Lookup the atomic weights of oxygen and hydrogen.
Atomic weight oxygen = 15.999
Atomic weight hydrogen = 1.00794
Calculate molar masses
Molar mass O2 = 2 * 15.999 = 31.998 g/mol
Molar mass H2O = 2 * 1.00794 + 15.999 = 18.01488 g/mol
Now determine how many moles of O2 you have
2.1 g / 31.998 g/mol = 0.065629102 mol
Balance the equation so you get as the balanced equation,
2 C4H6(g) + 11 O2(g) → 8 CO2(g) + 6 H2O(g)
Looking at the balanced equation, for every 11 moles of O2 consumed, 5 moles of H2O are produced. So divide the number of moles of O2 you have by 11, then multiply by 5, giving:
0.065629102 mol / 11 * 5 = 0.02983141 mol
And finally, multiply by the molar mass of H2O, so
0.02983141 mol * 18.01488 g/mol = 0.53740927 g
Round the results to 2 significant figures getting 0.54 g</span>
The balanced equation that illustrates the reaction is: 2C4H6 + 11O2 ......> 8CO2 + 6H2O
number of moles = mass / molar mass number of moles of oxygen = 2.1 / 32 = 0.065625 moles
Now, from the balanced equation, we can note that: 11 moles of oxygen are required to produce 6 moles of water. Therefore: 0.065625 moles of oxygen will produce: (0.065625*6) / 11 = 0.03579 moles of water
number of moles = mass / molar mass mass = number of moles * molar mass mass of water = 0.03579 * 18 = 0.644 grams
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