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3 years ago

A(n) _______________ compound is a group of atoms held together by chemical bonds.

1 answer:

3 0

Is molecule an answer? It wouldn't let me see all the answers. if it is, molecule is the correct answer. they are held together by a covalent bond, I believe.

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If you digested 25 mg of pure ferrocene in nitric acid and then diluted the resulting solution up to 500 mL with 1% aqueous hydr

Vilka [71]

Answer:

1.345*10⁻⁴ mol/L

15.023 mg/L

Explanation:

The chemical <u>formula of ferrocene</u> is Fe(C₅H₅)₂, thus its molecular weight is:

55.845 g/mol + 10*12g/mol + 10 *1g/mol = 185.845 g/mol

The moles of Fe contained in 25 mg (or 0.025 g) of ferrocene are:

$0.025gFerrocene*\frac{1molFerrocene}{185.845g} *\frac{1mol Fe}{1molFerrocene}=1.345*10^{-4} molFe$

The final volume is 500 mL, or 0.5 L. So the iron concentration in mol/L is:

$\frac{1.345*10^{-4}molFe}{0.5L}= 2.69*10^{-4} mol/L$

We can convert that value into mg/L:

$2.69*10^{-4} \frac{molFe}{L} *\frac{55.845g}{1molFe}*\frac{1000mg}{1g}=15.023 mg/L$

6 0

3 years ago

How many moles of methane are produced when 85.1 moles of carbon dioxide gas react with excess hydrogen gas?

tino4ka555 [31]

Taking into account the reaction stoichiometry, 340.0 moles of methane are produced when 85.1 moles of carbon dioxide gas react with excess hydrogen gas

<h3>Reaction stoichiometry</h3>

In first place, the balanced reaction is:

CO₂ + 4 H₄ → CH₄ + 2 H₂O

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

CO₂: 1 mole
H₄: 4 moles
CH₄: 1 mole
H₂O: 2 moles

<h3>Moles of CH₄ formed</h3>

The following rule of three can be applied: if by reaction stoichiometry 1 mole of CO₂ form 4 moles of CH₄, 85.1 moles of CO₂ form how many moles of CH₄?

$moles of CH_{4} =\frac{85.1 moles of CO_{2}x4 moles of CH_{4} }{1 moles of CO_{2}}$

<u><em>moles of CH₄= 340.4 moles</em></u>

Then, 340.0 moles of methane are produced when 85.1 moles of carbon dioxide gas react with excess hydrogen gas

Learn more about the reaction stoichiometry:

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brainly.com/question/24653699

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6 0

2 years ago

A large balloon contains 233 L of neon at 22.0C and 760. Torr. If the balloon ascends to an altitude where the temperature is -

shepuryov [24]

Answer: The volume in the balloon at the higher altitude is 260 L

Explanation:

The combined gas equation is,

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

where,

$P_1$ = initial pressure of gas = 760 torr

$P_2$ = final pressure of gas = 511 torr

$V_1$ = initial volume of gas = 233 L

$V_2$ = final volume of gas = ?

$T_1$ = initial temperature of gas = $22.0^0C=(22.0+273)K=295K$

$T_2$ = final temperature of gas = $-52.0^0C=(-52.0+273)K=221K$

Now put all the given values in the above equation, we get:

$\frac{760\times 233}{295}=\frac{511\times V_2}{221}$

$V_2=260L$

The volume in the balloon at the higher altitude is 260 L

3 0

3 years ago

The energy entering this system is equal to the energy leaving the system. Based on the law of conservation of energy, how many

Alla [95]

The law of conservation of energy is one of the most commonly used principles in physics and chemistry wherein it states that "Energy<span> can neither be created nor destroyed; rather, it transforms from one form to another." Therefore, the energy entering the system, should be equal to the amount of energy leaving the system.</span>

5 0

4 years ago

How many grams of NH3 can be produced from 2.27mol of N2 and excess H2.

Diano4ka-milaya [45]

The reaction formula of this is N2 + 3H2 = 2NH3. So the ratio of mol number of N2 and NH3 is 1:2. The mol number of NH3 is 2.27*2=4.54 mol. So the mass is 4.54*17=77.18 g.

3 0

3 years ago