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3 years ago

I need help identifying the type of reactions. Can anyone help?

Chemistry

2 answers:

Eddi Din [679]3 years ago

7 0

Answer:

Reaction 5: Decomposition reaction.

Reaction 6: Single replacement reaction

Reaction 7: Combination reaction.

Reaction 8: Combustion reaction.

Explanation:

Reaction 5: 2KClO₃ → 2KCl + 3O₂.

It is a decomposition reaction.

A decomposition reaction is a type of chemical reaction in which a single compound breaks down into two or more elements or new compounds.

In this reaction: potassium chlorate decomposes into two single components (potassium chloride and oxygen).
So, it is a decomposition reaction.

Reaction 6: Zn + 2HCl → H₂ + ZnCl₂.

It is a single replacement reaction.

A single-replacement reaction, a single-displacement reaction, is a reaction by which one (or more) element(s) replaces an/other element(s) in a compound.
It is most often occur if element is more reactive than the other, thus giving a more stable product.

In this reaction, zinc metal (more active) displaces the hydrogen to form hydrogen gas and zinc chloride, a salt. Zinc reacts quickly with the acid to form bubbles of hydrogen.

Reaction 7: N₂O₅ + H₂O → 2HNO₃.

It is a combination "synthesis" reaction.
A synthesis reaction has two or more reactants and only one product.
In this reaction, dinitrogen pentoxide reacts with water to produce nitric acid.
So, it is considered as a synthetic "combination" reaction.

Reaction 8: 2C₂H₆ + 7O₂ → 4CO₂ + 6H₂O.

It is a combustion reaction.

A combustion reaction is a reaction where hydrocarbon alkane is completely burned in oxygen to produce water and carbon dioxide.

In this reaction 1.0 mole of ethane is burned to give 4.0 moles of carbon dioxide and 6.0 moles of water.

So, it is considered as a combustion reaction.

Rainbow [258]3 years ago

3 0

<h2>Answer:</h2>

The type of reaction and explanation is attached in the picture

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The equilibrium constant Kp for the reaction (CH3),CCI (g) = (CH3),C=CH, (g) + HCl (g) is 3.45 at 500. K. (5.00 x 10K) Calculate

Karolina [17]

Answer: The value of $K_p$ for the reaction is 6.32 and concentrations of $(CH_3)_2C=CH,HCl\text{ and }(CH_3)_3CCl$ is 0.094 M, 0.094 M and 0.106 M respectively.

Explanation:

Relation of $K_p$ with $K_c$ is given by the formula:

$K_p=K_c(RT)^{\Delta ng}$

where,

$K_p$ = equilibrium constant in terms of partial pressure = 3.45

$K_c$ = equilibrium constant in terms of concentration = ?

R = Gas constant = $0.0821\text{ L atm }mol^{-1}K^{-1}$

T = temperature = 500 K

$\Delta n_g$ = change in number of moles of gas particles = $n_{products}-n_{reactants}=2-1=1$

Putting values in above equation, we get:

$3.45=K_c\times (0.0821\times 500)^{1}\\\\K_c=\frac{3.45}{0.0821\times 500}=0.084$

The equation used to calculate concentration of a solution is:

$\text{Molarity}=\frac{\text{Moles}}{\text{Volume (in L)}}$

Initial moles of $(CH_3)_3CCl(g)$ = 1.00 mol

Volume of the flask = 5.00 L

So, $\text{Concentration of }(CH_3)_3CCl=\frac{1.00mol}{5.00L}=0.2M$

For the given chemical reaction:

$(CH_3)_3CCl(g)\rightarrow (CH_3)_2C=CH(g)+HCl(g)$

Initial: 0.2 - -

At Eqllm: 0.2 - x x x

The expression of $K_c$ for above reaction follows:

$K_c=\frac{[(CH_3)_2C=CH]\times [HCl]}{[(CH_3)_3CCl]}$

Putting values in above equation, we get:

$0.084=\frac{x\times x}{0.2-x}\\\\x^2+0.084x-0.0168=0\\\\x=0.094,-0.178$

Negative value of 'x' is neglected because initial concentration cannot be more than the given concentration

Calculating the concentration of reactants and products:

$[(CH_3)_2C=CH]=x=0.094M$

$[HCl]=x=0.094M$

$[(CH_3)_3CCl]=(0.2-x)=(0.2-0.094)=0.106M$

Hence, the value of $K_p$ for the reaction is 6.32 and concentrations of $(CH_3)_2C=CH,HCl\text{ and }(CH_3)_3CCl$ is 0.094 M, 0.094 M and 0.106 M respectively.

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3 years ago

Exactly one mole of an ideal gas is contained in a 2.00-liter container at 1,000 K. What is the pressure exerted by this gas?

levacccp [35]

Use PV =nRT

so P = nRT/V

= 1 mole(0.08205 L atm/K mol)(1000K) / 2 L

= 41 atm

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MakcuM [25]

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astra-53 [7]

Answer:

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