a sample of pure air contains 80% N2 10% O2 co2 5% and 5% argon by moles the average molecular weight of sample is
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This % means 80 g H2 and 20 g O2 in 100 g Sol.
80% H2 means moles of H2= 80÷2=40 moles
20% O2 means moles of O2=20÷32=0.625 moles
Total moles in mix.= 40.625 moles
40.625 moles of have mass =100 g
so 1 mole has mass= molecular mass= 100÷40.625=2.46 g
vaibhav1722:
answer is 29.8
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Answer:
29.8 g/mol
Explanation:
As the percentage composition is given, we will simply multiply them with the molecular weight of respective gases and add them together. And then we will divide the result with hundred as we are taking percentages.
Step1: [80*(MW of N2) + 10*(MW of O2) + 5*(MW of CO2) + 5*(MW of Ar)]/100
Step2: [80*28 + 10*32 + 5*44 + 5*40]/100
Step3: [2240+ 320 + 220 + 200]/100
Step4: [2980]/100
So, average molecular weight of this sample of air will we 29.8 g/mol
Hope it helps!!!
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