Copper reacts with nitric acid according to the equation 3Cu(s)+8HNO3-->3CuNO3 +2NO +4H2O.calculate mass of copper nitrate produced when 24g of copper reacts with nitric acid
24g = 0.38 moles Cu
The equation tells you that you will get that many moles of CuNO3
so how many grams is that?
oops. oobleck's answer needs to be modified but not because he did anything wrong. oobleck's work is OK; however, the equation is not balanced so the numbers don't work out. Here is the correctly balanced equation.
3Cu(s) + 8HNO3 --> 3Cu(NO3)2 + 2NO +4H2O.
sorry - I was working with the rare copper mono-carbonate molecule ...
please help
To calculate the mass of copper nitrate produced when 24g of copper reacts with nitric acid, you need to use stoichiometry.
1. Start by determining the molar mass of copper (Cu). The molar mass of copper is 63.55 g/mol.
2. Convert the given mass of copper (24g) to moles by dividing it by the molar mass of copper:
Moles of Cu = 24g / 63.55 g/mol = 0.378 mol
3. Examine the balanced chemical equation:
3Cu(s) + 8HNO3 -> 3CuNO3 + 2NO + 4H2O
4. According to the balanced equation, 3 moles of copper (Cu) react to produce 3 moles of copper nitrate (CuNO3).
5. Calculate the moles of copper nitrate produced by multiplying the moles of copper by the stoichiometric ratio:
Moles of CuNO3 = 0.378 mol Cu * (3 mol CuNO3 / 3 mol Cu) = 0.378 mol CuNO3
6. Finally, calculate the mass of copper nitrate produced by multiplying the moles of copper nitrate by its molar mass:
Mass of CuNO3 = 0.378 mol CuNO3 * (187.57 g/mol CuNO3) = 71.1 g
Therefore, the mass of copper nitrate produced when 24g of copper reacts with nitric acid is 71.1 grams.