1. To balance the equation:
K2Cr2O7 (aq) + 2AgNO3 (aq) → Ag2Cr2O7 (s) + 2KNO3 (aq)
2. This reaction can be classified as a double replacement reaction, also known as a precipitation reaction. This is because the reactants swap their cations and anions to form the products, and one of the products Ag2Cr2O7 precipitates out as a solid.
3. To calculate the theoretical yield of Ag2Cr2O7, we first need to determine the limiting reactant. The limiting reactant is the reactant that is completely consumed and limits the amount of product formed.
To find the limiting reactant, we can compare the moles of the reactants:
Given:
AgNO3: 2.6 g
K2Cr2O7: 1.5 g
To convert grams to moles, we need to know the molar masses:
AgNO3: 169.87 g/mol
K2Cr2O7: 294.19 g/mol
The moles of AgNO3 = (2.6 g / 169.87 g/mol)
The moles of K2Cr2O7 = (1.5 g / 294.19 g/mol)
Next, let's compare the molar ratios between AgNO3 and K2Cr2O7 from the balanced equation:
The ratio is 2:1 (AgNO3: K2Cr2O7)
Using this ratio, we can find the moles of K2Cr2O7 equivalent to the moles of AgNO3:
Moles of K2Cr2O7 = 0.5 * (moles of AgNO3)
Now, compare these moles of K2Cr2O7 to the actual moles of K2Cr2O7. If the actual moles are greater than the calculated moles, the actual moles become the limiting reactant.
4. In this case, the limiting reactant is determined by comparing the actual moles of K2Cr2O7 to the calculated moles of K2Cr2O7. If the actual moles are greater than the calculated moles, K2Cr2O7 becomes the limiting reactant. If the actual moles are less than the calculated moles, AgNO3 becomes the limiting reactant.
Hope this helps! Let me know if you have any further questions.
willkiddhill