If a sample of benzene (C6H6) is 91% pure and the combustion of benzene by the reaction has a 54% yield, how much water is produced from 0.49 mol of a sample of impure benzene?

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The reaction for the combustion of benzene (C6H6) is given by the chemical equation: 2C6H6 + 15O2 --> 12CO2 + 6H2O

2 moles of benzene yield 6 moles of water, or each mole of benzene yields 3 moles of water.

The purity of the 0.49 mole of benzene that is burned is 91%. This gives 0.49*0.91 = 0.4459 moles

The yield of the reaction is 54%. Using this the amount of water produced is 0.4459*3*0.51 = 0.6822

Given that the benzene has a purity of 91% and the yield of the reaction is 54%, 0.49 moles of benzene leads to the production of 0.6822 moles of water.

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