The weight of aluminum are required to produce 8.70 moles of aluminum chloride is 234.9 g
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What is the use of aluminium chloride ?</h3>
Aluminum chloride is useful for the treatment of palmar, plantar, and axillary hyperhidrosis.
Aluminum chloride has also been reported to be useful in facial and scalp hyperhidrosis
The balanced chemical equation represents the mole ratio in which the chemicals combine.
In this case, illustrates that 2 mol Al produces 2 mol Al Cl₃, hence these 2 chemicals are in a 1:1 ratio.
Thus, to produce 8.70 mol aluminium chloride, it will require 8.70 mol aluminium.
But this quantity of Al has a mass in grams of
m = n × Mr
= 8.70 mol × 27g/mol
= 234.9 g
Hence, The weight of aluminum are required to produce 8.70 moles of aluminum chloride is 234.9 g
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We can express the rate equation in this form:
-r = k A^n B^m
where -r is the rate
k is the rate constant,
A is the concentration of CH3Cl
n is the order with respect to CH3Cl
B is the concentration of H2O
m is the order with respect to H2O
We can solve this by trial and error or by calculus. The first method is easier. The rate constant does not depend on the concentration of the reactant. Assume values of n and m and solve for k in each experiment. The only option that gives really close values of k in each experiment is:
<span>C. CH3Cl: firstorder H2O: second order
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25.0 g.....................................................
Answer : The percent of the carbon−14 left is, 0.242 %
Explanation :
This is a type of radioactive decay and all radioactive decays follow first order kinetics.
To calculate the rate constant, we use the formula :
Now we have to calculate the amount left.
Expression for rate law for first order kinetics is given by :
where,
k = rate constant = 
t = time taken for decay process = 50000 years
a = initial amount or moles of the reactant = 7 g
a - x = amount or moles left after decay process = ?
Putting values in above equation, we get:
The amount left of carbon-14 = 0.0169 g
Now we have to calculate the percent of the carbon−14 left.
Therefore, the percent of the carbon−14 left is, 0.242 %
Answer:
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Explanation:
