What mass of copper(II) nitrate would be produced from the complete reaction of 25.1 g of copper, according to the chemical reaction shown below?
Cu + 2 AgNO3 ----> Cu(NO3)2 + 2 Ag
From the equation 1 mole of copper yields 1 mole of the nitrate.
calculate number of moles of copper from
number of moles od Cu = mass/atomic mass of Cu
this will be the same as the number of moles of the nitrate.
Thus mass of nitrate = number of moles of Cu x molecular mass of Cu nitrate.
To determine the mass of copper(II) nitrate (Cu(NO3)2) produced, you need to follow these steps:
1. Write down the balanced chemical equation:
Cu + 2 AgNO3 ----> Cu(NO3)2 + 2 Ag
2. Calculate the molar mass of copper (Cu):
The molar mass of copper (Cu) is 63.55 g/mol.
3. Convert the mass of copper (Cu) given in the question to moles:
Divide the mass of copper (Cu) by its molar mass:
Moles of Cu = Mass of Cu / Molar mass of Cu
Moles of Cu = 25.1 g / 63.55 g/mol
4. Use the stoichiometry of the balanced chemical equation to determine the number of moles of copper(II) nitrate (Cu(NO3)2) produced:
According to the balanced chemical equation, 1 mole of Cu reacts with 1 mole of Cu(NO3)2.
Therefore, the number of moles of Cu(NO3)2 produced is equal to the number of moles of Cu.
5. Convert the number of moles of copper(II) nitrate (Cu(NO3)2) to mass:
Multiply the number of moles of Cu(NO3)2 by its molar mass:
Mass of Cu(NO3)2 = Moles of Cu(NO3)2 × Molar mass of Cu(NO3)2
Now, you have all the necessary steps to calculate the mass of copper(II) nitrate (Cu(NO3)2) produced.