Answer:
339.2K
Explanation:
Using Charles law equation;
V1/T1 = V2/T2
Where;
V1 = initial volume (L)
V2 = final volume (L)
T1 = initial temperature (K)
T2 = final temperature (K)
According to the information provided in this question,
V1 = 2.97 L
V2 = 3.42 L
T1 = 21.6°C = 21.6 + 273 = 294.6K
T2 = ?
Using V1/T1 = V2/T2
2.97/294.6 = 3.42/T2
Cross multiply
2.97 × T2 = 294.6 × 3.42
2.97T2 = 1007.532
T2 = 1007.532 ÷ 2.97
T2 = 339.236
The final temperature is 339.2K
Answer:
The type of reaction that is occuring is 164.8 kJ.
Answer:
The answer to your question is d. 0.5 M
Explanation:
Data
[A] = 1M
K = 0.5
Concentration of B and C at equilibrium = x
Concentration of A at equilibrium = 1 - x
Equation of equilibrium
k = ![\frac{[B][C]}{A}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BB%5D%5BC%5D%7D%7BA%7D)
Substitution
![0.5 = \frac{[x][x]}{1 - x}](https://tex.z-dn.net/?f=0.5%20%3D%20%5Cfrac%7B%5Bx%5D%5Bx%5D%7D%7B1%20-%20x%7D)
Simplification
0.5 = 
Solve for x
0.5(1 - x) = x²
0.5 - 0.5x = x²
x² + 0.5x - 0.5 = 0
Find the roots x₁ = 0.5 x₂ = -1
There are no negative concentrations so the concentration of A at equilibrium is
[A] = 1 - 0.5
= 0.5 M