At -32.7 °C, a gas takes up 0.750 mL. What temperature, in °C, would be needed to reduce the volume to half that amount? pleaseee answer correctly

-152.92°C

Explanation:

Initial volume = 0.750 mL

Initial temperature = -32.7 °C (-32.7 + 273.15 K = 240.45 k)

Final temperature = ?

Final volume = 0.750 mL / 2= 0.375 mL

Solution:

The given problem will be solve through the Charles Law.

Mathematical expression:

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume  

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

T₂ = T₁V₂ / V₁

T₂ =  240.45 k  × 0.375 mL / 0.750 mL

T₂ = 90.17 mL.K / 0.750 mL

T₂ = 120.23  K

Temperature in celsius:

120.23  K - 273.15 = -152.92°C

- both b and d.

-since b and d are the closest coastlines then that makes it the most affected.

< 3

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.