Titration is a common method of determining the amount or concentration of an unknown substance. The method is easy to use if the quantitative relationship between two reacting solutions is known. The method is particularly well-suited to acid-base and oxidation-reduction reactions. Titrations are routinely used in industry to analyze products to be sold. Many manufacturers are under strict standards of quality control because their products are sold for public consumption. In this experiment, we will analyze a number of commercial products and, in some cases, test the validity of the information given on their labels and/or the claims made in television commercials. The products to be tested include antacid tablets, vinegar, fruit juice, and household ammonia.
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Answer:
The options are
A.Surroundings get colder and the system decreases in volume.
B.Surroundings get hotter and the system expands in volume.
C.Surroundings get hotter and the system decreases in volume.
D.Surroundings get hotter and the system does not change in volume.
From the Most energy released to the most absorbed , the order is
B. Surroundings get hotter and the system expands in volume.
D. Surroundings get hotter and the system does not change in volume.
C. Surroundings get hotter and the system decreases in volume.
A. Surroundings get colder and the system decreases in volume.
77.
To find the answer u have to subtract the atomic mass from the atomic number.
Answer: c. 179 kJ/mol
Explanation:
According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.
According to Hess’s law, the chemical equation can be treated as algebraic expressions and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.
Given:
(1)
(2)
(3)
(4)
On subtracting eq (1) from eq (2) we have:
-
Hence the enthalpy change for the raection is 179.0 kJ/mol.
