Answer:
Theoretical yield of C6H10 = 3.2 g.
Explanation:
Defining Theoretical yield as the quantity of product obtained from the complete conversion of the limiting reactant in a chemical reaction. It can be expressed as grams or moles.
Equation of the reaction
C6H11OH --> C6H10 + H2O
Moles of C6H11OH:
Molar mass of C6H110H = (12*6) + (1*12) + 16
= 100 g/mol
Mass of C6H10 = 3.8 g
number of moles = mass/molar mass
=3.8/100
= 0.038 mol.
Using stoichoimetry, 1 moles of C6H110H was dehydrated to form 1 mole of C6H10 and 1 mole of water.
Therefore, 0.038 moles of C6H10 was produced.
Mass of C6H10 = molar mass * number of moles
Molar mass of C6H10 = (12*6) + (1*10)
= 82 g/mol.
Mass = 82 * 0.038
= 3.116 g of C6H10.
Theoretical yield of C6H10 = 3.2 g
Answer:
we need to look at what actually happens to reactant molecules during a chemical. in order for the reaction to take place , some or all of the chemical bonds in the reactants must be broken so that the new bonds, those of the products , can form.
The formula is:
frequency * h (Planck's constant) = Energy
So, to find frequency you need just divide energy by the constant:
frequency = (8 * 10^-15 J) / (6.63 * 10^-34 J*s) = 1.2 * 10^19 1/s or 1.2 * 10^19 Hz
Explanation:
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