Hello There! ^_^
Your question: What is the pressure of a fixed volume of hydrogen gas at 38.8°C if it has a pressure of 1.36 atm at 15.0°C..?
Your answer: P1/ T1= P2/ T2
Change C to Kelvin
273+ C= K
38.3+ 273= 311K
15.0+ 273= 288K
2.38/ 288= P2/ 311.3
740.894= 288 (P2)
P2= 2.57 atm.
Thus, you got you answer!
Hope this helps!
C. A person pushing a box across the floor
The reduction in the temperature leads to an automatic decrease in the pressure of the gas inside the he container. This is due to the decreased number of collisions per unit area of the container walls. Pressure law states that at constant volume, the pressure of a fixed mass of a gas is directly proportional to the absolute temperature.
The equation is as follow,
<span> HBr </span>₍aq₎ + H₂O ₍l₎ →
Solution:
HBr being strong acid with Ka value of 1.0 × 10⁹. When HBr is added to water, water acts as a base and HBr acts as a acid. Water picks the proton (H⁺) from HBr and converts into Conjugate acid (H₃O⁺) ahile HBr is converted into Conjugate Base (Br⁻) after loosing proton. The equation for this reaction is as follow,
HBr ₍aq₎ + H₂O ₍l₎ → H₃O⁺ ₍aq₎ + Br⁻ ₍aq₎
Ionic Bonds have a Lower melting and Covalent have higher.
