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andriy [413]
3 years ago
13

Steam reforming of methane ( CH4 ) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the sta

rting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 200.mL flask with 2.4 atm of methane gas and 3.9 atm of water vapor at 46.0°C. She then raises the temperature, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 6.5 atm. Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture.
Chemistry
1 answer:
Hatshy [7]3 years ago
5 0

<u>Answer:</u> The pressure equilibrium constant for the reaction is 1473.8

<u>Explanation:</u>

We are given:

Initial partial pressure of methane gas = 2.4 atm

Initial partial pressure of water vapor = 3.9 atm

Equilibrium partial pressure of hydrogen gas = 6.5 atm

The chemical equation for the reaction of methane gas and water vapor follows:

                        CH_4+H_2O\rightleftharpoons CO+3H_2

<u>Initial:</u>               2.4       3.9

<u>At eqllm:</u>        2.4-x    3.9-x        x       3x

Evaluating the value of 'x':

\Rightarrow 3x=6.5\\\\x=2.167

So, equilibrium partial pressure of methane gas = (2.4 - x) = [2.4 - 2.167] = 0.233 atm

Equilibrium partial pressure of water vapor = (3.9 - x) = [3.9 - 2.167] = 1.733 atm

Equilibrium partial pressure of carbon monoxide gas = x = 2.167 atm

The expression of K_p for above equation follows:

K_p=\frac{p_{CO}\times (p_{H_2})^3}{p_{CH_4}\times p_{H_2O}}

Putting values in above equation, we get:

K_p=\frac{2.167\times (6.5)^3}{0.233\times 1.733}\\\\K_p=1473.8

Hence, the pressure equilibrium constant for the reaction is 1473.8

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Consider the following reaction:
iren [92.7K]

Answer:

A. ΔG° = 132.5 kJ

B. ΔG° = 13.69 kJ

C. ΔG° = -58.59 kJ

Explanation:

Let's consider the following reaction.

CaCO₃(s) → CaO(s) + CO₂(g)

We can calculate the standard enthalpy of the reaction (ΔH°) using the following expression.

ΔH° = ∑np . ΔH°f(p) - ∑nr . ΔH°f(r)

where,

n: moles

ΔH°f: standard enthalpy of formation

ΔH° = 1 mol × ΔH°f(CaO(s)) + 1 mol × ΔH°f(CO₂(g)) - 1 mol × ΔH°f(CaCO₃(s))

ΔH° = 1 mol × (-635.1 kJ/mol) + 1 mol × (-393.5 kJ/mol) - 1 mol × (-1206.9 kJ/mol)

ΔH° = 178.3 kJ

We can calculate the standard entropy of the reaction (ΔS°) using the following expression.

ΔS° = ∑np . S°p - ∑nr . S°r

where,

S: standard entropy

ΔS° = 1 mol × S°(CaO(s)) + 1 mol × S°(CO₂(g)) - 1 mol × S°(CaCO₃(s))

ΔS° = 1 mol × (39.75 J/K.mol) + 1 mol × (213.74 J/K.mol) - 1 mol × (92.9 J/K.mol)

ΔS° = 160.6 J/K. = 0.1606 kJ/K.

We can calculate the standard Gibbs free energy of the reaction (ΔG°) using the following expression.

ΔG° = ΔH° - T.ΔS°

where,

T: absolute temperature

<h3>A. 285 K</h3>

ΔG° = ΔH° - T.ΔS°

ΔG° = 178.3 kJ - 285K × 0.1606 kJ/K = 132.5 kJ

<h3>B. 1025 K</h3>

ΔG° = ΔH° - T.ΔS°

ΔG° = 178.3 kJ - 1025K × 0.1606 kJ/K = 13.69 kJ

<h3>C. 1475 K</h3>

ΔG° = ΔH° - T.ΔS°

ΔG° = 178.3 kJ - 1475K × 0.1606 kJ/K = -58.59 kJ

5 0
3 years ago
What volume of carbon dioxide gas at STP is required to produce 456.9g of lithium carbonate?
Margarita [4]

Answer:

It would have to be around 9.8 volume

Explanation:

7 0
3 years ago
What volume in mt, of 0.5a M1HCI solution is needed to neutralize 77 ml of 1.54 M NaOH solution?
Rainbow [258]

Answer:

237.2 mL.

Explanation:

  • We have the rule: at neutralization, the no. of millimoles of acid is equal to the no. of millimoles of the base.

(XMV) acid = (XMV) base.

where, X is the no. of (H) or (OH) reproducible in acid or base, respectively.

M is the molarity of the acid or base.

V is the volume of the acid or base.

<em>(XMV) HCl = (XMV) NaOH.</em>

<em></em>

For HCl; X = 1, M = 0.5 M, V = ??? mL.

For NaOH, X = 1, M = 1.54 M, V = 77.0 mL.

<em>∴ V of HCl = (XMV) NaOH / (XV) HCl = (</em>1)(1.54 M)(77.0 mL) / (1)(0.5 M) = <em>237.2 mL.</em>

8 0
3 years ago
Write the complete balanced equation for the following reaction: Al + Fe(NO2)2 Fe + Al(NO2)3
algol13
The equation is already balanced.
7 0
3 years ago
C9H20 +<br> 02 - &gt; CO2 +<br> H2O<br><br> what is the balanced equation of this
san4es73 [151]

Hey there!

C₉H₂O + O₂ → CO₂ + H₂O

First let's balance the C.

There's 9 on the left and 1 on the right. So, let's add a coefficient of 9 in front of CO₂.

C₉H₂O + O₂ → 9CO₂ + H₂O

Next let's balance the H.

There's 2 on the left and 2 on the right. This means it's already balanced.

C₉H₂O + O₂ → 9CO₂ + H₂O

Lastly, let's balance the O.

There's 3 on the left and 19 on the right. So, let's add a coefficient of 9 in front of O₂.

C₉H₂O + 9O₂ → 9CO₂ + H₂O

This is our final balanced equation.

Hope this helps!

8 0
2 years ago
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