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densk [106]
3 years ago
9

Find the number of moles of argon in 452 g of argon.

Chemistry
1 answer:
andrey2020 [161]3 years ago
6 0

Answer: 13.31 moles.

Explanation: So take 452 grams of Argon and multiply by the molar mass of Argon. Your units will cancel out, leaving you with moles of Argon.

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A curium-245 nucleus is hit with a neutron and changes as shown by the equation. Complete the equation by filling in the missing
Lera25 [3.4K]

Try this option:

^{245}_{96}Cm+^1_0n=^{103}_{42}Mo+^{245+1-103-3*1}_{96+0-42-3*0}(X)+3^1_0n;

^{245}_{96}Cm+^1_0n=> ^{103}_{42}Mo+^{140}_{54}(X)+3^1_0n;

^{245}_{96}Cm+^1_0n=> ^{103}_{42}Mo+^{140}_{54}Xe+3^1_0n;

Answer:

^{140}_{54}Xe

8 0
3 years ago
Read 2 more answers
Please help fast...please
RSB [31]

Answer:

Radioactive

Explanation:

hope this helped! :)

5 0
3 years ago
Given: 2H2O2 → 2H2O + O2 structure of H2O2: H–O–O–H Bond Bond Energy (kJ/mol) O–H 459 O=O 494 O–O 142 Based on the given bond en
ICE Princess25 [194]

Answer:

B. - 210 kJ

Explanation:

<em>∵ ΔHrxn = ∑(bond energies)products - ∑(bond energies)reactants.</em>

  • The bond formation in the products releases energy (exothermic).
  • The bond breaking in the reactants requires energy (endothermic).

The products:

  • H₂O contains 2 O-H (- 459 kJ/mol) bonds.
  • O₂ contain 1 O=O (- 494 kJ/mol) bond.

The reactants:

  • H₂O₂ contain 2 O–H (459 kJ/mol) bonds and 1 O–O (142 kJ/mol) bond.

∵ ΔHrxn = ∑(bond energies)products - ∑(bond energies)reactants.

<em>∴ ΔHrxn = [2 (2 x (O–H bond energy) + (1 x (O=O bond energy)] - 2 [(2 x (O–H bond energy) + (1 x (O–O bond energy)] </em>= [2 (2 x - 459 kJ/mol) + (1 x - 494 kJ/mol)] - 2 [(2 x 459 kJ/mol) + (1 x 142 kJ/mol)] = (- 2330 kJ) + (2120 kJ) = <em>- 210 kJ.</em>

5 0
3 years ago
Which is the Lewis structure for H3PO4?
Fed [463]

<u><em>Answer:</em></u>

  • The correct structure of phosphoric acid is A.

<u><em>Explanation</em></u>

  • P should form five covalent bonds. In this strcuture P form three single bond with 3-hydroxyl groups while one single bondformed with oxygen. As oxygen will form two bonds , it carry negative charge, while P should form five bond but here it is forming 4 bonds due to this P has positive charge but overall structure contain neutral charge due to cancellation of positive and negative charges. Beside this, there are 3 H,  Four O and One P according to formula H3PO4.
5 0
4 years ago
If your end product is 200.0 g KMnO4 how much KOH did you start with?
aniked [119]

Answer:

m_{KOH}= 142.0gKOH

Explanation:

Hello there!

In this case, according to the following chemical reaction we found on goo gle as it was not given:

2MnO_2+4KOH+O_2\rightarrow 2KMnO4+2KOH+H_2

Whereas we can see a 2:4 mole ratio of potassium permanganate product to potassium hydroxide reactant with molar masses of 158.03 g/mol and 54.11 g/mol respectively. In such a way, by developing the following stoichiometric setup, we obtain the mass of KOH to start with:

m_{KOH}=200.0gKMnO_4*\frac{1molKMnO_4}{158.03gKMnO_4}*\frac{4molKOH}{2molKMnO_4}  *\frac{56.11gKOH}{1molKOH}\\\\m_{KOH}= 142.0gKOH

Best regards!

8 0
3 years ago
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