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BabaBlast [244]
2 years ago
9

Molecules can be composed of ____. Select all that apply. … 1. two of more of the same atoms 2. two or more smaller molecules 3.

two or more different atoms 4.one or more particle plzzzzzz help me fast im giving 100 pts
Chemistry
2 answers:
docker41 [41]2 years ago
8 0

Answer:

1. two or more of the same atoms.

Explanation:

A molecule contains 2 identical atoms.

For example H2 is two molecules of hydrogen.

Remember, the 2 is in subscript.

kirill115 [55]2 years ago
8 0

Answer:

1. two or more of the same atoms

Explanation:

its the only one that makes sense

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What is the maximum number of grams of ammonia, nh3, which can be obtained from the reaction of 10.0 g of h2 and 80.0 g of n2? n
Lelechka [254]

<u>Answer:</u> The mass of ammonia produced is 28.22 g

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}     .....(1)

  • <u>For hydrogen gas:</u>

Given mass of hydrogen gas = 10.0 g

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1, we get:

\text{Moles of hydrogen gas}=\frac{10.0g}{2g/mol}=5mol

  • <u>For nitrogen gas:</u>

Given mass of nitrogen gas = 80.0 g

Molar mass of nitrogen gas = 28 g/mol

Putting values in equation 1, we get:

\text{Moles of nitrogen gas}=\frac{80.0g}{28g/mol}=2.86mol

The given chemical equation follows:

N_2+3H_2\rightarrow 2NH_3

By Stoichiometry of the reaction:

3 moles of hydrogen gas reacts with 1 mole of nitrogen gas

So, 5 moles of hydrogen gas will react with = \frac{1}{3}\times 5=1.66mol of nitrogen gas

As, given amount of nitrogen gas is more than the required amount. So, it is considered as an excess reagent.

Thus, hydrogen gas is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

3 moles of hydrogen gas produces 1 mole of ammonia

So, 5 moles of hydrogen gas will produce = \frac{1}{3}\times 5=1.66moles of ammonia

Now, calculating the mass of ammonia from equation 1, we get:

Molar mass of ammonia = 17 g/mol

Moles of ammonia = 1.66 moles

Putting values in equation 1, we get:

1.66mol=\frac{\text{Mass of ammonia}}{17g/mol}\\\\\text{Mass of ammonia}=(1.66mol\times 17g/mol)=28.22g

Hence, the mass of ammonia produced is 28.22 g

4 0
2 years ago
5. Rubbing alcohol is a commonly used disinfectant and has a cooling effect when applied to the skin. The active ingredient in r
WITCHER [35]

Answer:

Explanation:

70% (vol/vol) means

cotnaimns 70 %(vol/vol) 70 ml of isoprapnol is there in 100 ml of Rubbing sold alcohol.

if it is 200 ml then obvouly it has the 70*2 =140 ml of isoproanol  required.

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2 years ago
The amount of gas that occupies 36.52 L at 68.0°C and 672 mm Hg is __________ mol.
ASHA 777 [7]
We assume that this gas is an ideal gas. We use the ideal gas equation to calculate the amount of the gas in moles. It is expressed as:

PV = nRT
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n = 1.15 mol of gas

Hope this answers the question. Have a nice day.
7 0
2 years ago
Sulfur and oxygen react to produce sulfur trioxide. In a particular experiment, 7.9 grams of SO3 are produced by the reaction of
shutvik [7]

Answer:

  • <u>79%</u>

Explanation:

<u>1) Balanced chemical equation:</u>

  • 2S + 3O₂ → 2SO₃

<u>2) Mole ratio:</u>

  • 2 mol S : 3 mol O₂ : 2 mol SO₃

<u>3) Limiting reactant:</u>

  • Number of moles of O₂

        n = 6.0 g / 32.0 g/mol = 0.1875 mol O₂

  • Number of moles of S:

         n = 7.0 g / 32.065 g/mol = 0.2183 mol S

  • Ratios:

        Actual ratio: 0.1875 mol O₂ / 0.2183 mol S =0.859

        Theoretical ratio: 3 mol O₂ / 2 mol S = 1.5

Since there is a smaller proportion of O₂ (0.859) than the theoretical ratio (1.5), O₂ will be used before all S be consumed, and O₂ is the limiting reactant.

<u>4) Calcuate theoretical yield (using the limiting reactant):</u>

  • 0.1875 mol O₂ / x = 3 mol O₂ / 2 mol SO₃

  • x = 0.1875 × 2 / 3 mol SO₃ =  0.125 mol SO₃

<u>5) Yield in grams:</u>

  • mass = number of moles × molar mass = 0.125 mol × 80.06 g/mol =  10.0 g

<u>6) </u><em><u>Percent yield:</u></em>

  • Percent yield, % = (actual yield / theoretical yield) × 100
  • % = (7.9 g / 10.0 g) × 100 = 79%
6 0
2 years ago
Which choice below correctly completes the sentence? _______ reaches the Earth's surface through _______, then turns into ______
blondinia [14]

Answer:

d , before the molten rock becomes lava, it is first magma, and most people know that lava is ejected from volcanoes

4 0
2 years ago
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