What mass of copper (II) nitrate, Cu(NO_3)_2, must be decomposed to produce 1500

Question

What mass of copper (II) nitrate, Cu(NO_3)_2, must be decomposed to produce 1500 g (assume the zeros are significant figures) of copper (II) oxide, CuO? What mass of nitrogen dioxide, NO_2, would be produced by the decomposition of 75.0 g of copper (II) nitrate? How many moles of oxygen would be produced by the decomposition of 75.0 g of copper (II) nitrate? A solution containing 50.0 g of LiOH is mixed with a solution containing 50.0 g of HCl: Which compound is in excess and what mass of LiCl is produced?

Explanation / Answer

Cu(NO3)2 -----> CuO + 2NO2 + O2
1)
moles of CuO produced = mass of CuO / molar mass of CuO
= 1500 / 79.545
= 18.857 mol
moles of Cu(NO3)2 required = moles of CuO = 18.857 mol
mass of Cu(NO3)2 = number of moles * molar mass
= 18.857 mol * 187.56
=3537 g
Answer: 3537 g

2)
mole sof Cu(NO3)2 decomposed = 75.0/187.56 = 0.3999 mol
moles of NO2    produced = 2*0.3999 = 0.7998 mol
mass of NO2 produced = mol*molar mass of NO2
= 0.7998*46
=36.79 g
Answer: 36.79 g

3)
moles of O2 = 0.3999 mol
Answer: 0.3999 mol

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