To find the temperature at which the volume of the gas would be 0.550 L, given that it is 0.432 L at -20.0 °C, apply Charles’s Law.
The formula is v1/T1 = v2/T2
Known values:
V1 = 0.550 L
T1 = ?
T2 = -20°C + 273 = 253 K
V2 = 0.432 L
Rearranging for T1:
T1 = (V1 × T2) / V2
Calculating:
T1 = (0.55 L × 253) / 0.432 L = 322.11 K or 49.11°C
The direction of the arrow indicates that the bond involving the chlorine atom and the fluorine atom is nonpolar. The fluorine atom pulls the electrons in the bond with greater strength, resulting in the chlorine atom being a little positive.
Explanation:
- The bond formed between chlorine and fluorine displays nonpolar characteristics because both atoms contribute an equal share of electrons within the bond. Examples such as H2, F2, and Cl2 illustrate this concept well.
- Both chlorine and fluorine are electronegative elements, yet fluorine resides above chlorine in the periodic table. Fluorine's position above chlorine gives it a somewhat higher electronegativity compared to chlorine. This explains why fluorine molecules attract electrons more efficiently than chlorine atoms, resulting in chlorine exhibiting a slight positive charge in bonds between Cl and F.
From the provided data, the unknown mixture was composed of salt, salicylic acid, and sand. It is understandable that the student suspected the presence of sand, yet scientific experimentation must verify such assumptions. The test involving salt and salicylic acid reveals that salt dissolves in water, while salicylic acid is only slightly soluble, and sand does not dissolve at all. By introducing the unknown into water, the salt would dissolve first, followed by the partial dissolution of salicylic acid. Heating the mixture could allow for the evaporation of salicylic acid, resulting in the remaining salt. If traces of sand were observed in the dissolved sample, it could suggest contamination.
Answer: The correct option is (1).
Explanation:
Group 16 is the third-from-last column in the periodic table and is known as the oxygen family.
Members of this group include oxygen, sulfur, selenium, tellurium, and polonium.
Elements in Group 16 have 6 valence electrons in their outermost shell.
The electronic configuration of sulfur is 
.
Because sulfur belongs to Group 16, it has 6 valence electrons.
