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3 years ago

The rate constant for the first-order decomposition of n2o is 3.40 s-1. what is the half-life of the decomposition?

Chemistry

2 answers:

Nadya [2.5K]3 years ago

4 0

<u>Answer:</u> The half life of the decomposition reaction is 0.204 s

<u>Explanation:</u>

The equation used to calculate half life for first order kinetics:

$t_{1/2}=\frac{0.693}{k}$

where,

k = rate constant of the reaction = $3.40s^{-1}$

$t_{1/2}$ = half life of the reaction = ?

Putting values in above equation, we get:

$t_{1/2}=\frac{0.693}{3.40s^{-1}}\\\\t_{1/2}=0.204s$

Hence, the half life of the decomposition reaction is 0.204 s

stiks02 [169]3 years ago

3 0

Hey There:

First order half life equation :

T 1/2 = ln ( 2 ) /K

T 1/2 = 0.693 / 3.40

T 1/2 = 0.204 s

Answer B

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Gaseous butane, CH3(CH2)2CH, reacts with gaseous oxygen gas, O2, to produce gaseous carbon dioxide, CO2, and gaseous water, H2O.

weeeeeb [17]

Answer:

Percentage yield of carbon dioxide is 49.9%

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

2CH3(CH2)2CH3 + 13O2 —> 8CO2 + 10H2O

2C4H10 + 13O2 —> 8CO2 + 10H2O

Next, we shall determine the masses of butane and oxygen that reacted and the mass of carbon dioxide produced from the balanced equation. This is illustrated below:

Molar mass of butane C4H10 = (12×4) + (10×1)

= 48 + 10

= 58 g/mol

Mass of C4H10 from the balanced equation = 2 × 58 = 116 g

Molar mass of O2 = 16 × 2 = 32 g/mol

Mass of O2 from the balanced equation = 13 × 32 = 416 g

Molar mass of CO2 = 12 + (16×2)

= 12 + 32

= 44 g/mol

Mass of CO2 from the balanced equation = 8 × 44 = 352 g

Summary:

From the balanced equation above,

116 g of butane reacted with 416 g of oxygen to produce 352 g of carbon dioxide.

Next, we shall determine the limiting reactant. This can be obtained as follow:

From the balanced equation above,

116 g of butane reacted with 416 g of oxygen.

Therefore, 34.29 g of butane will react with = (34.29 × 416) / 116 = 122.97 g of oxygen.

From the calculation made above, we can see clearly that only 122.97 g out of 165.7 g of oxygen reacted completely with 34.29 g of butane. Therefore, butane is the limiting reactant and oxygen is the excess reactant.

Next, we shall determine the theoretical yield of carbon dioxide.

In this case, we shall use the limiting reactant because it will give the maximum yield of carbon dioxide as all of it is used up in the reaction.

The limiting reactant is butane and the theoretical yield of carbon dioxide can be obtained as follow:

From the balanced equation above,

116 g of butane reacted to produce 352 g of carbon dioxide.

Therefore, 34.29 g of butane will react to produce = (34.29 × 352) / 116 = 104.05 g of carbon dioxide.

Therefore, the theoretical yield of carbon dioxide is 104.05 g

Finally, we shall determine the percentage yield of carbon dioxide as follow:

Actual yield of carbon dioxide = 51.9 g

Theoretical yield of carbon dioxide = 104.05 g

Percentage yield of carbon dioxide =?

Percentage yield = Actual yield /Theoretical yield × 100

Percentage yield of carbon dioxide = 51.9 / 104.05 × 100

Percentage yield of carbon dioxide = 49.9%

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3 years ago

1. Look at the DNA molecule shown at right. What does it look like?

jarptica [38.1K]

Answer:

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a block of iron has the dimensions of 3.00 cm x 3.00 cm x 3.00 cm. it has a mass of 213 g. when placed in water, the block sinks

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When the block of iron is placed in water the volume of water that is displaced is 27.0 cm³

<u><em> calculation</em></u>

The volume water that is displaced is equal to volume of block of the iron

volume of block of iron = length x width x height

length= 3 cm

width = 3 cm

height = 3 cm

volume is therefore = 3 cm x 3 cm x 3 cm = 27 cm³ therefore the volume displaced = 27 cm³ since the volume of water displaced is equal to volume of block.

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Answer:

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3 years ago

Methane and oxygen react to form carbon dioxide and water. what mass of water is formed if 0.80 g of methane reacts with 3.2 g o

Charra [1.4K]

1.8 g

<h3>Further explanation</h3>

<u>Given:</u>

0.80 g of methane reacts with 3.2 g of oxygen to produce 2.2 g of carbon dioxide.

<u>Question:</u>

What mass of water is formed?

<u>The Process:</u>

Methane and oxygen react to form carbon dioxide and water. Remember this, the chemical activity that uses oxygen to produce light and heat is also called the combustion process.

In any chemical reaction, the sum of the masses of the reactants is equal to the sum of the masses of the products. That's right, this is called conservation of the masses.

Let us write the word equation of the chemical reaction and then solve the problem following the law of the conservation of mass.

$\boxed{ \ Methane + Oxygen \rightarrow Carbon \ dioxide + Water\ }$

$\boxed{ \ 0.80 \ g \ + \ 3.2 \ g \rightarrow 2.2 \ g \ + \ m_{Water}? \ }$

$\boxed{ \ m_{reactants} = m_{products} \ }$

$\boxed{ \ 0.80 \ g \ + \ 3.2 \ g = 2.2 \ g \ + \ m_{Water} \ }$

Rewrite by rearranging as follows:

$\boxed{ \ 2.2 \ g \ + \ m_{Water} = 0.80 \ g \ + \ 3.2 \ g \ }$

$\boxed{ \ 2.2 \ g \ + \ m_{Water} = 4.0 \ g \ }$

$\boxed{ \ m_{Water} = 4.0 \ g - 2.2 \ g \ }$

Thus the mass of water formed is 1.8 g.

The balanced equation with state symbols is:

$\boxed{ \ CH_4_{(g)} + 2O_2_{(g)} \rightarrow CO_2_{(g)} + 2H_2O_{(l)} \ }$

<u>Notes:</u>

The French scientist Antoine Laurent Lavoisier represented his essential contribution by declaring the law of conservation of mass as one of the fundamental laws in chemistry.
The law of the conservation of the mass states that in a chemical reaction the sum of the masses of the reactants is equal to the sum of the masses of the products. $\boxed{\boxed{ \ m_{reactants} = m_{products} \ }}$

<h3>Learn more</h3>

Flammability as one of the chemical properties brainly.com/question/1767022
Carbon atoms can form four covalent bonds brainly.com/question/3064597
About the solution as a homogeneous mixture brainly.com/question/637791

Keywords: methane and oxygen, react to form carbon dioxide and water, combustion, to produce, the conservation of mass, the word equation, the balanced equation, Lavoisier

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