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vekshin1
3 years ago
8

Describe a simple chemical test that could be used to distinguish between members of each of the following pairs of compounds (a

) 4-Chlorophenol and 4-chloro-1-methylbenzene (c) 4-Methylphenol and 2,4,6-trinitrophenol (b) 4-Methylphenol and 4-methylbenzoic acid (d) Ethyl phenyl ether and 4-methylphenol

Chemistry
1 answer:
MA_775_DIABLO [31]3 years ago
8 0

Answer:

Explanation:

(A) Phenol gives violet color by complexation with Fe3+ solution . It is best identification...

(B) For b , same phenolic test can be done ...But other esterification is also possibility...

(C) Picric acid has a particular identification test ,  

(D) Here , like the first one , phenolic test with FeCl3 gives violet color for 4-ethylphenol and no color for ethyl phenyl ether...

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3. Svante Arrhenius developed a definition of acids and bases
Alexus [3.1K]

Answer:

Explanation:

BIG OL BEAN

6 0
3 years ago
If you burn 55.6 g of hydrogen and produce 497 g of water, how much oxygen reacted?
tester [92]

Answer:

441.28 g Oxygen

Explanation:

  • The combustion of hydrogen gives water as the product.
  • The equation for the reaction is;

2H₂(g) + O₂(g) → 2H₂O(l)

Mass of hydrogen = 55.6 g

Number of moles of hydrogen

Moles = Mass/Molar mass

          = 55.6 g ÷ 2.016 g/mol

          = 27.8 moles

The mole ratio of Hydrogen to Oxygen is 2:1

Therefore;

Number of moles of oxygen = 27.5794 moles ÷ 2

                                               = 13.790 moles

Mass of oxygen gas will therefore be;

Mass = Number of moles × Molar mass

Molar mass of oxygen gas is 32 g/mol

Mass = 13.790 moles × 32 g/mol

<h3>          = 441.28 g</h3><h3>Alternatively:</h3>

Mass of hydrogen + mass of oxygen = Mass of water

Therefore;

Mass of oxygen = Mass of water - mass of hydrogen

                          = 497 g - 55.6 g

<h3>                           = 441.4 g </h3>
6 0
4 years ago
Read 2 more answers
What type of organism converts nitrogen into a usable form for plants?
inessss [21]
I think it is bacteria
3 0
3 years ago
Read 2 more answers
If you only have 36.5 grams of Potassium Carbonate (K2CO3 molar mass = 138.2 g/mole). How many liters of a 0.52 M solution can y
kirza4 [7]

Answer:

0.508 L of solution.

Explanation:

Always a safe bet to convert to moles:

n= {m \over MM}\\

Where n is moles, m is mass, and MM is molar mass.

Now remember the equation for concentration (molarity):

C={n \over V}

Where C is the concentration, n is moles, and V is volume.

To make this easy, combine the two equations (note n appears in both, so you can do a substitution) and solve for V as the question asks:

C={m \over MM \times V}\\0.52={36.5 \over 138.2 \times V}\\V={36.5 \over 138.2 \times 0.52}\\V=0.508

Therefore we can make 0.508 L of solution.

8 0
3 years ago
What mass of ammonia can be produced if 13.4 grams of nitrogen gas reacted ?
aivan3 [116]

Answer:

If 13.4 grams of nitrogen gas reacts we'll produce 16.3 grams of ammonia

Explanation:

Step 1: Data given

Mass of nitrogen gas (N2) = 13.4 grams

Molar mass of N2 = 28 g/mol

Molar mass of NH3 = 17.03 g/mol

Step 2: The balanced equation

N2 + 3H2 → 2NH3

Step 3: Calculate moles of N2

Moles N2 = Mass N2 / molar mass N2

Moles N2 = 13.4 grams / 28.00 g/mol

Moles N2 = 0.479 moles

Step 4: Calculate moles of NH3

For 1 mol N2 we need 3 moles H2 to produce 2 moles NH3

For 0.479 moles N2 we'll produce 2*0.479 = 0.958 moles

Step 5: Calculate mass of NH3

Mass of NH3 = moles NH3 * molar mass NH3

Mass NH3 = 0.958 moles * 17.03 g/mol

Mass NH3 = 16.3 grams

If 13.4 grams of nitrogen gas reacts we'll produce 16.3 grams of ammonia

3 0
3 years ago
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