A vacuum is a space that contains no gas particles. A partial vacuum contains ve

Question

A vacuum is a space that contains no gas particles. A partial vacuum contains very few gas particles. how does the term partial vacuum apply to what you observed with aluminium can? Atmospheric pressure is the force that result from billions upon billions if gas molecules colliding with object. How did the pressure of the atmosphere affect the aluminium can after it had been inverted is the baker? A sample of chlorine gas has a volume of 355mL at 38.5 degree C and 217 kPa of pressure. The temperature lowered to 25.5 degree C and 425 mm Hg. Calculate the now volume in Liters. Mg(s) = 2HCI(aq) rightarrow H_2(g) + MgCI_2(aq) When 50.0 g of hydrochloric acid rescues with excess magnesium metal, what pressure, in kPa, will the hydrogen gas produced event at a temperature of 28 degree C in a container that has a volume of 125 mL? (The ideal gas constant, R = 8.314 L*kPa/mol*K).

Explanation / Answer

4) Pressure is so low that any particles in the space do not affect any processes being carried on, in vaccum
However, partial vaccum is applied to the aluminium can, which means that there is some pressure but it is
   significantly low.
   There is some influence of atmospheric pressure on the inverted beaker, because it experiences some buoyancy forces.
5) V = 355 mL = 0.355 lit ; T = 38.5 oC = 311.65 K ; P = 217 Kpa
   PV = nRT
   217 * 0.355 = n* 8.314 * 311.65
   n = 0.029731 mol of Cl2
   T = 25.5oC = 298.65 K ; P = 425 mmHg = 56.662 Kpa (same no of mol of Cl2 but volume varies)
56.662 * V = 0.029731 * 8.314 * 298.65
V = 1.3028 lit

6) P = ? ; V= 125 mL = 0.125 lit ; T = 28oC = 301.15 K
   50 gm of HCl reacts with magnesium metal ,
   mol of HCl = 50 gm / 36.46094 g/mol = 1.37133 moles of HCl
n= mol of H2 = 1.37133 moles of HCl * ( 1 mol of H2 / 2 mol of HCl ) = 0.685665 mol of H2 are produced
P * 0.125 =  0.685665 * 8.314 * 301.15
P = 13733.9 Kpa

  

     

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