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How many moles of H2O (molar mass = 18.0 g/mol) are produced when 3.76 moles of C8H18 (molar mass = 114 g/mol)?
How many moles of H2O (molar mass = 18.0 g/mol) are produced when 3.76 moles of C8H18 (molar mass = 114 g/mol) are burned? The balanced equation for the reaction is: 2 C8H18(g) + 25 O2(g)--> 16 CO2(g) + 18 H2O(g)
4 Answers
- 1 decade agoFavourite answer
According to the above equation,
2 moles of C8H18 give 18 moles of H2O
=>3.76 moles of C8H18 give 9*3.76=33.84 moles of H2O
- jacob sLv 71 decade ago
2 C8H18(g) + 25 O2(g)--> 16 CO2(g) + 18 H2O(g)
3.76 moles C8H18(18 H2O/2 C8H18)=33.84 moles H2O
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For the NH4NO3 question, in case you recognize the moles, it is easy to calculate the mass of the quantity. The molar mass of ammonium nitrate is the sum of the molar lots of each and every of the climate in ammonium nitrate. N = 14.00 g/mol H = a million.008 g/mol O = sixteen.00 g/mol There are 2 nitrogens, 4 hydrogens, and 3 oxygens in ammonium nitrate. as a result, the molar mass of ammonium nitrate is: 2(14.00g/mol) + 4(a million.008g/mol) + 3(sixteen.00 g/mol) = 80.032 g/mol Now you will possibly in basic terms multiply the form of moles of the substance cases the molar mass to get the mass. to illustrate, in case you have 2 moles of ammonium nitrate, you will possibly have 2mol(80.032 g/mol) or one hundred sixty grams of ammonium nitrate.
