Hydrogen cyanide is produced industrially from the reaction of gaseous ammonia, oxygen, and methane.

2 NH₃(g) + 3 O₂(g) + 2 CH₄(g) â 2 HCN(g) + 6 H₂O(g)

If 5.29 â 10³ kg each of NH₃, O₂, and CH₄ are reacted, what mass of HCN and of H₂O will be produced, assuming 100% yield?

HCN g

H₂O g

A solution is prepared by dissolving 14.4 g ammonium sulfate in enough water to make 113.0 mL of stock solution. A 13.20-mL sample of this stock solution is added to 52.30 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.

An 11.7-L sample of gas is determined to contain 0.40 mol N₂. At the same temperature and pressure, how many moles of gas would there be in a 10.-L sample?

Question

Hydrogen cyanide is produced industrially from the reaction of gaseous ammonia, oxygen, and methane.

2 NH₃(g) + 3 O₂(g) + 2 CH₄(g) â 2 HCN(g) + 6 H₂O(g)

If 5.29 â 10³ kg each of NH₃, O₂, and CH₄ are reacted, what mass of HCN and of H₂O will be produced, assuming 100% yield?

HCN	g
H₂O	g

A solution is prepared by dissolving 14.4 g ammonium sulfate in enough water to make 113.0 mL of stock solution. A 13.20-mL sample of this stock solution is added to 52.30 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.

An 11.7-L sample of gas is determined to contain 0.40 mol N₂. At the same temperature and pressure, how many moles of gas would there be in a 10.-L sample?

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