A container of compressed hydrogen with a fixed volume has a pressure of 13.0 atm at a temperature of 20.0 °C. If its temperature shoots up to 102 °C, what will the pressure be? A. 2.55 atm B. 10.2 atm C. 16.6 atm D. 66.3 atm

P₂ = 16.6 atm

Explanation:

Given data:

Initial pressure = 13.0 atm

Initial temperature = 20.0°C (20+273 = 293 K)

Final temperature = 102.0°C (102+273 =375 K)

Final pressure = ?

Solution:

According to Gay-Lussac Law,

The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.

Mathematical relationship:

P₁/T₁ = P₂/T₂

Now we will put the values in formula:

13.0 atm / 293 K =  P₂/375 K

P₂ = 13.0 atm × 375 K / 293 K

P₂ = 4875 atm. K /293 K

P₂ = 16.6 atm

1) in periodic acid (HIO₄), iodine has oxidation number +7, hydrogen has oxidation number +1, oxygen has -2, compound has neutral charge:
+1 + x + 4 · (-2) = 0.
x = +7.

2) in molecule of iodine (I₂), iodine has oxidation number 0, because iodine is nonpolar molecule.

3) in sodium iodide (NaI), iodine has oxidation number -1, sodium has oxidation number +1:
+1 + x = 0.
x = -1.

4) in iodic acid (HIO₃), iodine has oxidation number +5, hydrogen has oxidation number +1, oxygen has -2, compound has neutral charge:
+1 + x + 3 · (-2) = 0.
x = +5.