SOLUTION: the element europium (EU) exists in nature as two isotopes: (151 EU)with a mass of 150.9196 amu & (153 EU) with a mass of 152.9209 amu. The average mass of EU is 151.96 How do you
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-> SOLUTION: the element europium (EU) exists in nature as two isotopes: (151 EU)with a mass of 150.9196 amu & (153 EU) with a mass of 152.9209 amu. The average mass of EU is 151.96 How do you
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Question 45866: the element europium (EU) exists in nature as two isotopes: (151 EU)with a mass of 150.9196 amu & (153 EU) with a mass of 152.9209 amu. The average mass of EU is 151.96 How do you calculate the relative abundance of the two EU isotopes? X% times 150.9196 (plus) Y% times 152.9209 equals = 151.96. what are the X and Y percentages? And what is the formula to identify the unknowns X and Y? Answer by stanbon(75887) (Show Source):
You can put this solution on YOUR website! How do you calculate the relative abundance of the two EU isotopes? X% times 150.9196 (plus) Y% times 152.9209 equals = 151.96. what are the X and Y percentages?
Let the percentages be respectively x and y, as you have indicated.
EQUATIONS:
1st: x+y=100% = 1
2nd: 150.9196x + 152.9209y = 151.96
Solve this using substitution.
I get x= 48.01% and y=51.99%
Cheers,
Stan H.
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