using cu+2AgNo3= Cu(No3)2 + 2Ag if you start with 100 grams of copper how many grams of silver can be obtained
To determine the number of grams of silver that can be obtained using the equation "Cu + 2AgNO3 → Cu(NO3)2 + 2Ag," we need to use stoichiometry.
Stoichiometry is a mathematical relationship between reactants and products in a chemical reaction. In this case, the equation tells us that 1 mole of copper (Cu) reacts with 2 moles of silver nitrate (AgNO3) to produce 1 mole of copper nitrate (Cu(NO3)2) and 2 moles of silver (Ag).
To solve this problem, we need to follow these steps:
Step 1: Convert the given mass of copper to moles.
To do this, we need to know the molar mass of copper (Cu), which is approximately 63.55 g/mol. So, using the formula:
moles = mass / molar mass
moles of copper = 100 g / 63.55 g/mol
Step 2: Use stoichiometry to find the moles of silver.
From the balanced equation, we can see that 1 mole of copper reacts with 2 moles of silver (Ag). So, the moles of silver (Ag) produced will be the same as the moles of copper (Cu), i.e., the moles calculated in Step 1.
moles of silver = moles of copper
Step 3: Convert the moles of silver to grams.
To do this, we need to know the molar mass of silver (Ag), which is approximately 107.87 g/mol. Using the formula:
mass = moles x molar mass
mass of silver = moles of silver x molar mass of silver
Substituting the values, we get:
mass of silver = moles of silver x 107.87 g/mol
Therefore, the number of grams of silver that can be obtained can be calculated by multiplying the moles of copper (calculated in Step 1) by the molar mass of silver (107.87 g/mol).