What are the theoretical molar ratio values for Ag:Cu and Ag:AgNO3? Compare these values to the values you got in your experiment and compute a percent error for your work.

To determine the theoretical molar ratio values, we need to know the balanced chemical equations for the reactions involving Ag:Cu and Ag:AgNO3.

For Ag:Cu:
The balanced chemical equation for the reaction between silver (Ag) and copper (Cu) is:
2Ag + Cu -> 2Ag + Cu

The molar ratio in this reaction is 2:1, indicating that for every 2 moles of Ag, 1 mole of Cu is required.

For Ag:AgNO3:
The balanced chemical equation for the reaction between silver (Ag) and silver nitrate (AgNO3) is:
Ag + AgNO3 -> 2Ag + NO3

The molar ratio in this reaction is 1:1, meaning that for every 1 mole of Ag, 1 mole of AgNO3 is required.

Next, let's compare these theoretical molar ratios with the values obtained in your experiment. To do this, you need to determine the actual molar ratios obtained from your experimental data.

Once you have the actual molar ratios, you can calculate the percent error using the formula:
Percent Error = ((|Theoretical Value - Experimental Value|) / Theoretical Value) * 100

To compute the percent error, subtract the theoretical molar ratio value from the experimental molar ratio value (using absolute values to eliminate any negative signs), divide the difference by the theoretical value, and then multiply by 100 to get the percentage.

Remember to substitute the correct values for the theoretical and experimental molar ratios in the formula to calculate the percent error.