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3 years ago

Given the equation below, What is the reducing agent?

Chemistry

1 answer:

Scilla [17]3 years ago

6 0

Answer:

Reducing agent - S

Explanation:

The equation for the reaction is given as;

K2Cr2O3 + H2O + S --> SO2 + KOH + Cr2O3

The balanced equation is given as:

2K2Cr2O7 + 2H2O + 3S → 3SO2 + 4KOH + 2Cr2O3

The reducing agent can be obtained by comparing the oxidation number of the elements. Increase in oxidation number signifies a reducing agent

Reactant - 1

Product - 1

Reactant - +2

Product - +3

Reactant - -2

Product - -2

Reactant - +1

Product - +1

Reactant - O

Product - +4

S has an increase in oxidation number hence it is the reducing agent.

Although Cr has an increase in oxidation number, it occurs as a compound.

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"Calculate the pH during the titration of 30.00 mL of 0.1000 M C3H7COOH(aq) with 0.1000 M LiOH(aq) after 29.9 mL of the base hav

Ivanshal [37]

Answer:

pH = 7.29

Explanation:

<em>Ka of butanoic acid is 1.54x10⁻⁵</em>

To obtain the pH of the solution you must use H-H equation for butanoic acid:

pH = pKa + log₁₀ [C₃H₇COO⁻] / [C₃H₇COOH]

Where pKa is defined as -log Ka = 4.81

Now, you need to find [C₃H₇COO⁻] and [C₃H₇COOH] concentrations (Also, you can find moles of each substance and replace them in the equation.

Butanoic acid reacts with LiOH, producing C₃H₇COO⁻, thus:

C₃H₇COOH + LiOH → C₃H₇COO⁻ + H₂O + Li⁺

Moles of both reactants, C₃H₇COOH and LiOH are:

C₃H₇COOH = 0.0300L ₓ (0.1000mol / L) = 0.003000moles of C₃H₇COOH

LiOH = 0.0299L ₓ (0.1000mol / L) = 0.00299 moles of LiOH.

That means moles of C₃H₇COO⁻ produced are <em>0.00299 moles</em>.

And moles of C₃H₇COOH that remains in solution are:

0.00300 - 0.00299 = <em>0.00001 moles of C₃H₇COOH</em>

Replacing in H-H equation:

pH = pKa + log₁₀ [C₃H₇COO⁻] / [C₃H₇COOH]

pH = 4.81 + log₁₀ [0.00299moles] / [0.00001moles]

7 0

3 years ago

If the azeotropic mixture is 72% perchloric acid by mass, what is the mole percent of water in the azeotrope?

WARRIOR [948]

Answer:

Mole percent of water in azeotrope is 69%

Explanation:

Clearly, the azeotrope consists of water and perchloric acid.

So, 72% perchloric acid by mass means 100 g of azeotrope contains 72 g of perchloric acid and 28 g of water.

Molar mass of water = 18.02 g/mol and molar mass of perchloric acid = 100.46 g/mol

So, 72 g of perchloric acid = $\frac{72}{100.46}mol$ of perchloric acid = 0.72 mol of perchloric acid

Also, 28 g of water = $\frac{28}{18.02}mol$ of water = 1.6 mol of water

Hence total number of mol in azeotrope = (1.6+0.72) mol = 2.32 mol of azeotrope

So, mole percent of water in azeotrope = [(moles of water)/(total no of moles)] $\times 100$ %

Mole percent of water = $\frac{1.6}{2.32}\times 100$ % = 69%

3 0

4 years ago

Please help will mark brainliest.<br><br> there are four questions and a formula

fomenos

Explanation:

1=2 atoms

2=4-n where n is the number of bonds to that carbon

3=10

4=2

7 0

4 years ago

Using chemical equations, show how the triprotic acid H3PO4 ionizes in water. Phases are optional.

castortr0y [4]

Explanation:

H3PO4 is a weak acid so it partially dissociates in water

Ka1

H3PO4 (aq) + H2O(l) <----> H2PO4-(aq) + H3O+ (aq)

Ka2

H2PO4- (aq) + H2O(l) <----> HPO4 2- (aq) + H3O+ (aq)

Ka3

HPO4 2- (aq) + H2O(l) < ---> PO4 3- (aq) + H3O+ (aq)

6 0

3 years ago

What’s the correct full electron configuration for an atom of zinc?

jonny [76]

Answer:

[Ar] 3d¹⁰ 4s²

Explanation:

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4 years ago