The chemical equation below shows the reaction between tin (Sn) and hydrogen fluoride (HF).

Sn + 2HF SnF2 + H2

The molar mass of HF is 20.01 g/mol. How many moles of Sn are required to react with 40 g of HF?

Question

The chemical equation below shows the reaction between tin (Sn) and hydrogen fluoride (HF).

Sn + 2HF  SnF2 + H2

The molar mass of HF is 20.01 g/mol. How many moles of Sn are required to react with 40 g of HF?

jfraser · Answer

since the molar mass of HF is 20g, and they tell you to react 40g of HF, how many MOLES of HF are you starting with?

anonymous · Answer

20?

jfraser · Answer

each mole of HF weigh 20g. It tells you to use 40g. How many moles is 40g, if each mole weighs 20g?

anonymous · Answer

2 mole

jfraser · Answer

yes, 2 moles. Now, the balanced reaction tells you what the mole ratio of the reactants is going to be. When 2 moles of HF are used, how many moles of Sn are also used?

anonymous · Answer

1 Mole

jfraser · Answer

yes, 1 mole. That's it, problem solved\