A reaction x y has a rate constant of 1.37 hr–1 and is allowed to react for 1.2 hours. if the final concentration of x is 0.21
m, what was the original concentration of x?
1 answer:
The unit measurement of the rate constant is a guide to tell you the rate order. If it's unit is 1/time, then it is a first-order reaction. From the picture attached, the formula to be used would be:
ln[A] = ln[A₀] - kt
ln[0.21] = ln[A₀] - (1.37)(1.2)
Solving for A₀,
A₀= 1.09 M
<em>Hence, the original concentration of X was 1.09 M.</em>
ln[A] = ln[A₀] - kt
ln[0.21] = ln[A₀] - (1.37)(1.2)
Solving for A₀,
A₀= 1.09 M
<em>Hence, the original concentration of X was 1.09 M.</em>
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621.4L
Explanation:
Given parameters:
Initial volume = 547L
Initial temperature = 331K
Final temperature = 376K
Unknown:
Final volume = ?
Solution:
The appropriate gas law to use is the Charles's law.
The Charles's law shows the relationship between the volume and temperature of a gas under constant pressure.
The law states that "The volume of a fixed of a gas varies directly as its absolute temperature if the pressure is constant".
Mathematically;
V₁ is the initial volume
T₁ is the initial temperature
V₂ is the final volume
T₂ is the final temperature
Since the unknown is the final volume, we make it the subject of the expression;
V₂ =
V₂ = 621.4L
learn more:
Boyle's law brainly.com/question/8928288
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