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4 years ago

_____ is required to start a chemical reaction.

Chemistry

1 answer:

adelina 88 [10]4 years ago

5 0

Activation energy is the minimum energy needed for a particular reaction to occur.

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A metal coin has certain properties that can be measured if the coin were to go from earth to moon the coins will remain the sam

PtichkaEL [24]

Answer:

its matter

Explanation:

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3 years ago

A 4.80g piece of magnesium (Mg) displaces 2.76mL of water when it is placed in a graduated cylinder. What is the density of magn

AnnZ [28]

Answer:

Explanation:

The density of a substance can be found by using the formula

$density = \frac{mass}{volume} \\$

From the question we have

$density = \frac{4.80}{2.76} \\ = 1.73913...$

We have the final answer as

Hope this helps you

8 0

3 years ago

This guy wants to go to the movies with me to watch Avengers Endgame and it's 3 hours long, but he has a girlfriend, and me and

Thepotemich [5.8K]

Answer:

possibly but he could just think of you as a best friend because he has a gf

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4 0

4 years ago

Read 2 more answers

Given the following balanced equation, determine the rate of reaction with respect to [SO3]. If the rate of O2 loss is 3.56 x 10

Olenka [21]

Answer:

7.12 × 10⁻³ M/s

Explanation:

Step 1: Write the balanced reaction

2 SO₂ + O₂ ⇒ 2 SO₃

Step 2: Establish the appropriate molar ratio

According to the balanced equation, the molar ratio of O₂ to SO₃ is 1:2.

Step 3: Calculate the rate of formation of SO₃

The rate of loss of O₂ is 3.56 × 10⁻³ mol O₂/L.s. The rate of formation of SO₃ is:

3.56 × 10⁻³ mol O₂/L.s. × 2 mol SO₃/1 mol O₂ = 7.12 × 10⁻³ mol SO₃/L.s

7 0

3 years ago

Gallium oxide, Ga.Oy, forms when gallium is combined with oxygen. A 1.25 g of Ga is allowed to react with excess oxygen and 1.68

mrs_skeptik [129]

Answer : The chemical formula of a compound is, $Ga_2O_3$

Solution : Given,

Mass of gallium = 1.25 g

Mass of gallium oxide = 1.68 g

Mass of oxygen = Mass of gallium oxide - Mass of gallium

Mass of oxygen = 1.68 - 1.25 = 0.43 g

Molar mass of Ga = 69.72 g/mole

Molar mass of O = 16 g/mole

Step 1 : convert given masses into moles.

Moles of Ga = $\frac{\text{ given mass of Ga}}{\text{ molar mass of Ga}}= \frac{1.25g}{69.72g/mole}=0.0179moles$

Moles of O = $\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{0.43g}{16g/mole}=0.027moles$

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For Ga = $\frac{0.0179}{0.0179}=1$

For O = $\frac{0.027}{0.0179}=1.5$

The ratio of Ga : O = 1 : 1.5

To make in whole number we multiple ratio by 2, we get:

The ratio of Ga : O = 2 : 3

The mole ratio of the element is represented by subscripts in empirical formula.

The Empirical formula = $Ga_2O_3$

The empirical formula weight = 2(69.72) + 3(16) = 187.44 gram/eq

Now we have to calculate the molecular formula of the compound.

Formula used :

$n=\frac{\text{Molecular formula}}{\text{Empirical formula weight}}$

$n=\frac{187.44}{187.44}=1$

Molecular formula = $(Ga_2O_3)_n=(Ga_2O_3)_1=Ga_2O_3$

Therefore, the chemical of the compound is, $Ga_2O_3$

5 0

3 years ago