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3 years ago

Which type of chemical reaction typically produces carbon dioxide and water as its products?

Chemistry

1 answer:

klio [65]3 years ago

3 0

This is combustion
CH4+2O2---> CO2 +2H2O

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What is the hydroxide ion concentration of a solution whose pOH is 6.42?

Sergeeva-Olga [200]

Answer : The hydroxide ion concentration of a solution is, $3.8\times 10^{-7}M$

Explanation :

As we know that:

pH : It is defined as the negative logarithm of hydrogen ion concentration.

Mathematically,

$pH=-\log [H^+]$

Similarly,

pOH : It is defined as the negative logarithm of hydroxide ion concentration.

Mathematically,

$pOH=-\log [OH^-]$

Given:

pOH = 6.42

$6.42=-\log [OH^-]$

$[OH^-]=3.8\times 10^{-7}M$

Therefore, the hydroxide ion concentration of a solution is, $3.8\times 10^{-7}M$

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3 years ago

Potassium has an atomic number of 19.

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4 years ago

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3 years ago

How do the test variables (independent variables) and outcome variables (dependent variables) in an experiment compare? A. The o

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Explanation:

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3 years ago

Read 2 more answers

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

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3 years ago