Answer
is: the final pressure of the gas is closest to 3,17 atm.
<span><span>
p</span>₁ =
3,2 atm.</span><span>
T₁ =
310 K.</span><span>
V₁ =
6 L.</span><span>
p₂ = ?</span><span>
T₂ =
410K.</span><span>
V₂ = 8,0 L.</span><span>
<span>Use combined gas law - the volume of amount of gas is proportional to the ratio of
its Kelvin temperature and its pressure.</span><span>
p</span></span><span>₁V₁/T₁ =
p₂V₂/T₂.</span><span>
<span>3,2 atm · 6,0 L ÷ 310 K = p</span>₂ · 8,0 L ÷ 410 K.</span><span>
0,0619 = 0,0195p</span><span>₂.</span><span>
p</span><span>₂ =
3,17 atm.</span>
Answer:
Explanation:
Percent composition is percentage by the mass of element present in the compound.
Given , Mass of sulfur= 32.1 amu
Mass of oxygen = 16.0 amu
Mass of sulfur trioxide 
= 32.1 amu + 3*16.0 amu = 80.1 amu
<u>Answer: </u>The concentration of 
in the solution is 
<u>Explanation:</u>
pH is defined as the negative logarithm of hydrogen ion concentration present in the solution.
![pH=-\log [H^+]](https://tex.z-dn.net/?f=pH%3D-%5Clog%20%5BH%5E%2B%5D)
.....(1)
We are given:
pH of solution = 2.5
Putting values in equation 1, we get:
![2.5=-\log [H^+]](https://tex.z-dn.net/?f=2.5%3D-%5Clog%20%5BH%5E%2B%5D)
![[H^+]=10^{-2.5}](https://tex.z-dn.net/?f=%5BH%5E%2B%5D%3D10%5E%7B-2.5%7D)
![[H^+]=3.16\times 10^{-3}M](https://tex.z-dn.net/?f=%5BH%5E%2B%5D%3D3.16%5Ctimes%2010%5E%7B-3%7DM)
Hence, the concentration of in the solution is
As far as I remember, the needed formula for squaric acid is C4H2O4.
According to this one mole should be 114.06 g., which means we have <span>0.015mol of this acid.
Then we can easly calculate : </span><span>4(0.015) = 0.06 mol for both for Carbon and Oxygen and </span><span>0.03 mol of Hydrogen.
</span><span>To get more clear answer, we multiply by avogadros :
</span><span>6.022 x 10^23. Hope everything is clear! regards</span>
The significant figure is only 1 which is just the number 5. The zeros don't count.
