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alexdok [17]
3 years ago
9

3Al + 3NH4ClO4 → Al2O3 + AlCl3 + 3NO + 6H2O How many moles of AlCl3 are produced?

Chemistry
2 answers:
zhuklara [117]3 years ago
7 0

Answer: 1 mol of AlCl_3 will be produced from this reaction.

Explanation: Reaction follows,

3Al+3NH_4ClO_4\rightarrow Al_2O_3+AlCl_3+3NO+6H_2Oc

As seen from the balanced chemical equation above, we get

For every 3 moles of Aluminium and 3 moles of NH_4ClO_4, 1 mole of Al_2O_3 is formed.

For every 3 moles of Aluminium and 3 moles of NH_4ClO_4, 1 mole of AlCl_3 is formed.

For every 3 moles of Aluminium and 3 moles of NH_4ClO_4, 3 moles of NO is formed.

For every 3 moles of Aluminium and 3 moles of NH_4ClO_4, 6 moles of H_2O is formed.

Kay [80]3 years ago
7 0

The answer is 746 moles of water are produced from 373 moles of Al.

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bagirrra123 [75]
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3 0
3 years ago
Read 2 more answers
An electric range burner weighing 699.0 grams is turned off after reaching a temperature of 482.0°C, and is allowed to cool down
jasenka [17]

Answer:

0.42 J/gºC

Explanation:

We'll begin by calculating the heat energy used to heat up the water. This can be obtained as follow:

Mass (M) of water = 560 g

Initial temperature (T₁) = 22.7 °C

Final temperature (T₂) = 80.3 °C.

Specific heat capacity (C) of water = 4.18 J/gºC

Heat (Q) absorbed =?

Q = MC(T₂ – T₁)

Q = 560 × 4.18 (80.3 – 22.7)

Q = 2340.8 × 57.6

Q = 134830.08 J

Finally, we shall determine the specific heat capacity of the burner. This can be obtained as follow:

Mass (M) of burner = 699 g

Initial temperature (T₁) = 482.0°C

Final temperature (T₂) = 22.7 °C

Heat (Q) evolved = – 134830.08 J

Specific heat capacity (C) of the burner =?

Q = MC(T₂ – T₁)

–134830.08 = 699 × C (22.7 – 482.0)

–134830.08 = 699 × C × –459.3

–134830.08 = –321050.7 × C

Divide both side by –321050.7

C = –134830.08 / –321050.7

C = 0.42 J/gºC

Therefore, the specific heat capacity of the burner is 0.42 J/gºC

8 0
2 years ago
DNA contains which sugar molecule?
pishuonlain [190]

dna contains phosphate

3 0
3 years ago
Balance 6Sb +6Cl2– 6SbCl3
labwork [276]

<u>Answer:</u>

<u>Balancin</u>g is making the number of atoms of each element same on both the sides  (reactant and product side).

To find the number of atoms of each element we multiply coefficient and the subscript  

For example 5 Ca_1 Cl_2 contains

5 × 1 = 5,Ca atoms and

5 × 2 = 10, Cl atoms

If there is a bracket in the chemical formula

For example 3Ca_3 (P_1 O_4 )_2 we multiply coefficient \times subscript \times number outside the bracket.......... to find the number of atoms  

(Please note: 3 is the coefficient, and if there is no number given then 1 will be the coefficient )

So

3 × 3 = 9, Ca atoms  

3 × 1 × 2 = 6, P atoms  

3 × 4 × 2 = 24, O atoms are present.

So

Let us balance the equation given

1Sb +1Cl_2 > 1SbCl_3

(Unbalanced)

Reactant side - Number of atoms of each element - Product side

1  - Sb - 1

2 - Cl - 3  

So we have on the product side odd number of Cl to convert to even number, multiply SbCl_3 by 2

The equation changes to

1Sb +1Cl_2> 2SbCl_3

Reactant side - Number of atoms of each element - Product side

1  - Sb - 2

2 - Cl - 6

Multiplying Sb by 2 and Cl_2

2Sb +3Cl_2> 2SbCl_3

The equation is balanced now!!!!  

Reactant side - Number of atoms of each element - Product side

2  - Sb - 2

6 - Cl - 6

Balanced.

4 0
2 years ago
The reaction H2SO4 + 2 NaOH -&gt; Na2SO4 + 2H2O applied to an acid-base tritration. The equivalence point occurs when 26.66 mL o
bazaltina [42]
We make use of ratios to solve this question.
            moles NaOH = c · V = 0.1923 mmol/mL · 26.66 mL = 5.126718 mmol
            moles H2SO4 = 5.126718 mmol NaOH · 1 mmol H2SO4 / 2 mmol NaOH = 2.563359 mmol
Hence
            [H2SO4]= n/V = 2.563359 mmol / 42.45 mL = 0.06039 M
The answer to this question is  [H2SO4] = 0.06039 M

8 0
3 years ago
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