STP conditions imply a temperature of 273.15 K and a pressure of 100 kPa. When tose conditions are met, 1 mole of any ideal gas will have a volume of 22.7 L. So, if 1 mole occupies a volume of 22.7 L, 2 moles will occupy a volume twice as big. Likewise, 0.5 moles will occupy half the volume 1 mole occupies.
Answer:
Final volume is 3.50L
Explanation:
It is possible to find volume of a gas using combined gas law:

<em>Where P is pressure, V is volume and T is temperature of 1: initial state and 2: final state</em>
If initial state of the gas is:
1.75L of a gas is at 700K and is under 250kPa of pressure
And final state is:
298K and 53.2kPa.
Replacing:

0.625L = 0.1785*V₂
<em>3.50L = V₂</em>
Thus, <em>final volume is 3.50L</em>
The answer for this question would be 150
The molecular mass of
is: 1·1 + 1·14.01 + 2·16 = 47.01 g/mol.
Now we can convert the mass into mol of
:
