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wlad13 [49]
3 years ago
15

Assuming 1 mol of Fe3+ and 2 mol of SCN- were allowed to react and reach equilibrium. 0.5 mol of product was formed. The total v

olume at equilibrium was 1 L. How much Fe3+ remained at equilibrium? (in mol) (1 point) Your Answer: How much SCN- remained at equilibrium? (in mol) (1 point) Your Answer: What’s the equilibrium constant, Kc? (1 point)
Chemistry
1 answer:
zaharov [31]3 years ago
3 0

Answer:

a. 0.5 mol

b. 1.5 mol

c. 0.67

Explanation:

Fe3+ + SCN- -----> [FeSCN]2+

a. The ratio of the product to Fe3+ is 1:1. Meaning that if 0.5 mol of product was produced up then 0.5 mol of Fe3+ was used. Leaving 0.5 mol remaining at equilibrium

b. The ratio of the product to SCN= is 1:1. Meaning that if 0.5 mol of product was produced up then 0.5 mol of SCN- was used. Leaving 1.5 mol remaining at equilibrium

c. KC =  0.5/(0.5*1.5) =  0.67

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Answer:

C

Explanation:

It afffects changes in pressure and temperature not melting and boiling points

5 0
2 years ago
.266 mol CO plus .524 Mol H2 gives how many moles of CH3OH
Readme [11.4K]

Explanation:

Carbon monoxide and hydrogen gas reacts together to form methanol:

CO + 2H2 => CH3OH

Since 0.266mol * 2 = 0.532mol > 0.524mol, the limiting reactant here is hydrogen and therefore there will be 0.524mol / 2 = 0.262mol of methanol.

3 0
3 years ago
What is the difference between a homogeneous and a heterogeneous mixture?
Ne4ueva [31]

Answer and explanation :

DIFFERENCE BETWEEN HOMOGENEOUS AND HETEROGENEOUS MIXTURE :

  • In homogeneous mixture the component which are present in the mixture all are in the same proportion whereas in heterogeneous mixture the component which are present in the mixture don't have the same proportion
  • We can not pick out the component of homogeneous mixture but in heterogeneous mixture we can pick out the components from the mixture
  • Example of homogeneous mixture is water, oil ,water sugar solution, milk  blood etc. And example of heterogeneous mixture is solution of sand and water ,concrete etc.
7 0
3 years ago
When a chemical reaction is at equilibrium, which of the following statements is always TRUE?
AysviL [449]

<u>Answer:</u> The correct answer is Option D.

<u>Explanation:</u>

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric coefficients. It is represented by K_{eq}

For a general chemical reaction:

aA+bB\rightarrow cC+dD

The K_{eq} is written as:

K_{eq}=\frac{[C]^c[D]^d}{[A]^a[B]^b}

There are 3 conditions:

  • When K_{eq}>1; the reaction is product favored.
  • When K_{eq}; the reaction is reactant favored.
  • When K_{eq}=1; the reaction is in equilibrium.

At equilibrium, the  ratio of concentration of reactants to the concentration of products is equal to 1.

At equilibrium, the rate of forward reaction is equal to rate of backward reaction.

Hence, the correct answer is Option D.

7 0
3 years ago
In a constant‑pressure calorimeter, 70.0 mL of 0.350 M Ba(OH)2 was added to 70.0 mL of 0.700 M HCl. The reaction caused the temp
DanielleElmas [232]

<u>Answer:</u> The amount of heat absorbed by the solution is 2.795 kJ

<u>Explanation:</u>

To calculate the mass of water, we use the equation:

\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}

Density of water = 1 g/mL

Volume of water = [70 + 70] = 140 mL

Putting values in above equation, we get:

1g/mL=\frac{\text{Mass of water}}{140mL}\\\\\text{Mass of water}=(1g/mL\times 140mL)=140g

To calculate the heat absorbed, we use the equation:

q=mc\Delta T

where,

q = heat absorbed

m = mass of water = 140 g

c = heat capacity of water = 4.186 J/g°C

\Delta T = change in temperature = T_2-T_1=(28.74-23.97)^oC=4.77^oC

Putting values in above equation, we get:

q=140g\times 4.186J/g^oC\times 4.77^oC=2795.4J=2.795kJ

Hence, the amount of heat absorbed by the solution is 2.795 kJ

3 0
3 years ago
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