Since the temperature
is a constant, we can use Boyle's law to solve this.<span>
<span>Boyle' law says "at a constant temperature, the
pressure of a fixed amount of an ideal gas is inversely proportional to its
volume.
P α 1/V
</span>⇒
PV = k (constant)<span>
Where, P is the pressure of the gas and V is the
volume.
<span>Here, we assume that the </span>gas in the balloon is an ideal gas.
We can use Boyle's law for these two situations as,
P</span>₁V₁ = P₂V₂<span>
P₁ = 100.0 kPa = 1 x 10⁵ Pa
V₁ =
3.3 L
P₂ =
90.0 x 10³ Pa
V₂ =?
By substitution,
1 x 10⁵ Pa x 3.3 L = 90 x 10³ Pa x V₂</span><span>
V</span>₂ = 3.7 L<span>
</span><span>Hence, the volume of gas when pressure is 90.0 kPa
is 3.7 L.</span></span>
The answer is C which is PbSo
The correct answer is 3) 2CO2(g) ⇄ 2CO(g) + O2(g)
this is the correct one because it is a decomposition reaction and all the number of atoms is equal on both sides.
there are 2 C atoms on both sides.
and 4 O atoms on both sides.
and 1) the atoms numbers are equal on both sides but not correct as it not a
correct number as it has 1/2 O2.
and 2) CO2(g) ⇆ CO(g) + O2
the number of O atoms is not equal on both sides of the equation.
we have 2 O atoms on the left side and 3 O atoms on the right side.
so, this not a balanced equation.
4) also not correct 2CO(g) + O2 ⇆ 2CO2
as it is not a decomposition reaction and the 2CO & O2 are as reactants not products.
so the correct answer is 3) 2CO2(g) ⇆ 2CO(g) + O2(g)
Ionic bonds are a metal and a non metal bond and a covalent bond is two no metals banded together.
