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alexandr1967 [171]
3 years ago
10

As a pendulum swing from its highest to its lowest position along an arc, what happens to its kinetic energy and potential energ

y
A. Both the potential energy and kinetic energy decrease

B. The potential energy decreases while the kinetic energy increases

C. The kinetic energy decreases while the potential energy increases

D. Both the potential energy and kinetic energy increase
Chemistry
1 answer:
Hatshy [7]3 years ago
5 0

Answer:

B.The potential energy decreases while the kinetic energy increases.

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Analysis of a gaseous chlorofluorocarbon, CClxFy, shows that it contains 11.79% C and 69.57% Cl. In another experiment, you find
uranmaximum [27]

Answer:

The molecular formula = C_2Cl_{4}F_2

Explanation:

Moles =\frac {Given\ mass}{Molar\ mass}

% of C = 11.79

Molar mass of C = 12.0107 g/mol

<u>% moles of C = 11.79 / 12.0107 = 0.9816</u>

% of Cl = 69.57

Molar mass of Cl = 35.453 g/mol

<u>% moles of Cl = 69.57 / 35.453 = 1.9623</u>

Given that the gaseous chlorofluorocarbon only contains chlorine, flourine and carbon. So,

% of F = 100% - % of C - % of C = 100 - 11.79 - 69.57 = 18.64

Molar mass of F = 18.998 g/mol

<u>% moles of F = 18.64 / 18.998 = 0.9812</u>

Taking the simplest ratio for C, Cl and F as:

0.9816 : 1.9623 : 0.9812

= 1 : 2 : 1

The empirical formula is = CCl_2F

Also, Given that:

Pressure = 21.3 mm Hg

Also, P (mm Hg) = P (atm) / 760

Pressure = 21.3 / 760 = 0.02803 atm

Temperature = 25 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T = (25 + 273.15) K = 298.15 K  

Volume = 458 mL  = 0.458 L (1 mL = 0.001 L)

Using ideal gas equation as:

PV=nRT

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

0.02803 atm × 0.458 L = n × 0.0821 L.atm/K.mol × 298.15 K  

⇒n = 0.00052445 moles

Given that :  

Amount  = 0.107 g  

Molar mass = ?

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

0.00052445= \frac{0.107\ g}{Molar\ mass}

Molar\ mass= 204.0233\ g/mol

Molecular formulas is the actual number of atoms of each element in the compound while empirical formulas is the simplest or reduced ratio of the elements in the compound.

Thus,  

Molecular mass = n × Empirical mass

Where, n is any positive number from 1, 2, 3...

Mass from the Empirical formula = 1×12.0107 + 2×35.453 + 1×18.998 = 101.9147 g/mol

Molar mass = 204.0233 g/mol

So,  

Molecular mass = n × Empirical mass

204.0233 = n × 101.9147

⇒ n = 2

<u>The molecular formula = C_2Cl_{4}F_2</u>

6 0
3 years ago
A certain food web is made up of turtles, pond weeds, water fleas, and tadpoles. Which organism is most likely the producer in t
Simora [160]
The pond weeds are the producers because they are a plant
6 0
2 years ago
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.....................jsjkakmnak
cluponka [151]

Answer:

i can relate

Explanation:

6 0
3 years ago
What is an atomic number? An atomic mass?
mrs_skeptik [129]

Answer:

The atomic number is the number of the elements inside the periodic table and the mass is the weight or a number under the elements.

Explanation:

Correct me if I am wrong

4 0
3 years ago
Read 2 more answers
Draw the structure of a compound with the molecular formula C9H10O2 that exhibits the following spectral data. (a) IR: 3005 cm-1
Nikitich [7]

Answer:

The answer is 3-Phenylpropanoic acid (see attached structure)

Explanation:

From spectral data:

3005 cm-1 ⇒ carboxylic acid (broad band)

1670 cm-1 ⇒ C=C

1603 cm-1 ⇒ Aromatic C-C bond

H NMR frequency at 2.6 ppm, singlet, ⇒ OH with no surrounding protons, possible deshielding  (clearer investigation of  spectrum would be expedient).

Hence, our C9H10O2 compound has an aromatic ring and carboxylic acid group attached to it.

7 0
3 years ago
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