An oxide of Y has the formula YO. When 1.08g of this oxide is heated strongly, it decomposes completely to give 60.0 cm3 of oxygen, measured at room temperature and pressure. Calculate the relative atomic mass of Y.
(Relative atomic mass of O: 16.0 ;
molar volume of gas at room temperature and pressure= 24.0 dm3)
我想問應該點計
我地chem教左relative atomic mass= a% x Ma + b% x Mb + c% x Mc
同埋one mole=6.02 x10^23 mol -1
但係都係唔識計
請各位幫幫手thx!
chemistry:reactivity of metals
2012-10-14 12:51 am
回答 (1)
2012-10-14 3:13 am
✔ 最佳答案
In gasMolar volume of Oxygen(O2) at RTP=24*1000*21% cm^3 <=(氧氣佔大氣21% 仲有1dm=10cm 1dm^3=1000cm^3 所以要乘1000)
=5040 cm^3
Number of moles of Oxygen given out during the decomposition of YO
=60/5040
=1/84
'.'The ratio of Y(2+) ions : O(2-)=1:1
.'.They have the same number of mole
Let m g be the relative atomic mass of Y
(1/84)m + (1/84)*16=1.08
m+16=90.72
m=74.72
.'.The relative atomic mass of Y is 74.72g .
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