An experiment requires 47.9 g g of ethylene glycol, a liquid whose density in SI units is 1114 kg/m3 k g / m 3 . Rather than wei
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Answer:
M = 0.011
Half reactions for reduction and oxidation:
oxidation:
HC12H6Cl2O2N + NH+ +2e- = HC12H8Cl2O2N
reduction:
C6H8O6 = C6H6O6 + 2H+ + 2e-
Explanation:
Molarity of the ascorbic acid solution:
Ascorbic acid molar mass = 173.12 g/mol
Then you have to find the mols:
mol = 2g/176,12 =0.011 mol Ascorbic acid.
Use the molarity equation:
Molarity (M) = 0.011 mol / 1 L = 0.011 M
Reactions for the reduction of DCPIP by ascorbic acid:
These reactions have to be balanced by the oxide reduction method.
Because it involves the transfer of electrons from ascorbic acid to the DCPIP.
Remember: when is happens a reduction, also happens oxidation.
To see the reactions watch the images attached.
The first one has the calculus for the molarity of the ascorbic acid solution.
The second one has the reactions for the reduction and oxidation of the compounds.
Answer:
24.525 g of sulfuric acid.
Explanation:
Hello,
Normality (units of eq/L) is defined as:
Since the sulfuric acid is the solute, and we already have the volume of the solution (500 mL) but we need it in liters (0.5 L, just divide into 1000), the equivalent grams of solute are given by:
Now, since the sulfuric acid is diprotic (2 hydrogen atoms in its formula) 1 mole of sulfuric acid has 2 equivalent grams of sulfuric acid, so the mole-mass relationship is developed to find its required mass as follows:
Best regards.
The empirical formula of the substance would be
The constituents of the compound are as follows:
N = 54/201.6 = 26.78% = 26.78/14 = 1.91 moles
H = 15/201.6 = 7.44% = 7.44/1 = 7.44 moles
Cl = 132.6/201.6 = 65.48% = 65.48/35.5 = 1.84 moles
Divide the number of moles by the smallest"
N = 1.91/1.84 = 1
H = 7.44/1.84 = 4
Cl = 1.84/1.84 = 1
Thus, the empirical formula is
More on empirical formula can be found here: brainly.com/question/14044066
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