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3 years ago

What mass of CO2 can be produced from the decomposition of 4.8 moles of Fe2(CO3)3?

Chemistry

1 answer:

gavmur [86]3 years ago

7 0

Answer: 633.6 g of $CO_2$ can be produced from the decomposition of 4.8 moles of $Fe_2(CO_3)_3$

Explanation:

The balanced chemical equation for decomposition of $Fe_2(CO_3)_2$ is :

$Fe_2(CO_3)_2\rightarrow Fe_2O_3+3CO_2$

According to stoichiometry :

1 mole of $Fe_2(CO_3)_2$ produce = 3 moles of $CO_2$

Thus 4.8 moles of $Fe_2(CO_3)_2$ will rproduce= $\frac{3}{1}\times 4.8=14.4moles$ of $CO_2$

Mass of $CO_2=moles\times {\text {Molar mass}}=14.4moles\times 44g/mol=633.6g$

Thus 633.6 g of $CO_2$ can be produced from the decomposition of 4.8 moles of $Fe_2(CO_3)_3$

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(a) What is the total volume (in L) of gaseous products, measured at 350°C and 735 torr, when an automobile engine burns 100. g

Anarel [89]

Answer:

Part A

The volume of the gaseous product is $V = 787L$

Part B

The volume of the the engine’s gaseous exhaust is $V_e = 2178 \ L$

Explanation:

Part A

From the question we are told that

The temperature is $T = 350^oC = 350 +273 =623K$

The pressure is $P = 735 \ torr = \frac{735}{760} = 0.967\ atm$

The of $C_8 H_{18} = 100.0g$

The chemical equation for this combustion is

$2 C_8 H_{18}_{(l)} + 25O_2_{(l)} ----> 16CO_2_{(g)} + 18 H_2 O_{(g)}$

The number of moles of $C_8 H_{18}$ that reacted is mathematically represented as

$n = \frac{mass \ of \ C_8H_{18} }{Molar \ mass \ of C_8H_{18} }$

The molar mass of $C_8 H_{18}$ is constant value which is

$M = 114.23 \ g/mole$

So $n = \frac{100 }{114.23} }$

$n = 0.8754 \ moles$

The gaseous product in the reaction is $CO_2_{(g)}$ and water vapour

Now from the reaction

2 moles of $C_8 H_{18}$ will react with 25 moles of $O_2$ to give (16 + 18) moles of $CO_2_{(g)}$ and $H_2 O_{(g)}$

1 mole of $C_8 H_{18}$ will react with 12.5 moles of $O_2$ to give 17 moles of $CO_2_{(g)}$ and $H_2 O_{(g)}$

This implies that

0.8754 moles of $C_8 H_{18}$ will react with (12.5 * 0.8754 ) moles of $O_2$ to give (17 * 0.8754) of $CO_2_{(g)}$ and $H_2 O_{(g)}$

So the no of moles of gaseous product is

$N_g = 17 * 0.8754$

$N_g = 14.88 \ moles$

From the ideal gas law

$PV = N_gRT$

making V the subject

$V = \frac{N_gRT}{P}$

Where R is the gas constant with a value $R = 0.08206 \ L\cdot atm /K \cdot mole$

Substituting values

$V = \frac{14.88* 0.08206 *623}{0.967}$

$V = 787L$

Part B

From the reaction the number of moles of oxygen that reacted is

$N_o = 0.8754 * 12.5$

$N_o = 10.94 \ moles$

The volume is

$V_o = \frac{10.94 * 0.08206 *623}{0.967}$

$V_o = 579 \ L$

No this volume is the 21% oxygen that reacted the 79% of air that did not react are the engine gaseous exhaust and this can be mathematically evaluated as

$V_e = V_o * \frac{0.79}{0.21}$

Substituting values

$V_e = 579 * \frac{0.79}{0.21}$

$V_e = 2178 \ L$

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2 years ago

Identify the base-conjugate acid pair in this balanced equation:

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<h3><u>Answer;</u></h3>

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<h3><u>Explanation;</u></h3>

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NH3 is the base; while NH4+ is the conjugate acid

HNO3 is the acid; while NO3- is the conjugate base

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Answer:

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A ⇌ B

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The rate of forward reaction = |r₁| = k₁ [A]

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Hope this Helps!!!

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oksian1 [2.3K]

Answer:

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Explanation:

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