of moles of gas molecule

R = Gas constant

T = Temperature

5) Boiling point is the point at which the water vapor pressure is equal to the atmospheric pressure. Therefore if atmospheric pressure increases boliling point increases and vice versa

6) Partial Pressure of O2 = 0.21 x 265 = 55.65 mm of Hg

7) Amorphous solids do not have a sharp melting point whereas crystalline solids melt at a sharp temperature. Amorphous solids are less rigid whereas crystalline solids are more rigid.

Related Questions

Navigate

• Browse (All)
• Browse U
• Subjects

---

---

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