Copper(II) nitrate decomposes upon heating to form copper(II) oxide, nitrogen dioxide gas, and oxygen gas. If 1.0 mole of copper(II) nitrate decomposes, how many moles of nitrogen dioxide would be formed?
Cu(NO3)2 --> CuO + NO2 + O2 unbaslanced
now balance
2Cu(NO3)2 --> 2CuO + 4NO2 + O2
has 2 Cu
has 4 N
has 12 O good
so 4 mols NO2 for each 2 mols Cu(NO3)2
so twice as many
so 2
Worst
SO
Copper (II) nitrate is heated to form copper oxide nitrogen dioxide and oxygen gas.
CHEM IS AMAZING.
To determine the number of moles of nitrogen dioxide gas formed, we need to calculate the stoichiometric ratio between copper(II) nitrate and nitrogen dioxide in the chemical equation.
The balanced equation for the decomposition of copper(II) nitrate is:
3 Cu(NO3)2 → 3 CuO + 6 NO2 + O2
According to the balanced equation, for every 3 moles of Cu(NO3)2, we get 6 moles of NO2.
Since we have 1.0 mole of copper(II) nitrate, we can set up a simple stoichiometric ratio to calculate the number of moles of nitrogen dioxide:
(1.0 mole Cu(NO3)2) x (6 moles NO2 / 3 moles Cu(NO3)2) = 2.0 moles NO2
Therefore, if 1.0 mole of copper(II) nitrate decomposes, 2.0 moles of nitrogen dioxide will be formed.