The experimental density of CO2 at STP is 0.10/0.056=1.78 g/L. The percent error equals to (1.96-1.78)/1.96*100%=9.18%. So the answer is 9.18%.
When the salt AgI dissolves, it dissociates as follows;
AgI --> Ag⁺ + I⁻
molar solubility of salt is the amount of salt that can be dissolved in 1 L of solution
since the ions dissociated are in 1:1 molar ratio, the molar solubility of the ions are equivalent to the molar solubility of the salt.
ksp is the solubility product constant of the salt
ksp = [Ag⁺][I⁻]
ksp = (9.1 x 10⁻⁹ mol/L)²
ksp = 8.28 x 10⁻¹⁷
I think because there is no such quantum shell as -1/2.
Answer:
Determining what data to collect.
Explanation: