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3 years ago

Consider this equilibrium: I2(s) + H2O(l) H + (aq) + I-(aq) + HOI(aq). What is the Keq expression for this equilibrium?

1 answer:

3 0

<span>The Keq expression for I2(s) + H2O(l) H + (aq) + I-(aq) + HOI(aq) equilibrium is H2(g) + I2(g) <----> 2 HI(g).In this Keq expression hydrogen reacts with iodine gives Hydrogen Iodide.HI is a diatomic molecule and it is one of the primary source of iodine which act as a reducing agent.Totally it is the reverse chemical equilibrium reaction.</span>

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This is what the map is for question 4

serious [3.7K]

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3 years ago

Determine the mole fractions and partial pressures of CO2, CH4, and He in a sample of gas that contains 1.20 moles of CO2, 1.79

BARSIC [14]

Answer : The mole fraction and partial pressure of $CH_4,CO_2$ and $He$ gases are, 0.267, 0.179, 0.554 and 1.54, 1.03 and 3.20 atm respectively.

Explanation : Given,

Moles of $CH_4$ = 1.79 mole

Moles of $CO_2$ = 1.20 mole

Moles of $He$ = 3.71 mole

Now we have to calculate the mole fraction of $CH_4,CO_2$ and $He$ gases.

$\text{Mole fraction of }CH_4=\frac{\text{Moles of }CH_4}{\text{Moles of }CH_4+\text{Moles of }CO_2+\text{Moles of }He}$

$\text{Mole fraction of }CH_4=\frac{1.79}{1.79+1.20+3.71}=0.267$

and,

$\text{Mole fraction of }CO_2=\frac{\text{Moles of }CO_2}{\text{Moles of }CH_4+\text{Moles of }CO_2+\text{Moles of }He}$

$\text{Mole fraction of }CO_2=\frac{1.20}{1.79+1.20+3.71}=0.179$

and,

$\text{Mole fraction of }He=\frac{\text{Moles of }He}{\text{Moles of }CH_4+\text{Moles of }CO_2+\text{Moles of }He}$

$\text{Mole fraction of }He=\frac{3.71}{1.79+1.20+3.71}=0.554$

Thus, the mole fraction of $CH_4,CO_2$ and $He$ gases are, 0.267, 0.179 and 0.554 respectively.

Now we have to calculate the partial pressure of $CH_4,CO_2$ and $He$ gases.

According to the Raoult's law,

$p_i=X_i\times p_T$

where,

$p_i$ = partial pressure of gas

$p_T$ = total pressure of gas = 5.78 atm

$X_i$ = mole fraction of gas

$p_{CH_4}=X_{CH_4}\times p_T$

$p_{CH_4}=0.267\times 5.78atm=1.54atm$

and,

$p_{CO_2}=X_{CO_2}\times p_T$

$p_{CO_2}=0.179\times 5.78atm=1.03atm$

and,

$p_{He}=X_{He}\times p_T$

$p_{He}=0.554\times 5.78atm=3.20atm$

Thus, the partial pressure of $CH_4,CO_2$ and $He$ gases are, 1.54, 1.03 and 3.20 atm respectively.

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3 years ago

Calculate the approximate volume of a 1.50 mol sample of gas at 15.0°C and a pressure of 3.75 atm

Papessa [141]

Answer:

The answer is J (9.46 L)

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3 years ago

Which scenario represents an unbalanced force?

ladessa [460]

A . A person Jumping represents an unbalanced force.

<u>Explanation:</u>

If equal amount of force applied on any object from both the directions, then the object will not move and so the force is a balanced force.

If an unequal amount of force on an object from both sides then the object will move in the opposite direction of the maximum force applied, so it is called as an unbalanced force.

When the force is unbalanced then its velocity will change, so options C and D are omitted.

In Option B the vase is sitting on a table, just kept so there is no action of any unbalanced force.

But a person jumping represents an unbalanced force, since the person do not jump with constant velocity and it will vary.

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3 years ago

Identify what type of reaction is below. Also, determine what coefficients that would balance the chemical equation. ___ C4H10 +

Evgen [1.6K]

This is a combustion reaction because it is being combined with oxygen. Then to balance you will put the number of carbons you have or 4 in front of the CO2 and then same with H2. Then you will add up the oxygen and divide it by two to get. 1, (13/2), 4, 5

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2 years ago