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Varvara68 [4.7K]
2 years ago
12

A compound is 150.86 g carbon, 8.86 g hydrogen, and 20.10 g oxygen by

Chemistry
1 answer:
Ivahew [28]2 years ago
8 0

Answer:

C20 H14 O2

Explanation:

Remark

This is a sample, which the question does not say and should. It is a fraction of 1 mole. So what you have to do is multiply the numbers given by x and equate it to 286.28

Equation

150,86* x + 8.86*x + 20.1*x  = 286.28

179.8x = 286.28

x = 286.26/179.8

x = 1.592

Now multiply the given numbers by 1.592

150.86 * 1.592 = 240.58

8.85 * 1.592 = 14.1

20.1 * 1.592 = 32

Rounding you get

240/12 = 20

14.1/1 = 14

32/16 = 2

C20 H14 O2

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Explanation:

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Explain how copper conducts electricity?
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Answer:

Copper is a metal made up of copper atoms closely packed together. As a result, the electrons can move freely through the metal. For this reason, they are known as free electrons. They are also known as conduction electrons because they help copper be a good conductor of heat and electricity.

Explanation:

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What the total charge of an atom with 8 protons 10 neutrons and 10 electrons?
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Suppose the flask is already at equilibrium but then the volume of the reaction flask is then reduced what will happen
sveta [45]

1) Answer is: c) The reaction will proceed right.

Balanced chemical reaction: N₂(g) + 3H₂(g) ⇄ 2NH₃(g) ΔH = +92 kJ.

Reducing the volume of the system increase the partial pressures of the products and reactants.

With a pressure increase due to a decrease in volume, the side of the equilibrium with fewer moles is more favorable, there are 4 moles at the left side (three moles of hydrogen and one mole of nitrogen) and 2 moles (ammonia) at the right side of the reaction.

2) Answer is: d) The partial pressure of ammonia will increase.

This reaction is endothermic (enthalpy is higher than zero), which means that heat is added.

According to Le Chatelier's principle when the reaction is endothermic heat is included as a reactant and when the temperature increased, the heat of the system increase, so the system consume some of that heat by shifting the equilibrium to the right,  producing more ammonia.

8 0
3 years ago
The rate constant k for a certain reaction is measured at two different temperatures temperature 376.0 °c 4.8 x 108 280.0 °C 2.3
9966 [12]

Answer:

The activation energy for this reaction = 23 kJ/mol.

Explanation:

Using the expression,

\ln \dfrac{k_{1}}{k_{2}} =-\dfrac{E_{a}}{R} \left (\dfrac{1}{T_1}-\dfrac{1}{T_2} \right )

Where,

k_1\ is\ the\ rate\ constant\ at\ T_1

k_2\ is\ the\ rate\ constant\ at\ T_2

E_a is the activation energy

R is Gas constant having value = 8.314×10⁻³ kJ / K mol  

k_2=2.3\times 10^8

T_2=280\ ^0C  

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

T(K) = T( °C) + 273.15  

So,  

T = (280 + 273.15) K = 553.15 K  

T_2=553.15\ K  

k_1=4.8\times 10^8  

T_1=376\ ^0C  

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

T(K) = T( °C) + 273.15  

So,  

T = (376 + 273.15) K = 649.15 K  

T_1=649.15\ K  

So,  

\left(\ln \left(\:\frac{4.8\times \:\:\:10^8}{2.3\times \:\:\:10^8}\right)\right)\:=-\frac{E_a}{8.314\times \:10^{-3}\ kJ/mol.K}\times \:\left(\frac{1}{649.15\ K}-\frac{1}{553.15\ K}\right)

E_a=-\frac{10^{-3}\times \:8.314\ln \left(\frac{10^8\times \:4.8}{10^8\times \:2.3}\right)}{-\frac{96}{359077.3225}}\ kJ/mol

E_a=-\frac{\frac{8.314\ln \left(\frac{4.8}{2.3}\right)}{1000}}{-\frac{96}{359077.3225}}\ kJ/mol

E_a=22.87\ kJ/mol

<u>The activation energy for this reaction = 23 kJ/mol.</u>

6 0
2 years ago
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