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3 years ago

If the forward reaction is favored in the equilibrium, what will increase?

Chemistry

1 answer:

Lorico [155]3 years ago

5 0

Answer:

Option C:- concentration of products

Explanation:

According to Le Chateleir's principle,

if the forward reaction is favored in the equilibrium then concentration of products will increase and concentration of reactants will decrease.

If the reverse reaction is favored in the equilibrium then concentration of products will decrease and concentration of reactants will increase.

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What kinds of processes can cause rocks to change?

DENIUS [597]

1.Heat:Heat can cause rock to melt,forcing real changes in its chemical and physical makeup;forcing some elemental components to chemically react with each other,both internal and external,chemical components to form entirely new material.
another way is erosion

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3 years ago

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Lithium acetate, LiCH3CO2, is a salt formed from the neutralization of the weak acid acetic acid, CH3CO2H, with the strong base

Vesna [10]

Answer : The pH of 0.289 M solution of lithium acetate at $25^oC$ is 9.1

Explanation :

First we have to calculate the value of $K_b$ .

As we know that,

$K_a\times K_b=K_w$

where,

$K_a$ = dissociation constant of an acid = $1.8\times 10^{-5}$

$K_b$ = dissociation constant of a base = ?

$K_w$ = dissociation constant of water = $1\times 10^{-14}$

Now put all the given values in the above expression, we get the dissociation constant of a base.

$1.8\times 10^{-5}\times K_b=1\times 10^{-14}$

$K_b=5.5\times 10^{-10}$

Now we have to calculate the concentration of hydroxide ion.

Formula used :

$[OH^-]=(K_b\times C)^{\frac{1}{2}}$

where,

C is the concentration of solution.

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

$[OH^-]=(5.5\times 10^{-10}\times 0.289)^{\frac{1}{2}}$

$[OH^-]=1.3\times 10^{-5}M$

Now we have to calculate the pOH.

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

$pOH=-\log (1.3\times 10^{-5})$

$pOH=4.9$

Now we have to calculate the pH.

$pH+pOH=14\\\\pH=14-pOH\\\\pH=14-4.9=9.1$

Therefore, the pH of 0.289 M solution of lithium acetate at $25^oC$ is 9.1

4 0

4 years ago

Which natural polymers are involved with making clothing?

fredd [130]

Answer:

A. wool, silkworm, cocoon, and cellulose

Explanation:

I hope this helped!

7 0

3 years ago

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Suppose that 0.25 mole of gas C was added to the mixture without changing the total pressure of the mixture. How does the additi

Yanka [14]

Here we have to get the effect of addition of 0.25 moles of gas C on the mole fraction of gas A in a mixture of gas having constant pressure.

On addition of 0.25 moles of C gas, the mole fraction of gas A will be $\frac{moles of gas A}{moles of gas A + 0.25}$ .

The partial pressure of gas A can be written as $P_{A}$ = $x_{A}$ ×P (where $x_{A}$ is the mole fraction of gas A present in the mixture and P is the total pressure of the mixture.

The mole fraction of gas A in a mixture of gas A and C is = $\frac{moles of gas A}{moles of gas A + moles of gas C}$ and $\frac{moles of gas C}{moles of gas A + moles of gas C}$ respectively.

Thus on addition of 0.25 moles of C gas, the mole fraction of gas A will be $\frac{moles of gas A}{moles of gas A + 0.25}$ .

Which is different from the initial state.

4 0

3 years ago

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URGENT HELP NEEDED

balu736 [363]

the balanced equation for the reaction is as follows
2C₄H₁₀ + 13O₂ ---> 8 CO₂ + 10H₂O
stoichiometry of C₄H₁₀ to O₂ is 2:13
stoichiometry applies to the molar ratio of reactants and products. Avagadros law states that volume of gas is directly proportional to number of moles of gas when pressure and temperature are constant.
Therefore volume ratio of reactants is equal to molar ratio, volume ratio of C₄H₁₀ to O₂ is 2:13
2 L of C₄H₁₀ reacts with 13 L of O₂
then 100 L of C₄H₁₀ reacts with 13/2 x 100 = 650 L
therefore 650 L of O₂ are required

7 0

3 years ago

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