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3 years ago

How many grams of carbon dioxide are produced by complete combustion of 5 grams of c5h10

Chemistry

1 answer:

Lemur [1.5K]3 years ago

5 0

Answer:

15.4 g

Explanation:

The reaction that takes place is:

2C₅H₁₀ + 15O₂ → 10CO₂ + 10H₂O

First we convert 5 grams of C₅H₁₀ into moles, using its molar mass:

5 g ÷ 70 g/mol = 0.07 mol C₅H₁₀

Then we convert C₅H₁₀ moles into CO₂ moles, using the stoichiometric coefficients of the reaction:

0.07 mol C₅H₁₀ * $\frac{10molCO_2}{2molC_5H_{10}}$ = 0.35 mol CO₂

Finally we convert 0.35 moles of CO₂ into grams:

0.35 mol CO₂ * 44 g/mol = 15.4 g

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Why might a metallic compound be mistaken for an ionic compound, based on its physical properties?

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Answer:

(D). Both metallic and ionic compounds can conduct electricity when molten. However, only metallic compounds can conduct electricity in a solid state.

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Metallic compound have the ability to conduct electricity. Since they are Metals they have loosely held electrons which can contribute to electricity conduction.

Ionic compound are brittle physically, ionic compound cannot conduct electricity while being in solid state as the ions are held strongly by electrostatic force of attraction, they can only conduct electricity while they are in molten or aqueous state. In molten state they are forming ions, and ions are free to move within the solution and therefore contribute to electricity conduction.

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3 years ago

A 20.00 mL Ba(OH)_2 solution of unknown concentration was neutralized by the addition of 47.67 mL of a 0.1236 M HCl solution. Wr

dalvyx [7]

Answer:

- Balanced chemical reaction:

$2HCl(aq) + Ba(OH)_2(aq) \rightarrow BaCl_2(aq) + 2H_2O(l)$

- Concentration of the initial barium hydroxide solution:

$M_{Ba(OH)_2}=0.1473M$

- Concentrations of barium and chloride ions:

$M_{Ba^{2+}}=0.04353M\\M_{Cl^-}=0.08707M$

Explanation:

Hello,

In this case, the balanced chemical reaction with the proper physical states is:

$2HCl(aq) + Ba(OH)_2(aq) \rightarrow BaCl_2(aq) + 2H_2O(l)$

Moreover, it is convenient to perform the titration analysis in terms of normalities, therefore, HCl's normality becomes equal to its molarity as it is monoprotic (only one hydrogen in its formula), thus, we find barium hydroxide's normality:

$N_{Ba(OH)_2}=\frac{N_{HCl}V_{HCl}}{V_{Ba(OH)_2}}=\frac{0.1236N*47.67mL}{20.00mL}=0.2946N$

Hence, for the molarity, since two hydroxiles are in the barium hydroxide, 2 grams-equivalents are 1 mole, thus, its molarity is:

$M_{Ba(OH)_2}=0.2946\frac{eq-g}{L}*\frac{1mol}{2eq-g}=0.1473\frac{mol}{L}=0.1473M$

Then, after mixing and carry out the neutralization reaction the resulting volume is:

$V_{final}=20.00mL+47.67mL=67.67mL=0.067L$

In addition, the moles of both barium and chloride ions are:

$n_{Ba^{2+}}=0.02L*0.1473\frac{molBa(OH)_2}{L} *\frac{1molBa^{2+}}{1molBa(OH)_2} \\n_{Ba^{2+}}=2.946x10^{-3}mol Ba^{2+}\\\\n_{Cl^-}=0.04767L*0.1236\frac{molHCl}{L} *\frac{1molCl^-}{1molHCl} \\n_{Cl^-}=5.892x10^{-3}mol Cl^-$

Finally, the concentrations of such ions are:

$M_{Ba^{2+}}=\frac{2.946x10^{-3}molBa^{2+}}{0.06767L}= 0.04353M\\M_{Cl^-}=\frac{5.892x10^{-3}molCl^-}{0.06767L}= 0.08707M$

Best regards.

5 0

3 years ago

Read 2 more answers

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charle [14.2K]

The correct answer is B. Platinum is the transition element among the choices. The elements belonging to this group are those having a partially filled d or f subshell. It usually refers to the d-block transition elements of the periodic table.

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