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2 years ago

Explain the reaction of non-metals with oxygen

1 answer:

3 0

Non-metals and oxygen produce non-metal oxides. Such as sulphur dioxide and nitrogen oxide which are responsible for acidic rain. Hope this helps

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Filtration can separate a mixture of fine sand and coarse gravel. The holes in the filter should be large enough to allow ______

Charra [1.4K]

The sand to pass through, but not the gravel. Hope this helps!

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2 years ago

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Which of the following statements is true?

Lera25 [3.4K]

The statement which is true is

metals lose electrons to become cations

<u><em>Explanation</em></u>

metals tends to loss electrons to attain noble gas electrons configuration.
When metal loses electrons they form a positive charged ions.
The positively charged ion is known as cations.
for example sodium metal (Na) loses 1 electron to form a cation with a charge of positive 1 ( Na^+)

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3 years ago

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Which planet listed below will take the longest amount of time to orbit the sun?

Tema [17]

Answer:

Neptune takes the longest to orbit the sun because of it's distance away from the Sun.

Explanation:

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2 years ago

What is the number placed in front of a compound to balance a chemical reaction?

stiks02 [169]

coefficient: they balance the chemical equation you have to make sure the number is as small as it can. It is also used to convert different compounds to compounds or quantities to quantities.

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3 years ago

3.5g of a Certain compound X, known to be made of carbon, hydrogen, and perhaps oxygen, and to have a molecular molar mass of 15

shutvik [7]

Answer:

C₅H₁₀O₅

Explanation:

1. Calculate the mass of each element in 2.78 mg of X.

(a) Mass of C

$\text{Mass of C} = \text{5.13 g CO}_{2}\times \dfrac{\text{12.01 g C}}{\text{44.01 g }\text{CO}_{2}}= \text{1.400 g C}$

(b) Mass of H

$\text{Mass of H} = \text{2.10 g H$_{2}$O}\times \dfrac{\text{2.016 g H}}{\text{18.02 g H$_{2}$O}} = \text{0.2349 g H}$

(c) Mass of O

Mass of O = 3.5 - 1.400 - 0.2349 = 1.87 g

2. Calculate the moles of each element

$\text{Moles of C = 1400 mg C}\times\dfrac{\text{1 mmol C}}{\text{12.01 mg C }} = \text{116.6 mmol C}\\\\\text{Moles of H = 234.9 mg H} \times \dfrac{\text{1 mmol H}}{\text{1.008 mg H}} = \text{233.1 mmol H}\\\\\text{Moles of O = 1870 mg O} \times \dfrac{\text{1 mmol O}}{\text{16.00 mg O}} = \text{116 mmol O}$

3. Calculate the molar ratios

Divide all moles by the smallest number of moles.

$\text{C: } \dfrac{116.6}{116.6}= 1\\\\\text{H: } \dfrac{233.1}{116.6} = 1.999\\\\\text{O: } \dfrac{116}{116.6} = 1.00$

4. Round the ratios to the nearest integer

C:H:O = 1:2:1

5. Write the empirical formula

The empirical formula is CH₂O.

6. Calculate the molecular formula.

EF Mass = (12.01 + 2.016 + 16.00) u = 30.03 u

The molecular formula is an integral multiple of the empirical formula.

MF = (EF)ₙ

$n = \dfrac{\text{MF Mass}}{\text{EF Mass }} = \dfrac{\text{150 u}}{\text{30.03 u}} = 5.00 \approx 5$

MF = (CH₂O)₅ = C₅H₁₀O₅

The molecular formula of X is C₅H₁₀O₅.

8 0

3 years ago