The volume will be one third of the original volume of an ideal gas.
Boyle’s law depicts the relationship between the pressure ,volume and the temperature of a gas. Boyle’s law states that the pressure of a gas is inversely proportional to its volume at a constant temperature.
P ∝ 1 / V
Or, PV = k
When the temperature is kept constant.
According to the question, when the pressure is increased from 2 atm to 6 atm , the pressure is increases thrice ,hence the volume will decrease three times simultaneously of the original volume of 1 mol of an ideal gas.
The equation of the Boyle’s law is; P1V1 = P2V2
Learn more about Boyle’s law here:
brainly.com/question/1437490
#SPJ4
<span>the K and Cl are 1:1 .. the problem is in the O .. you have 3
(left side) and 2 (right side) .. you multiply the O2 on the right by 3 ..
KClO3 ---> KCl + 3 O2
and now you have 6 O on the right and 3 on the left .. so you multiply the KClO3 by 2 ..
2 KClO3 ---> KCl + 3 O2
now you have 6 O on both sides .. now balance the K and Cl by multiplying KCl on the right by 2 ..
2 KClO3 ---> 2 KCl + 3 O2</span><span>
</span>
Answer:
-152.92°C
Explanation:
Initial volume = 0.750 mL
Initial temperature = -32.7 °C (-32.7 + 273.15 K = 240.45 k)
Final temperature = ?
Final volume = 0.750 mL / 2= 0.375 mL
Solution:
The given problem will be solve through the Charles Law.
Mathematical expression:
V₁/T₁ = V₂/T₂
V₁ = Initial volume
T₁ = Initial temperature
V₂ = Final volume
T₂ = Final temperature
Now we will put the values in formula.
V₁/T₁ = V₂/T₂
T₂ = T₁V₂ / V₁
T₂ = 240.45 k × 0.375 mL / 0.750 mL
T₂ = 90.17 mL.K / 0.750 mL
T₂ = 120.23 K
Temperature in celsius:
120.23 K - 273.15 = -152.92°C
"Caesium" is the strongest reducing agent in Periodic table.
Hope this helps!
Answer:
sickness.
Explanation:
some bacterium cause sickness, kike a stomach bug.
