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Find the mass of silver metal that will react with 2.000 L of 10.00 M nitric acid,...

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xinchaoyo | Student, Grade 11 | Honors

Posted January 16, 2012 at 5:11 PM via web

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Find the mass of silver metal that will react with 2.000 L of 10.00 M nitric acid, according to the equation:

Ag (s) + 2HNO3 (aq) --> AgNO3 (aq) + H2O (l) + NO2 (g)

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ndnordic | High School Teacher | (Level 2) Associate Educator

Posted January 16, 2012 at 9:37 PM (Answer #1)

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First you need to know how many moles of nitric acid you have.
Second, based on step one you can then see how many moles of silver will react based on the balanced chemical equation you have given. That tells you that for every two moles of nitric acid you will need one mole of silver.

Third, convert the number of moles of silver to mass by multiplying the elemental mass of silver times the number of moles of silver you determined.

1. The key is to recognize the relationship between moles, molarity, and volume.

M (molarity) = moles/liters

rearranging, moles = M * L

Use this relationship to find the number of moles of nitric acid.

2.  The number of moles of Ag is 1/2 the answer to step 1.

3. find mass of silver by multiplying the answer from step 2 times atomic mass of silver.

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