Answer:
![\boxed{Percentage \ Yield = 47.6 \ percent}](https://img.qammunity.org/2021/formulas/chemistry/middle-school/wfxnapbcg7d05zaa8u1bj1866kmdlj7f38.png)
Step-by-step explanation:
The balanced chemical reaction is
![2Li + 2H_(2)O \ \ \ -> \ \ \ 2LiOH + H_(2)](https://img.qammunity.org/2021/formulas/chemistry/middle-school/lyopivkh7rtknsxhrps7x93lcmfmo2ii58.png)
For the balanced reaction, we've
Lithium = 14 g
Water = 36 g
LiOH = 48 g
Hydrogen gas = 2 g
So,
14 g of lithium = 48 g of lithium hydroxide
And we have:
7.40 g of lithium = x grams of lithium hydroxide
Cross Multiplying,
x grams =
![(48*7.4)/(14)](https://img.qammunity.org/2021/formulas/chemistry/middle-school/ut3nmuu9w5cplsmxipwht8b6bxg025n840.png)
Grams of lithium = 25.4 g of lithium hydroxide
So, Theoretical Yield = 25.4 g of lithium hydroxide
Now, The %age yield:
%age Yield =
![(Actual \ Yield)/(Theoretical \ Yeild ) * 100](https://img.qammunity.org/2021/formulas/chemistry/middle-school/99s0nkh8phqaqiky0m5zhcqydefurnf2nw.png)
%age Yield =
![(12.1)/(25.4) * 100](https://img.qammunity.org/2021/formulas/chemistry/middle-school/tan9zrnqvnmwn5bz9xl4ji1xinf0nzsnz1.png)
%age Yield = 47.6%