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How many moles of P4 would you need to produce 34 g of PH3?

P4(s) + 6 H2(g) → 4 PH3(g)




0.25 mol
0.5 mol
1 mol
4 mol

Respuesta :

PAWTPIE

Molecular weight of P (Phosphorous) = 30.97g/mol

Hydrogen is just 1 g/mol.

How many moles is 34g of PH3?

Get the weight of PH3 (30.97 + (3X1)) = 33.97g/mol

So 34g/33.97g/mol = 1.0009 moles.

I bet for this problem it's easier to round this to 1.

If you look at just the moles in the equation:

P4(s) + 6 H2(g) → 4 PH3(g)

OR

1 + 6 → 4

If 1 (P4) gives us 4 (PH3), what gives us 1 (PH3)?

1/4 = x/1

solve for x

Eduard22sly

The number of mole of P₄ required to produce 34 g of PH₃ is 0.25 mole

How to determine the mole of PH₃

  • Mass of PH₃ = 34 g
  • Molar mass of PH₃ = 31 + (3×1) = 34 g/mol
  • Mole of PH₃ =?

Mole = mass / molar mass

Mole of PH₃ = 34 / 34

Mole of PH₃ = 1 mole

How to determine the mole of P₄ needed

P₄ + 6H₂ —> 4PH₃

From the balanced equation above,

4 moles of PH₃ were produced from 1 mole P₄.

Therefore,

1 mole of PH₃ will be produced from = (1/4) = 0.25 mole of P₄

Thus, 0.25 mole of P₄ is needed for the reaction

Learn more about stoichiometry:

https://brainly.com/question/14735801

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