A compound with an empirical formula of CH2O has a molar
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The chemical reaction is as follows:
Mass of reactant a is 1 g and molar mass is 94 g/mol. Converting mass into number of moles as follows:
Now, 1 mole of reactant a gives 1 mole of product d thus, 0.0106 mol of reactant a gives 0.0106 mol of product d.
Molar mass of product d is 125 g/mol, converting number of moles into mass as follows:
m=n×M=0.0106 mol×125 g/mol=1.33 g
Similarly, molar mass of reactant b is 118 g/mol and mass is 2 g, converting mass into number of moles,
1 mol of reactant b gives 1 mol of product d thus, 0.017 mol will give 0.017 mol of product d.
Converting number of moles into mass as follows:
m=n×M=0.017 mol×125 g/mol=2.12 g
Here, reactant that produces lesser product is limiting reactant and the amount of product it forms is theoretical yield.
Therefore, theoretical yield is 1.33 g.
