Hello, I really don't understand how to solve this question. Please help! For the reaction P4O10(s) + 6H2O(l)  4H3PO4(aq), what mass of P4O10 must be consumed if 3.71  10^23 molecules of H2O are also consumed?

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Hello, I really don't understand how to solve this question. Please help! For the reaction P4O10(s) + 6H2O(l)  4H3PO4(aq), what mass of P4O10 must be consumed if 3.71  10^23 molecules of H2O are also consumed?

Chemistry
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3.71*10^23 molecules of H2O can be converted to moles of H2O by dividing by Avogadro's number, 6.022*10^23 for every 6 moles of H2O consumed, 1 mole of P4O10 gets consumed, so divide the number of moles of H2O by 6 to find out the number of moles of P4O10 consumed then multiply your result by the molar mass of P4O10 to figure out how many grams are being used
Alright, thank you so much! It makes a lot more sense now!

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