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lozanna [386]
2 years ago
14

Infer Xenon, a nonreactive gas used in strobe lights, is a poor conductor of heat and electricity. Would you expect xenon to be

a metal, a nonmetal, or a
metalloid? Where would you expect it to be on the periodic table? Explain.
Chemistry
1 answer:
lesantik [10]2 years ago
4 0

Mark the lime poor conducter of heat and electricity.

  • Hence it's non metal

Yes why no ,Xenon is already has its secured place in modern periodic table.

  • It belongs to group 18,the Helium family and inert gas group having atomic no Z=54
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Explanation:

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8 0
3 years ago
A variable is something that can never be changed in an experiment. <br> False<br> True
Agata [3.3K]
I’m pretty sure it true
3 0
3 years ago
Determine whether or not each mixture is a buffer. check all that apply. check all that apply. hcl and hf hf and naf hc2h3o2 and
maksim [4K]
Hello!

A buffer is composed of a weak acid and its conjugate base or a weak base and its conjugate acid. From the given list:

HCl and HF: Strong Acid and Weak Acid. NOT BUFFER

HF and NaF: Weak Acid and Conjugate Base. BUFFER

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Have a nice day!
7 0
3 years ago
AV<br> 5. How many grams are in 0.52 moles of H3PO4?
Hoochie [10]

Answer:

50.96g

Explanation:

Given parameters:

Number of moles of H₃PO₄   = 0.52moles

Unknown:

Mass of the compound  = ?

Solution:

To find the mass of the compound:

    Mass  = number of moles x molar mass of H₃PO₄

Molar mass of H₃PO₄ = 3(1) + 31 + 4(16)  = 98g/mol

  Mass  = 0.52 x 98  = 50.96g

3 0
3 years ago
Oxalic acid can remove rust (Fe2O3) caused by bathtub rings according to the reaction Fe2O3(s) - 6H2C2O4(aq) rightarrow 2Fe(C2O4
Katena32 [7]

<u>Answer:</u> The mass of rust that can be removed is 1.597 grams

<u>Explanation:</u>

To calculate the number of moles for given molarity, we use the equation:

\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}     .....(1)

Molarity of oxalic acid solution = 0.1255 M

Volume of solution = 6.00\times 10^2mL = 600 mL = 0.600 L    (Conversion factor:  1 L = 1000 mL)

Putting values in equation 1, we get:

0.100M=\frac{\text{Moles of oxalic acid}}{0.600L}\\\\\text{Moles of oxalic acid}=(0.100mol/L\times 0.600L)=0.06mol

For the given chemical reaction:

Fe_2O_3(s)+6H_2C_2O_4(aq.)\rightarrow 2Fe(C_2O_4)_3^{3-}(aq.)+3H_2O(l)+6H^+(aq.)

By Stoichiometry of the reaction:

6 moles of oxalic acid reacts with 1 mole of ferric oxide (rust)

So, 0.06 moles of oxalic acid will react with = \frac{1}{6}\times 0.06=0.01mol of ferric oxide (rust)

To calculate the mass of rust for given number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Molar mass of rust (ferric oxide) = 159.7 g/mol

Moles of rust = 0.01 moles

Putting values in above equation, we get:

0.01mol=\frac{\text{Mass of rust}}{159.7g/mol}\\\\\text{Mass of rust}=(0.01mol\times 159.7g/mol)=1.597g

Hence, the mass of rust that can be removed is 1.597 grams

5 0
3 years ago
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