Astudent sets up a reaction and calculates a possible yield of 55.9g of silver. if the student preforms the reaction and the mass of actual silver obtained is 42.5g, what is the percent yield?

76.0 %  

Step-by-step explanation:

% yield = (actual yield/theoretical yield) × 100 %

Data:

Actual yield = 42.5 g

Theoretical yield = 55.9 g

Calculation:

% yield = (42.5 g/55.9 g) × 100 %

% yield = 76.0 %  

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"

answer; natural resources;