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

Hatshy [7]

Answer: The pressure equilibrium constant for the reaction is 1473.8

Explanation:

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:

$CH_4+H_2O\rightleftharpoons CO+3H_2$

Initial: 2.4 3.9

At eqllm: 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

5 0

4 years ago

Based on this reaction, find how many moles of co can be obtained starting with 7 mol ch4?

Klio2033 [76]

I will solve the question assuming the reaction used as below
1 CH4(g) + 1 H2O(g) ==> 1 CO(g) + 3 H2(g)

In the reaction, CH4 is the reactant and CO is the wanted product. If you look at the coefficient of the substance, for every 1 mol of CH4 react there will be 1 mol of CO produced. So, if you have 7 moles of CH4 the amount of CO produced would be: 7 moles * 1/1= 7 moles of CO

5 0

4 years ago

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A metal ion (X) with a charge of 2+ is attracted to a nonmetal ion (Z) with a charge of 3-.Which formula represents the resultin

Viefleur [7K]

Answer:

X₃Z₂

Explanation:

A metal ion (X) with a charge of 2+ = X²⁺

nonmetal ion (Z) with a charge of 3- = Z³⁻

In a neutral compound, the charges but balance each other to remain neutral. However in this case, the charges are not balanced.

A simple way to make the charges balance is by tweaking the number of the ions present in the compound.

We do this by multiplying the metal ion with 3 and the non metal ion by 2.

That way we have;

Metal ion = 3X2⁺ (Total charge - 6⁺)

Non metal ion = 2Z3⁻ (Total charge - 6⁻)

The charges are now balanced. The formular of the compound is;

X₃Z₂

5 0

3 years ago

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What is the pH of a solution in which [OH-] = 1.0 x 10-2 M

Degger [83]

Answer:

12

Explanation:

pOH = -log(1.0 x 10^-2) = 2

pH = 14 - pOH

pH = 14 - 2 = 12

7 0

3 years ago

1) 2C2H6 + 7O2 --> 4CO2 + 6H2O

Lena [83]

Answer:

a).

$2 \: moles \: of \: ethane \: react \: with \: 7 \: moles \: of \: oxygen \\ 24 \: moles \: react \: with \: ( \frac{24 \times 7}{2} ) \: moles \\ = 84 \: moles$

b).

$2 \: moles \: react \: with \: 7 \: moles \\ ( \frac{12 \times 2}{7} ) \: moles \: react \: with \: 12 \: moles \\ = 3 .43 \: moles \\ 1 \: mole \: weighs \: 30 \: g \\ 3.43 \: moles \: weigh \: (3.43 \times 30) \\ = 102.9 \: g$

c).

746.7 g

7 0

3 years ago

Did you cook the food yourself ?into passive​

Did you cook the food yourself ?into passive