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Upon balancing the equation below, how many moles of sodium cyanide are needed to react completely with 3.6 moles of sulfuric acid? H2SO4 + NaCN yields HCN + Na2SO4

2 Answers

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You would need 7.2 moles of sodium cyanide to completely react with 3.6 moles of sulfuric acid
User Palmer Dabbelt
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Step-by-step explanation:

The given chemical equation is as follows.


H_(2)SO_(4) + NaCN \rightarrow HCN + Na_(2)SO_(4)

Number of reactant atoms are as follows.

  • H = 2

  • SO_(4) = 1
  • Na = 1
  • CN = 1

Number of product atoms are as follows.

  • H = 1

  • SO_(4) = 1
  • Na = 1
  • CN = 1

Thus, in order to balance the equation, multiply NaCN by 2 on the reactant side and multiply HCN by 2 on the product side. Therefore, the balanced chemical equation will be as follows.


H_(2)SO_(4) +2NaCN \rightarrow 2HCN + Na_(2)SO_(4)

Hence, we need
2 * 3.6 = 7.2 moles of NaCN to react completely with 3.6 moles of
H_(2)SO_(4).

User Robse
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