At stp how many liters of oxygen are required to react completely with 3.6 liters

1 answer:

3 0

If it is assumed that this reaction is taking place at STP (standard temperature and pressure) then one mole of gas occupies 22.4L

<span>You can then calculate that 3.6L of Hydrogen contains 0.16mol </span>
<span>1mol/22.4L x 3.6L = 0.16mol </span>

<span>Every 2 moles of Hydrogen require 1 mole of oxygen to form water. Therefore half of the number of moles of oxygen are required. </span>
<span>0.16mol/2 = 0.08mol </span>

<span>Again, we know that at STP 1 mol occupies 22.4L </span>
<span>0.08mol x 22.4L/mol = 1.79L of O2 needed. </span>

<span>Also 3.6/2 = 1.8 All ideal gasses will occupy the same ammount of space at STP</span>

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<h2>Hello!</h2>

The answer is:

The new volume will be 1 L.

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To solve the problem, since we are given the volume and the first and the second pressure, to calculate the new volume, we need to assume that the temperature is constant.

To solve this problem, we need to use Boyle's Law. Boyle's Law establishes when the temperature is kept constant, the pressure and the volume will be proportional.

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