A 750-mL sample of hydrogen exerts a pressure of 822 torr at 325 K. What pressure does it exert if the temperature is raised to
475 K at constant volume
1 answer:
Answer:
1.20 × 10³ torr
Explanation:
Step 1: Given data
- Initial pressure (P₁): 822 torr
- Initial temperature (T₁): 325 K
- Final temperature (T₂): 475 K
Step 2: Calculate the final pressure of the gas
Considering the constant volume, if we assume the gas behaves ideally, we can calculate its final pressure using Gay-Lussac's law.
P₁/T₁ = P₂/T₂
P₂ = P₁ × T₂/T₁
P₂ = 822 torr × 475 K/325 K = 1.20 × 10³ torr
You might be interested in
Hi!
I think the oxidation state of all the atoms should change. :)
Hope this helps
Was .08 off its 4.08 like that guy explained
2021 hoped I helped you god bless you
Answer: these are just options, what is the main question, without it, we cannot determine which option is correct, so please repost the question.
Answer:
a
Explanation:
Density is a physical property.
