No SIM 3:32 PM Not Charging McGraw-Hill Educati Chapter 11 (Gases)-ezto.mheducat

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No SIM 3:32 PM Not Charging McGraw-Hill Educati Chapter 11 (Gases)-ezto.mheducat... × ( Chegg Study l Guide.. Atoms First 2e: Fall 2017 CHEM-1110-W77 General Chemistry 1 Jordan Taylor Chapter 11(Gases) instructions I help Question 21 (of 25) Save & Exit Submit value: 4.00 points 1 out of 3 attempts Be sure to answer all parts. Assistance Check My Work View Hint View Question Show Me Guided Solution Practice This Question Print Question Help Report a Problem A mixture of gases contains 0.320 mol CH4, 0.230 mol C,H6, and 0.290 mol C3Hg. The total pressure is 1.25 atm. Calculate the partial pressures of the gases. (a) CH4 atm (b) C2Ho atm (c) C3Hg atm

Explanation / Answer

n(CH4),n1 = 0.32 mol

n(C2H6),n2 = 0.23 mol

n(C3H8),n3 = 0.29 mol

Total number of mol = n1+n2+n3

= 0.32 + 0.23 + 0.29

= 0.84 mol

Partial pressure of each components are

a)

p(CH4),p1 = (n1*Ptotal)/total mol

= (0.32 * 1.25)/0.84

= 0.476 atm

b)

p(C2H6),p2 = (n2*Ptotal)/total mol

= (0.23 * 1.25)/0.84

= 0.342 atm

c)

p(C3H8),p3 = (n3*Ptotal)/total mol

= (0.29 * 1.25)/0.84

= 0.432 atm

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