Answer:

ΔG ≅ 199.91 kJ
Explanation:
Consider the reaction:

temperature = 298.15K
pressure = 22.20 mmHg
From, The standard Thermodynamic Tables; the following data were obtained






The equilibrium constant determined from the partial pressure denoted as
can be expressed as :


= 0.045

where;
R = gas constant = 8.314 × 10⁻³ kJ



199.912952 kJ
ΔG ≅ 199.91 kJ
The chemical reaction would be written as:
2HgO = 2Hg + O2
We use this reaction and the amount of the reactant to calculate for the moles of oxygen produced. THen, we use avogadro's number to convert it to molecules. We do as follows:
12.5 g HgO (1 mol / 216.59 g) (1 mol O2 / 2 mol HgO) ( 6.022x10^23 molecules O2 / 1 mol O2 ) = 1.74x10^22 molecules O2 produced
For your experiment, you would need to see decide what your hypothesis is before you design the experiment. If you want to see if the volume of gas changes depending on the container it's in, then you need to set it up depending on what you want to do with the volume.
The manipulated variable would be whatever you change, so if you switch container sizes, that would be the manipulated variable and the responding variable would be the volume of the gas.
I hope this helps!
Answer:
Down below
Explanation:
The following uses nickel(II) chloride
2AgNO3(aq) + NiCl2(aq) ==> Ni(NO3)2(aq) + 2AgCl(s) Molecular
Percentage Yield = (Actual Yield ÷ Theoretical Yield) × 100
∴ if theoretical yield is 26 g, but only 22.0 is recovered from the reaction,
then Percentage Yield = (22 g ÷ 26 g) × 100
= 84.6 %