Answer:
The pressure in that cylinder = 1.12atm
Explanation:
We use general gas law to calculate it. General gas law is gotten by combining Boyle's law, Charles' law and Avogadro's law. Thus
P = nRT/V
Where n = number of moles
R = the gas constant
T is the Temperature, V is the volume and P is the pressure.
Given: T = 319K, V = 24L, R = 0.0821 L.atm/K.mol
The first step is to find n using
n = mass of O2/molar mass of O2
=32.7/32
=1.0219
Now, using P =nRT/V
P = 1.0219 ×0.0821×319÷24
Therefore P = 1.12atm
If he was 30.8% too low, it means that he was at 69.2% of the boiling point needed. So 50o C is 69.2% of total.
In order to know what 100% is, you can divide the number by it's percentage and then multiply it by a hundred.
So: 50/30.8=1.623
1.623*100=162.3
So the correct boiling point of the liquid he was working with in the lab is 162.3 oC
First, 55 g of Hg is 3.65 moles because one mole of Hg has a molar mass of 200.59
Then, the mole ratio of Hg to CaO is 8:4 or 2:1. SO we divide 3.65 by 2 to get 1.82 moles of CaO
This is the same as 102.06 grams because one mole of CaO has a molar mass of 56.0774
Hope this helps!
Ngl didn’t read it so I’m not gonna answer it. Don’t report please just want to ask a question but have to answer two
