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3 years ago

15

What must happen in a chemical reaction? A. Energy is created B. Energy is transferred. C. Atoms are destroyed. D. Energy is des

troyed

2 answers:

Elanso [62]3 years ago

8 0

D because an explosion is a chemical reaction the creates energy then destroys it

rewona [7]3 years ago

5 0

C is the correct answer.

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at constant atmospheric pressure, the temperature of a gas that occupies the volume of 5.30 L is 298 K. what is the temperature

harkovskaia [24]

Answer:

The new temperature of the gas is 427K

Explanation:

In this case we use Charles's Law according to which the volume and temperature of a certain amount of gas are related, keeping the pressure constant.

V1 / T1 = V2 / T2

5,30L/298K=7,60L/T2

T2=7,60L/(5,30L/298K)=427,32K

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3 years ago

The distance from the top of one sound wave to the top of the next sound wave is called a (n)

Vikki [24]

Answer:

The answer is wavelength

Explanation:

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3 years ago

Calculate the number of c h and o atoms in 1.50g of glucose (c6h12o6) a sugar

goldfiish [28.3K]

Total number of atoms is 5.016×10²¹ Carbon and oxygen states 3.01×10²³ respectively, while hydrogen 6.02×10²³

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4 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

4 years ago

Which statement correctly describes electrochemical cells?

hoa [83]

Answer: C. Electrochemical cells involve oxidation-reduction reactions.

Explanation: Oxidation occurs at the anode, and reduction occurs at the cathode.

3 0

3 years ago