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3 years ago

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Which of the these is a balanced chemical equation? A) CO(g) + O2(g) → CO2(g) B) CO(g) + 2O2(g) → 2CO2(g) C) 2CO(g) + O2(g) → 2C

O2(g) D) 2CO(g) + 2O2(g) → 2CO2(g)

2 answers:

jenyasd209 [6]3 years ago

6 0

Answer: C.

This is because the atoms on either side of the equation in all the other solutions are not equal.

Alinara [238K]3 years ago

3 0

hello there the answer is c sir

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HCl +KOH ---> KCl + H20

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Answer:

5.59x10^-3 moles

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From the illustration made above, we can see evidently that 5.59x10^-3 moles of HCl is required to produce 5.59x10^-3 moles of KCl

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2 years ago

In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H2O (g) ⇌

Oksana_A [137]

Answer: Equilibrium constant is 0.70.

Explanation:

Initial moles of $CO$ = 0.35 mole

Volume of container = 1 L

Initial concentration of $CO=\frac{moles}{volume}=\frac{0.35moles}{1L}=0.35M$

Initial moles of $H_2O$ = 0.40 mole

Volume of container = 1 L

Initial concentration of $H_2O=\frac{moles}{volume}=\frac{0.40moles}{1L}=0.40M$

equilibrium concentration of $CO=\frac{moles}{volume}=\frac{0.18moles}{1L}=0.18M$ [/tex]

The given balanced equilibrium reaction is,

$CO(g)+H_2O(g)\rightleftharpoons CO_2(g)+H_2(g)$

Initial conc. 0.35 M 0.40M 0 0

At eqm. conc. (0.35-x) M (0.40-x) M (x) M (x) M

The expression for equilibrium constant for this reaction will be,

$K_c=\frac{[CO_2]\times [H_2O]}{[CO]\times [H_2O]}$

$K_c=\frac{x\times x}{(0.40-x)(0.35-x)}$

we are given : (0.35-x)= 0.18

x = 0.17

Now put all the given values in this expression, we get :

$K_c=\frac{0.17\times 0.17}{(0.40-0.17)(0.35-0.17)}$

$K_c=0.70$

Thus the value of the equilibrium constant is 0.70.

5 0

2 years ago