The final concentration after 172 seconds is 1.15 M. To obtain this answer, use the the integrated rate law for the order of reaction. Based on the problem, this is a second order reaction. The units of the rate constant also support that it is a second order reaction.
Further Explanation:
The solution to this problem is straightforward.
- Identify the integrated rate law for the corresponding order of reaction.
- Substitute the given values into the integrated rate law equation.
- Use algebra to solve for the unknown, C(f).
STEP 1: Since the reaction is a second order reaction, the integrated rate law will be:
where:
C(f) is the final concentration
k is the rate constant
t is the time
C(i) is the initial concentration
STEP 2: Plugging in the values given in the problem into the equation, the following equation should be obtained:
STEP 3: Using algebra to solve for C(f):
Since the given values only have 3 significant figures, the final answer must be expressed with 3 significant figures as well.
Therefore,
Learn More
- Learn more about half life brainly.com/question/4318844
- Learn more about first order reaction brainly.com/question/8139015
- Learn more about rate law brainly.com/question/1450796
Keywords: rate law, second order, integrated rate law
Answer: B) The half-life of Co-57 is 10 days
D) After twenty days have elapsed, about 25% of the Co-57 remains.
E) Scientists have an 8 gram sample of Co-57. After thirty days, 1 gram remains.
Explanation: