The formula C2H4 can be described as

Answers

Answer 1

Answer: C2H4 is Ethylene. Ethylene is a simple hydrocarbon alkaline.

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Which element has atoms that can bond with each other to form long chains or rings?(1) carbon (3) oxygen
(2) nitrogen (4) fluorine

Answers

The correct answer is option 1. It is the carbon (C) atom that can bond with each other to form ring and chain structures in compounds. These ring and chain structures and compounds are called organic compounds. Chain structures include alkanes, alkenes, alkynes. Ring structures include cyclic hydrocarbons and aromatic hydrocarbons.

Answer: Option (1) is the correct answer.

Explanation:

Carbon atoms are able to combine with its atoms resulting in formation of long chains. This property of carbon is known as catenation. Whereas carbon atom also has the property to combine with other atoms and results in the formation of long chains or rings.

On the other hand, oxygen, nitrogen, and fluorine does not form long chains or rings.

Thus, we can conclude that carbon is the element whose atoms can bond with each other to form long chains or rings.

[05.03]What is the pressure, in mm Hg, of 2.50 moles of an ideal gas if it has a volume of 50.0 liters when the temperature is 27.0° C?84.2 mm Hg 289 mm Hg 617 mm Hg 936 mm Hg

Answers

Assuming ideal gas law applies to the problem, we find the pressure from the given volume, temperature and number of moles. The ideal gas equation is PV=nRT. R is 0.0821 L atm/ mol K. Substituting the data given, P= (2.50 moles)(0.0821 L atm/ mol K)(27+273 K)/(50 L)= 1.2315 atm. This is equivalent to 936 mm Hg.

a. How much energy is needed to raise the temperature of a 75 g sample of aluminum from 22.4°C to 94.6°C?

Answers

To calculate the energy required to raise the temperature of a substance, you can use the formula:

Q = m * c * ΔT

Where:
Q is the energy (in joules)
m is the mass of the substance (in grams)
c is the specific heat capacity of the substance (in joules per gram-degree Celsius)
ΔT is the change in temperature (in degrees Celsius)

For aluminum, the specific heat capacity is approximately 0.897 J/g°C.

Given:
Mass of aluminum (m) = 75 g
Specific heat capacity of aluminum (c) = 0.897 J/g°C
Change in temperature (ΔT) = 94.6°C - 22.4°C = 72.2°C

Substituting the values into the formula:

Q = 75 g * 0.897 J/g°C * 72.2°C

Calculating the result:

Q = 4846.35 J

Therefore, approximately 4846.35 joules of energy are needed to raise the temperature of a 75 g sample of aluminum from 22.4°C to 94.6°C.

Introduction:

Understanding the amount of energy required to change the temperature of a substance is fundamental in many fields, from chemistry and physics to engineering and everyday applications. In this case, we're looking at how much energy it takes to heat a 75 g sample of aluminum.

Specific Heat Capacity of Aluminum:

To determine the energy required, we first need to consider the specific heat capacity of aluminum. The specific heat capacity (c) is a unique property of each material and represents the amount of heat energy needed to raise the temperature of 1 gram of that substance by 1 degree Celsius (or 1 Kelvin). For aluminum, the specific heat capacity (c) is approximately 0.897 J/g°C (joules per gram per degree Celsius).

Mass of the Sample:

The next piece of the puzzle is the mass of the aluminum sample. You mentioned that it's 75 grams, so we'll use that value in our calculations.

Change in Temperature:

We're looking to raise the temperature of the aluminum from 22.4°C to 94.6°C. To find the change in temperature (ΔT), we subtract the initial temperature from the final temperature:

ΔT = 94.6°C - 22.4°C = 72.2°C

Calculating the Energy:

Now, we can use the specific heat capacity formula to calculate the energy (Q) needed to raise the temperature of the aluminum sample:

Q = m * c * ΔT

Where:

Q is the energy in joules (J).

m is the mass of the sample (75 g).

c is the specific heat capacity of aluminum (0.897 J/g°C).

ΔT is the change in temperature (72.2°C).

Plugging in these values:

Q = 75 g * 0.897 J/g°C * 72.2°C

Q ≈ 4863.15 J

Conclusion:

Therefore, approximately 4863.15 joules of energy are needed to raise the temperature of a 75 g sample of aluminum from 22.4°C to 94.6°C. This calculation is essential in various scientific and practical applications, from cooking to materials engineering, and helps us understand the energy requirements for temperature changes in different substances.

50 grams of acetic acid C2H4O2 are dissolved in 200 g of water. Calculate the weight % and mole fraction of the acetic acid in the solution

Answers

$50g$ $of$ $C_2H_4O_2$ $in$ $200g$ $H_2O$

so:

$(50)/(200+50)+100\%= (50*100)/(250)\%=20\%$

$MW of acid = 2*C+4*H+2*O = 2*12+4*1+2*16=$

$=24+4+32=60g/mol$

so:

$(50g)/(60g/mol)\approx0.83moles$

it means that

in $50g$ of acid there is $\approx0.83$ moles of acid

$MW of H_2O = 2*H+O=2*1+16=2+16=18g/mol$

so:

$(200g)/(18g/mol)\approx11.11moles$

it means that:

in $200g$ of water there is $\approx11.11$ moles of water

therefore:

$(0.83mol)/(11.11mol+0.83mol)= (0.83mol)/(11.94mol)=0.069$

So your answers are:

$20\%$

and the mole fraction is:

$0.069$

What’s the easiest way to add energy to matter

Answers

Answer:

The easiest way is to heat matter which raises its internal energy andso the mass as well. Another possibility is to accelerate matter as in case of protons or heavy ions in the LHC, Protons ,for example , are accelerated to the energies of 6500 GeV which means increase of the rest mass by a factor of almost 7000

At equilibrium, a sample of gas from the system is collected into a 4.00 L flask at 600 K. The flask is found to contain 3.86 g of PCl₅, 12.7 g of PCl₃, and 13.3 g of Cl₂. What are the values of Kc and Kp for this reaction?