Name D C 24 How many moles of H PO are produced when 710 g P

Name: D: C 24 How many moles of H, PO, are produced when 71.0 g P,O1o reacts completely to form H, Po, P410(s) + 6H20()- 4H, Po, (ag) When glucose is consumed, it reacts with oxygen, (O2) in the body to produce carbon dioxide, water, and energy. How many moles of carbon dioxide would be produced if 45 g of C, H1, completely reacted with oxygen?

Solution

24) As per the balanced stoichiometric equation,

1 mole P₄O₁₀ = 4 moles H₃PO₄.

Molar mass of P₄O₁₀ = (4*30.9738 + 10*15.9994) g/mol = 187.8928 g/mol.

Mole(s) of P₄O₁₀ corresponding to 71.0 g P₄O₁₀ = (71.0 g)/(187.8928 g/mol) = 0.3779 mole.

Mole(s) of H₃PO₄ produced = (0.3779 mole P₄O₁₀)*(4 mole H₃PO₄/1 mole P₄O₁₀) = 1.5116 mole (ans).

25) Write the balanced chemical equation for the combustion of glucose as

C₆H₁₂O₆ + 9 O₂ ----------> 6 CO₂ + 12 H₂O + Energy

As per the balanced stoichiometric equation,

1 mole C₆H₁₂O₆ = 6 moles CO₂.

Molar mass of CO₂ = (1*12.011 + 2*15.999) g/mol = 44.009 g/mol.

Mole(s) of C₆H₁₂O₆ corresponding to 45 g CO₂ = (45 g)/(44.009 g/mol) = 1.0225 mole.

Mole(s) of CO₂ produced = (1.0225 mole C₆H₁₂O₆)*(6 moles CO₂/1 mole C₆H₁₂O₆) = 6.135 moles (ans).