Answer:
72.3%
Explanation:
The following data were obtained from the question:
Theoretical yield of MgO = 3.43 g
Actual yield of MgO = 2.48g
Percentage yield of MgO =.?
Percentage yield of a reaction can simply be obtained by dividing the actual yield by the theoretical yield multiplied by 100. This is illustrated below:
Percentage yield = Actual yield /Theoretical yield × 100
Thus, we can obtain the percentage yield of MgO as follow:
Theoretical yield of MgO = 3.43 g
Actual yield of MgO = 2.48g
Percentage yield of MgO =.? Percentage yield = Actual yield /Theoretical yield × 100
Percentage yield = 2.48/3.43 × 100
Percentage yield = 72.3%
Therefore, the percentage yield of MgO is 72.3%.
The balanced equation for the above reaction is
2Al + 6H₂O ---> 2Al(OH)₃ + 3H₂
stoichiometry of Al to H₂ is 2:3
number of Al moles reacted - 78.33 g / 27 g/mol = 2.901 mol
according to molar ratio
2 mol of Al forms - 3 mol of H₂
therefore 2.901 mol of Al - forms 3/2 x 2.901 = 4.352 mol
molar volume states that 1 mol of any gas occupies a volume of 22.4 L at STP
if 1 mol occupies 22.4 L
then 4.352 mol occupies - 22.4 L/mol x 4.352 mol = 97.48 L
volume occupied by H₂ is 97.48 L
The answer to your question is b
<span>What all chemical reactions have in common is that energy is released in various forms. Sometimes it's heat or light when there's an explosion, or theres gas and odors or a change in color, or sometimes solids are formed as a deposit. This all show that a reaction occurred and are used as proof.</span>