Question

How many moles of sodium cyanide (NaCN) would be needed to produce 4.2 moles of sodium sulfate (Na2SO4)?

H2SO4 + 2NaCN → 2HCN + Na2SO4 (4 points)

Answer 1

Answer:

8.4 moles of sodium cyanide (NaCN) would be needed to produce 4.2 moles of sodium sulfate (Na2SO4).

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Answer 2

Given: The given reaction is $H_2SO_4+2NaCN\rightarrow 2HCN+Na_2SO_4$.

To find: We have to find the amount of sodium cyanide (NaCN) that would be needed to produce 4.2 moles of sodium sulfate.

Solution:

The reaction is $H_2SO_4+2NaCN\rightarrow 2HCN+Na_2SO_4$.

In this reaction, one mole of sulfuric acid reacts with two moles of sodium cyanide to form two moles of hydrogen cyanide along with one mole of sodium sulfate.

Here 1 mole of sodium sulfate is formed from two moles of sodium cyanide.

Thus 4.2 moles of sodium sulfate is formed from 2×4.2=8.4 moles of sodium cyanide.

Thus 8.4 moles of NaCN is required.