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ladessa [460]
3 years ago
6

What is the mass, in grams, of 9.21×1024 molecules of methanol

Chemistry
1 answer:
Nina [5.8K]3 years ago
7 0

Answer: 490.02g

Explanation:

9.21x10^2^4 molecules of methanol

9.21x10^2^4molecules(\frac{1mol}{6.022x10^2^3molecules} )(\frac{32.04g}{1mol} )=490.02g

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Nikolay [14]

H-Cl pair of atoms has the most polar bond.

7 0
3 years ago
How many moles are in 1.51x10^26 atoms of xenon (Xe)? Please and thank you :)!!
RoseWind [281]
<h3>Answer:</h3>

251 mol Xe

<h3>General Formulas and Concepts:</h3>

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

  1. Brackets
  2. Parenthesis
  3. Exponents
  4. Multiplication
  5. Division
  6. Addition
  7. Subtraction
  • Left to Right

<u>Chemistry</u>

<u>Atomic Structure</u>

  • Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.

<u>Stoichiometry</u>

  • Using Dimensional Analysis
<h3>Explanation:</h3>

<u>Step 1: Define</u>

[Given] 1.51 × 10²⁶ atoms Xe

[Solve] moles Xe

<u>Step 2: Identify Conversions</u>

Avogadro's Number

<u>Step 3: Convert</u>

  1. [DA] Set up:                                                                                                     \displaystyle 1.51 \cdot 10^{26} \ atoms \ Xe(\frac{1 \ mol \ Xe}{6.022 \cdot 10^{23} \ atoms \ Xe})
  2. [DA] Multiply/Divide [Cancel out units]:                                                         \displaystyle 250.747 \ mol \ Xe

<u>Step 4: Check</u>

<em>Follow sig fig rule and round. We are given 3 sig figs.</em>

250.747 mol Xe ≈ 251 mol Xe

3 0
3 years ago
How many molecules are in 88g of carbon dioxide?
Volgvan
No of moles= 88/44 =2
therefore no. of molecules =

therefore no.of molecules= 12.046*10^23
8 0
3 years ago
Read 2 more answers
For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: O3(g)+2NO2(g)→N2O5(g
zavuch27 [327]

Answer: Rate=k[O_3][NO_2]^2

Explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

O_3(g)+NO_2(g)\rightarrow NO_3(g)+O_2(g)   slow

NO_3(g)+NO_2(g)\rightarrow N_2O_5(g)   fast

To determine the net chemical equation, we will simply add the above two equations, we get:

O_3(g)+2NO_2(g)\rightarrow N_2O_5(g)+O_2(g)

Rate=k[O_3][NO_2]^2

Order with respect to O_3 is 1 and Order with respect to NO_2 is 2.

Thus the rate law will be:  Rate=k[O_3][NO_2]^2

6 0
3 years ago
Question: complete the mechanism for the below oxidation of an alkene with kmno4. draw the missing curved
iren2701 [21]

Mechanism for oxidation of alkene by KMnO₄ is provided in the attached image:

6 0
3 years ago
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