A 4.0L weather balloon is launched from sea level where the temperature is 25°C. It rises to an altitude where the pressure is 0.05atm and the temperature is -75°C. If the balloon has the capacity to expand to a 50 liter volume before bursting, will the balloon survive?

The balloon will not survive.

Explanation:

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

where,

= initial pressure of gas =  1 atm

= final pressure of gas = 0.05 atm

= initial volume of gas = 4.0 L

= final volume of gas = ?

= initial temperature of gas =

= final temperature of gas =

Now put all the given values in the above equation, we get:

As the balloon has the capacity to expand to a 50 liter volume before bursting, it can not survive as it occupies volume higher than 50 L

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

the answer is 1 i believe