Ahelium balloon with a volume of 2.75 l and pressure of 1.04 atm and 27 °c flies in the sky and reaches an altitude where the temperature is -15 °c and the pressure is 0.530 atm. calculate the final volume of the balloon

4.64 L

Explanation:

Given Initial pressure (P1) = 1.04 atm , initial volume (V1) = 2.75L and initial temperature (T1) = 27C = 273+27 = 300K

Also given that final pressure (P2) = 0.530 atm , final temperature (T2) = 15C = 273-15 = 258 K and let the final volume be (V2) = V

We know that an ideal gas follows PV=nRT

Here n and R are constant

so

V = 4.64L

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.

answer: they produce more slow than unicellular organisms.