Question

How many moles of carbon are produced when 1745 g of glucose decomposes according to the following equation? C6H12O6 → 6C 6H2O

Answer 1

When 1745 g of glucose decomposes, the conversion of grams to moles using the molar mass of glucose (180.16 g/mol) and the stoichiometry of the reaction results in the production of 58.116 moles of carbon.

Step-by-step explanation:

To determine how many moles of carbon are produced when 1745 g of glucose decomposes, first we need to convert grams of glucose to moles using the molar mass of glucose which is 180.16 g/mol. The balanced chemical equation is C6H12O6 → 6C + 6H2O.

Using the molar mass of glucose (180.16 g/mol), you calculate the moles of glucose in 1745 g:

• 1745 g glucose * (1 mol glucose / 180.16 g) = 9.686 moles of glucose

According to the equation, 1 mole of glucose yields 6 moles of carbon. Therefore, you can use this ratio to calculate the moles of carbon produced:

• 9.686 moles of glucose * (6 moles of carbon / 1 mole of glucose) = 58.116 moles of carbon

So, when 1745 g of glucose decomposes, 58.116 moles of carbon are produced.

Answer 2

C6H12O6 -------> 6 C + 6 H20 moles C6H12O6 = ( 1745 g ) / ( 180 g/mol ) = 96.94 mol C6H12O6 mol C produced = ( 96.94 mol C6H12O6 reacted ) ( 6 mol C made / mol C6H12O6 reacted ) mol C produced = 58.17 moles C produced <----------------------- Hope I Helped You!!! :-) Have A Good Day!!!