Answer:
Explanation:
1. Molar concentration
Designate chloroform as C and acetone as A.
The molar concentration for C is derived from Moles of C per Litres of solution.
(a) Moles of C
We are assuming there are 0.187 moles of C.
This resolves that step.
(b) Litres of solution
Next, identify 0.813 moles of A.
(i) Mass of each component
(ii) Volume of each component
(iii) Volume of solution
Assuming mixing doesn't alter the total volume.
V = 15.08 mL + 59.70 mL = 74.78 mL
(c) Molar concentration of C
2. Molal concentration of C
Molal concentration is calculated as moles of solute per kilograms of solvent.
Total moles of C = 0.187 mol.
Mass of A = 47.22 g = 0.047 22 kg.
Answer:
No
Explanation:
No. The demonstration in question does not infringe upon the conservation of mass.
The law of conservation of mass states that mass cannot be created or destroyed in a chemical reaction; however, mass can change from one form to another during the process.
In this instance, although the remnants of the paper weigh 0.5 g compared to the original weight of 2.5 g, the ashes and gases produced during combustion account for the missing mass of the paper.
The portion that has been burnt has transformed into other states. If the gas and ashes are adequately contained, they will correspond to the weight of the original paper when added to the remaining paper.
The mixture’s density is 1.57 g/cm³.
Step 1: Determine the mass of the butter.
Step 2: Determine the mass of the sand.
Step 3: Determine the density of the mixture.
Total mass = 0.860 g + 2.28 g = 3.14 g.
Total volume = 1 cm³ + 1 cm³ = 2 cm³
Answer: The correct selection is (b).
Explanation:
The energy required to detach an electron from an atom or ion in its gaseous state is termed ionization energy.
This indicates that a smaller atom necessitates a greater amount of energy to remove its valence electron. The reason for this is that there exists a strong attraction between the nucleus and the electrons in smaller atoms or elements.
Therefore, a significant amount of energy is needed to dislodge the valence electrons.
The electronic configuration for helium is 
. Hence, due to its fully occupied valence shell, it exhibits greater stability.
Consequently, a large amount of energy is needed to remove an electron from a helium atom.
In conclusion, from the choices provided, the ionization energy of helium will be greater than that of the diatomic molecule.
