how much silver nitrate must be measured to yield 1.00g silver?

To determine the amount of silver nitrate needed to yield 1.00g of silver, you would need to know the stoichiometry of the reaction between silver nitrate and silver. The balanced chemical equation is necessary to solve this problem. Since it's not provided, we won't be able to give you an exact answer.

However, I can explain the general process you would need to follow to calculate the required amount of silver nitrate:

1. Write the balanced chemical equation for the reaction. The equation will show the ratio of silver nitrate to silver. For example:
AgNO3 + X --> Ag + Y

2. Find the molar mass of silver the compound AgNO3 and the molar mass of silver Ag.

3. Convert the given mass of silver from grams to moles by using the molar mass of silver.

4. Use the stoichiometry from the balanced equation to determine the mole ratio between silver and silver nitrate. This ratio will allow you to find the number of moles of silver nitrate needed to produce the desired amount of silver.

5. Finally, convert the moles of silver nitrate to grams by multiplying the number of moles by the molar mass of silver nitrate.

By following these steps, you can calculate the amount of silver nitrate required to yield 1.00g of silver, provided you have the balanced chemical equation.

Figure the percent Ag in AnNO3

amountAgNO3*decimalpercent=1g