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A + 2B+ 3C AB2 C3 Reaction of 6.0 g of ...

`A + 2B+ 3C AB_2 C_3`
Reaction of 6.0 g of A, `6.0 xx 10^(23)` atoms of B, and 0.036 mol of C yields 4.8 g of compound `AB_(2)C_(3)`. If the atomic mass of A and C are 60 and 80 amu, respectively. The atomic mass of B is: (Avogadro number `= 6 xx 10^(23)`)

A

70 amu

B

60 amu

C

50 amu

D

40 amu

Text Solution

Verified by Experts

The correct Answer is:
C
`{:(,A,+,2B,+,3C,rarr,AB_(2)C_(3)),(t = 0,0.1,,1,,0.036,,0):}`
C is limiting regent therefore moles of `AB_(2)C_(3)` will be 0.012.
Mass of 0.012 mol `AB_(2)C_(3)` is 4.8 gm
Mass of 1 mol `AB_(2)C_(3)` is `(4.8)/(0.012) = 400`
Molar mass of `AB_(2)C_(3)` is 400 gm
`A + 2B + 3C = 400 gm`
`60 + 2B + 240 = 400 rArr B = 50`
Atomic mass of B is 50u
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