If 25.0 g of sodium peroxide (Na2O2, MW = 78.0 g/mol) is reacted with 12.1 g of

Question

If 25.0 g of sodium peroxide (Na2O2, MW = 78.0 g/mol) is reacted with 12.1 g of water (H2O, MW = 18.0 g/mol) according to the following thermochemical equation:

What quantity of heat is released (assuming the pressure remains constant)?

If 25.0 g of sodium peroxide (Na2O2, MW = 78.0 g/mol) is reacted with 12.1 g of water (H2O, MW = 18.0 g/mol) according to the following thermochemical equation: What quantity of heat is released (assuming the pressure remains constant)? 2Na2O2(s)+2H2O(I) right arrow 4NaOH(s)+O2(g) delta H= - 126 kJ

Explanation / Answer

2 moles of Na2O2 recat with 2 mole of H2O produce 126 KJ of heat

25/78  moles of Na2O2 react with 12.1/18 mole of H2O

0.3205 moles of Na2O2 react with 0.672 mole of H2O

remaining water = 0.3517 moles

0.3205 moles of Na2O2 react with 0.3205 mole of H2O to produce 0.3205 * 126 /2 KJ of heat

0.3205 moles of Na2O2 react with 0.3205 mole of H2O to produce 20.1915 KJ of heat

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