Answer:
V₂ = 1.41 mL
Explanation:
According to general gas equation:
P₁V₁/T₁ = P₂V₂/T₂
Given data:
Initial volume = 21 mL
Initial pressure = 1 atm
Initial temperature = 10 °C (10 +273 = 283 K)
Final temperature = 12 °C (12 +273 = 285 K)
Final volume = ?
Final pressure = 15 atm
Formula:
P₁V₁/T₁ = P₂V₂/T₂
P₁ = Initial pressure
V₁ = Initial volume
T₁ = Initial temperature
P₂ = Final pressure
V₂ = Final volume
T₂ = Final temperature
Solution:
P₁V₁/T₁ = P₂V₂/T₂
V₂ = P₁V₁T₂/T₁ P₂
V₂ = 1 atm × 21 mL × 285 K / 283 K × 15 atm
V₂ = 5985 atm .mL. K / 4245 K. atm
V₂ = 1.41 mL
CBr4 is larger than CH4, so it has a higher London dispersion, A type of Intermolecular force. Higher force means longer time to
bring the substance to boil,Meaning a higher boil point
According to this formula:
K= A*(e^(-Ea/RT) when we have K =1.35X10^2 & T= 25+273= 298K &R=0.0821
Ea= 85.6 KJ/mol So by subsitution we can get A:
1.35x10^2 = A*(e^(-85.6/0.0821*298))
1.35x10^2 = A * 0.03
A= 4333
by substitution with the new value of T(75+273) = 348K & A to get the new K
∴K= 4333*(e^(-85.6/0.0821*348)
= 2.16 x10^2
Answer:
20.(45)L or about 20.4545L
Explanation:
PV = nRT
Where:
P - pressure
V - volume
n - number of particle moles
R - a constant
T - temperature in K
We can assume the P and n (and definitely R) stay the same, so we infer that
Compound= many parts together therefore bike is the answer
