Please show clear steps for this For the equation 2 H_2 (g) + O2 (g) rightarrow

Question

Please show clear steps for this

For the equation 2 H_2 (g) + O2 (g) rightarrow 2 H_2O (g), answer steps a-d to determine the minimum volume of O_2 gas required to react completely with 3.6 L of H_2 gas at STP? What is the mole relationship of H_2 and O_2 from the balanced equation? If l mole of any gas = 22.4 Liters, what is the LITER relationship of H_2 and O_2 in the balanced equation? Can't we also therefore say that 2 liters of H_2 react with 1 liter of O_2? So what is the minimum volume of O_2 gas required to react completely with 3.6 L of H_2 gas at STP?

Explanation / Answer

a.

From the reaction 2 moles of H2 combines with 1mole of O2

b.

2*22.4 lit of H2 conbines with 1*22.4 lit of O2

c.

No

d.

frome the reaction

2*22.4lit of H2 gas combines with 22.4lit of O2

then 3.6Lit of H2 gas combines with 1.8 lit of O2 gas

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