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3 years ago

What is an equilibrium constant

1 answer:

4 0

The equilibrium constant of a chemical reaction is the value of the reaction quotient when the reaction has reached equilibrium. An equilibrium constant value is independent of the analytical concentrations of the reactant and product species in a mixture, but depends on temperature and on ionic strength.

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Which is a characteristic of mixtures ?

sattari [20]

The characteristics of mixtures are:

a) they are made up of two of more substances

b) the two substances can be separated by physical means

c) there are two kinds of mixtures : homogenous and heterogenous

d) homogenous mixtures do not have any physicaly distinguished boundary

6 0

4 years ago

Read 2 more answers

The heat of combustion of propane, C3H8 (g) is -2057 kJ/mol. What would be the enthalpy change if enough propane was burned to g

Digiron [165]

Considering the reaction stoichiometry, the enthalpy change if enough propane was burned to give off 12 moles of carbon dioxide gas is 8228 kJ.

The balanced reaction is:

C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O(l)

The heat of combustion of propane, C₃H₈, is -2057 kJ/mol. This is, 2057 kJ is released for every 1 mol C₃H₈.

So to determine the enthalpy change if enough propane was burned to emit 12 moles of carbon dioxide, you must take into account the stoichiometry of the reaction.

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

C₃H₈: 1 mole
O₂: 5 moles
CO₂: 3 moles
H₂O: 4 moles

Then you can apply the following rule of three: if by stoichiometry 3 moles of CO₂ are produced by 1 mole of C₃H₈, 12 moles of CO₂ are produced by how many moles of C₃H₈?

$amount of moles of C_{3} H_{8} =\frac{12 moles of CO_{2}x1 mole of C_{3} H_{8} }{3 moles of CO_{2}}$

amount of moles of C₃H₈= 4 moles

So to determine the enthalpy change, you can apply the following rule of three: If for each mole of C₃H₈ 2057 kJ are released, for 4 moles of C₃H₈ how much heat is released?

$Heat released=\frac{4 molesx2057 kJ}{1 mole}$

Heat released= 8228 kJ

The enthalpy change if enough propane was burned to give off 12 moles of carbon dioxide gas is 8228 kJ.

Learn more:

5 0

3 years ago

How much heat must absorbed by the reaction system to convert 100g of NaNO3 into NaHSO4(s)?

Alex787 [66]

Answer:

about 4.8kJ

Explanation:

6 0

3 years ago

Rusting of iron is a very common chemical reaction. It results in one form from Fe reacting with oxygen gas to produce iron (III

Vlada [557]

Answer: The given amount of iron reacts with 9.0 moles of $O_2$ and produce 6.0 moles of $Fe_2O_3$

Explanation:

We are given:

Moles of iron = 12.0 moles

The chemical equation for the rusting of iron follows:

$4Fe+3O_2\rightarrow 2Fe_2O_3$

For oxygen gas:

By Stoichiometry of the reaction:

4 moles of iron reacts with 3 moles of oxygen gas

So, 12.0 moles of iron will react with = $\frac{3}{4}\times 12.0=9.0mol$ of oxygen gas

For iron (III) oxide:

By Stoichiometry of the reaction:

4 moles of iron produces 2 moles of iron (III) oxide

So, 12.0 moles of iron will produce = $\frac{2}{4}\times 12.0=6.0mol$ of iron (III) oxide

Hence, the given amount of iron reacts with 9.0 moles of $O_2$ and produce 6.0 moles of $Fe_2O_3$

5 0

3 years ago

will give brainliest!! please help ! .. Calculate the total pressure of the mixture in atmospheres ( atm ).

nordsb [41]

Answer:

13.94 atm

Explanation:

From the question given above, the following data were obtained:

Pressure of H₂ = 2 atm

Pressure of NH₃ = 303 KPa

Pressure of CO₂ = 3000 mmHg

Pressure of N₂ = 3800 torr

Total pressure (Pₜ) in atm =?

Next, we shall convert 303 KPa, 3000 mmHg and 3800 torr to atm.

This can be obtained as follow:

Converting 303 KPa to atm

101.325 KPa = 1 atm

Therefore,

303 KPa = 303 KPa × 1 atm / 101.325 KPa

303 KPa = 2.99 atm

Thus, 303 KPa is equivalent to 2.99 atm.

Converting 3000 mmHg to atm

760 mmHg = 1 atm

Therefore,

3000 mmHg = 3000 mmHg × 1 atm / 760 mmHg

3000 mmHg = 3.95 atm

Thus, 3000 mmHg is equivalent to 3.95 atm

Converting 3800 torr to atm

760 torr = 1 atm

Therefore,

3800 torr = 3800 torr × 1 atm / 760 torr

3800 torr = 5 atm

Thus, 3800 torr is equivalent to 5 atm.

Finally, we shall determine the total pressure of the mixture as follow:

Pressure of H₂ (P₁) = 2 atm

Pressure of NH₃ (P₂) = 2.99 atm

Pressure of CO₂ (P₃) = 3.95 atm

Pressure of N₂ (P₄) = 5 atm

Total pressure (Pₜ) in atm =?

Pₜ = P₁ + P₂ + P₃ + P₄

Pₜ = 2 + 2.99 + 3.95 + 5

Pₜ = 13.94 atm

Therefore, the total pressure of the mixture is 13.94 atm

4 0

3 years ago