Copper (II) sulfide is oxidized by molecular oxygen to produce gaseous sulfur tr

Question

Copper (II) sulfide is oxidized by molecular oxygen to produce gaseous sulfur trioxide and solid copper (II) oxide. Write a balanced chemical equation for this reaction. Identify which atoms are being oxidized and which are reduced. Write the two balanced half reactions that make up the reaction and prove that your balanced equation is correct. Write a paragraph analyzing the halif reactions and the balanced equation...what stands out for you? What surprises you? What makes this equation challenging? Look at the half reactions and the balanced equation to answer this part. [10 points] ) and Windows

Explanation / Answer

CuS + O2 -------> SO3 + CuO

oxidation half reaction,

+2-2 0        +6 -2
CuS + O2 -----> SO3

S atom changes its oxidation state from -2 to +6

Total electrons required = 8

Reduction half reaction,

+2-2 0         +2-2
CuS + O2 -----> CuO

O atom chage its oxidation state from 0 to -2

Total electrons required = 2

Balance the two half reactions,

CuS + 3/2 O2 ------> SO3 and CuS + 1/2 O2 -----> CuO

combining two equations for balaced equation,

CuS + 4 O2 ------> SO3 + CuO

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