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Serga [27]
2 years ago
6

Review Toples

Chemistry
1 answer:
jekas [21]2 years ago
5 0

Answer:

1.553 M^2s^-1

Explanation:

Now let us consider experiments 1,2,3.

In experiment 1 and 2, the concentration of NO is doubled and the initial rate of reaction is quadrupled.

0.575/0.144 = 4

So;

2^2 =4

In experiment 2 and 3

The concentration of reaction of H2 is doubled and the rate of reaction is doubled.

0.575/0.287 = 2

2^1 =2

So we can now write;

Rate =k[NO]^2 [H2]^1

Taking up the first reaction;

0.144 =k [0.475]^2 [0.411]

k = 0.144/ [0.475]^2 [0.411]

k = 1.553 M^2s^-1

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Equation: CH4 + 202 CO2 + 2H20
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Answer:

2:1

1.2 × 10² g

Explanation:

Step 1: Write the balanced combustion equation

CH₄ + 2 O₂ ⇒ CO₂ + 2 H₂O

Step 2: Establish the appropriate molar ratio

According to the balanced equation, the molar ratio of O₂ to CH₄ is 2:1.

Step 3: Calculate the moles of CH₄ required to react with 15 moles of O₂

We will use the previously established molar ratio.

15 mol O₂   1 mol CH₄/2 mol O₂ = 7.5 mol CH₄

Step 4: Calculate the mass corresponding to 7.5 moles of CH₄

The molar mass of CH₄ is 16.04 g/mol.

7.5 mol × 16.04 g/mol = 1.2 × 10² g

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3 years ago
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Explanation:

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Answer:

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Explanation:

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