Normal No Spacing Heading 7 Subtie E Gases Part III. Dalton\'s Law Model 3. Part

Question

Normal No Spacing Heading 7 Subtie E Gases Part III. Dalton's Law Model 3. Partial Pressure Moles of Pressure of Gas Moles of Pressure of Gas B Total Pressure Gas A A (atm) 0.5 0.5 0.0 0.5 1.0 1.0 1.5 Gas B 0 (atm) 0.0 0.5 0.5 1.0 0.5 1.0 1.5 (atm) 0.5 1.0 0.5 1.5 1.5 2.0 3.0 1. n the above model, what occurs to the pressure when the number of moles of A increases? Answer: 2. Is the pressure similarly affected when the moles of B increases? Answer: ?, when Volume and Temperature are held constant, then Since = Where condition 1 can be the pressure and number of moles of A only and the condition 2 can be the pressure and number of moles of gas B. 3. If the pressure of gas A is independent of the pressure of gas B, what can you say about the total pressure in the container? Answer: 4. What is the partial pressure of oxygen in a mixture both nitrogen and oxygen if the partial pressure of nitrogen is 535 mm Hg and the total pressure is 1.2 atm? Answer: English (us)

Explanation / Answer

partial pressure is defined as the pressure exerted by the gas if it alone occupies the entire volume of gas mixture, Partial pressure = mole fraction* total pressure

moles fraction = moles of given component/total moles

so when moles of A increases, mole fraction increases and which in turn increases the partial pressure of the gas. this is true for B as well.

total pressure = sum of partial pressure of individual gases = partial pressure of A + partial pressure of B

For 1st data point total pressure =0+0.5= 0.5 atm

for 2nd data point, total pressure = 0.5+0.5= 1 atm

3. Gvien total pressure = 1.2 atm, 1 atm= 760 mm Hg, total pressure = 1.2*760 =912 mm Hg

partial pressure of nitrogen= 535 mm Hg

total pressure = 912 mm Hg= partial pressure of nitrogen+ parital pressure of oxygen

partial pressure of oxygen= 912-535 =377 mm Hg

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