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3 years ago

Which of the following reactions is an example of a single replacement reaction?

Chemistry

1 answer:

qwelly [4]3 years ago

4 0

Answer:

Explanation:

This is the only reaction where a element is displaced out of a solution and turn a soild, due to it been less reactive than the other causing its displacement The electrochemical series can be used as reference.

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What’s the fastest way to balance chemical equations

Anon25 [30]

Hey there!

The best way to balance chemical equations is to first start by balancing polyatomic ions such as OH and SO₄.

Next, balance other elements, but save elements that are by themselves for last, such as H₂ or Fe. Once you balance everything else you can do the ones by themselves, it's much easier.

Hope this helps!

6 0

3 years ago

What term best defines the process that occurs when nuclei combine to produce a nucleus with more mass?

bekas [8.4K]

I just answered your other question and wrote all the definitions of the terms. I would say this is probably refering to Fusion because you are fusing together more nuclei into one nucleus. Fusion= bringing separate things into one entity.

4 0

3 years ago

Read 2 more answers

A particular solution of NaOH has hydronium concentration of 4x10-9 M. what is the solution’s pH?

bearhunter [10]

Answer:

The pH of the solution is 8, 40-

Explanation:

The pH indicates the acidity or basicity of a substance. PH values between 0 and less than 7 indicate acidic solutions, 7 neutral and greater than 7 to 14 basic. It is calculated as

pH = -log (H30+)

pH= -log (4x10-9M)

8 0

3 years ago

What is the MOLAR heat of combustion of methane(CH₄) if 64.00g of methane are burned to heat 75.0 ml of water from 25.00°C to 95

melamori03 [73]

Answer:

-5.51 kJ/mol

Explanation:

Step 1: Calculate the heat required to heat the water.

We use the following expression.

$Q = c \times m \times \Delta T$

where,

c: specific heat capacity
m: mass
ΔT: change in the temperature

The average density of water is 1 g/mL, so 75.0 mL ≅ 75.0 g.

$Q = 4.184J/g.\°C \times 75.0g \times (95.00\°C - 25.00\°C) = 2.20 \times 10^{3} J = 2.20 kJ$

Step 2: Calculate the heat released by the methane

According to the law of conservation of energy, the sum of the heat released by the combustion of methane (Qc) and the heat absorbed by the water (Qw) is zero

Qc + Qw = 0

Qc = -Qw = -22.0 kJ

Step 3: Calculate the molar heat of combustion of methane.

The molar mass of methane is 16.04 g/mol. We use this data to find the molar heat of combustion of methane, considering that 22.0 kJ are released by the combustion of 64.00 g of methane.

$\frac{-22.0kJ}{64.00g} \times \frac{16.04g}{mol} = -5.51 kJ/mol$

8 0

3 years ago

What is the pH of 0.0001 M NaOH

Gnom [1K]

The pH of NaOH is 10

6 0

4 years ago