Which gaseous element has the greatest density at stp n2 o2 cl2 f2?

Answers

Answer 1

Answer:

Density is an intensive property as it does not depend on the quantity of the substances Whereas mass and volume are extensive property. Therefore, Cl $_2$ is the only gaseous element has the greatest density at STP.

What is density?

Density tells about the compactness of the substances, how much dense is the substances in other words. Object that is more denser than water they just sink in the water.

Mathematically,

Density = Mass of the element ÷volume marked on the graduated cylinder

From formula we can see that density is directly proportional to molar mass of the given element. the increasing order of molar mass is N $_2$ < O $_2$ <F $_2$ <Cl $_2$ . The increasing order of density would be N $_2$ < O $_2$ <F $_2$ <Cl $_2$ .

Therefore, Cl $_2$ is the only gaseous element has the greatest density at STP.

To know more about density, here:

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Answer 2

Answer: 1 mole Cl2 will have a density of 71/22.4 gram per liter

In general 1 mole of any gas will have a density of (mol.mass)/22.4 gram per liter at STP

Answer : Electrons cannot exist in locations other than in specific orbits.

Explanation :

The emission spectrum of hydrogen shows discrete, bright, colored lines. The characteristic that the Bohr model supported with observation is that electrons cannot exist in location other than in specific orbits.

According to characteristics of Bohr's atomic model;

The energy levels of electrons are discrete, this is the reason which is shown by hydrogen emission spectrum as discrete, bright, colored lines.

Also, electrons are seen to orbit around the nucleus in orbits which has a set size and energy with a defined path.

Electrons can jump from one energy level to another, which results after absorbing or emitting an electromagnetic radiation with a frequency ν.

The characteristic of the Bohr model that would best support his observation is this assumption: "The energy of the electron in an orbit is proportional to its distance from the nucleus. The further the electron is from the nucleus, the more energy it has." The discrete, bright, colored lines might represent the electrons and its distance from the nucleus. The lights are caused by the energy it has.

Review the equation below. 2KClO3 mc012-1.jpg 2KCl + 3O2 How many moles of oxygen are produced when 2 mol of potassium chlorate (KClO3) decompose?

Answers

Stoichiometry of the reaction:

2 KClO₃   =   2 KCl + 3 O₂
  ↓ ↓

2 mole KClO₃ ----------> 3 mole O₂
2 mole KClO₃ ----------> ?

KClO₃ = 2 * 3 / 2

KClO₃ = 6 / 2

= 3 moles de KClO₃

hope this helps!

Answer:

the answer is 3

Explanation:

2 mol of potassium chlorate x $(3)/(2)$ = 3

also just did it on edge

In an experiment, 12.0 dm3 of oxygen, measured under room conditions, is used to burn completely 0.10 mol of propan-1-ol. What is the final volume of gas, measured under room conditions? A 7.20 dm3 B 8.40 dm3 C 16.8 dm3 D 18.00 dm3

Answers

The chemical reaction is

C3H8O + (9/2) O2 = 3CO2 + 4H2O

Theoretical amount of oxygen needed = 0.1 mol of propanol ( 4.5 mol O2 / 1 mol propanol) = 0.45 mol

The amount of oxygen used in mol can be calculated using the ideal gas equation

PV = nRT

@room conditions

P = 1 atm

T = 25C ~ 298 K

R = 0.08205 mol – L/ atm – K

1 dm3 = 1 L

(1 atm) (12 L) = n (0.08205)*(298K)

n = 0.49 mol O2

Excess O2 = 0.49 – 0.45 = 0.04 mol O2

Amount of CO2 produced = 0.1 mol propanol (3 mol CO2/ 1 mol propanol) = 0.3 mol

Amount of H2) produced = 0.1 mol propanol (4 mol H2O/ 1 mol propanol) = 0.4 mol

TOTAL amount of gases = 0.04 + 0.3 + 0.4 = 0.74 mol

Therefore

V = (0.74*0.08205*298)/1

V = 18.0 dm3, the answer is letter D

Answer:The the correct answer is option (A).

Explanation:

$2C_3H_7OH+9O_2\rightarrow 6CO_2+8H_2O$

12 L of oxygen gas burns 0.10 mol of propanol.(1 L = 1 $dm^3$ )

According to reaction, 2 moles of propanol gives 6 moles of $CO_2$ then, 0.10 moles of propanol will give: $(6)/(2)* 0.10$ moles of $CO_2$ that is 0.30 mol.

$n_(CO_2)=0.30 mol$

The final volume of the gas evolved after the reaction can be determined by Ideal gas equation. Since, the reaction is taking place at room temperature the value of pressure and temperature will be:

At room temperature:

Pressure = 1 atm

Temperature , T= 293 K

$PV=nRT$

$PV=n_(CO_2)RT$

$V_(CO_2)=(0.30 mol * 0.0821 L atm/mol K* 298 K)/(1 atm)=7.33 L=7.33 dm^3$

The closest answer from the given options is option (A) that is 7.20 $dm^3$

Under which conditions of temperature and pressure would a sample of H2(g) behave most like an ideal gas?(1) 0°C and 100 kPa
(2) 0°C and 300 kPa
(3) 150°C and 100 kPa
(4) 150°C and 300 kPa

Answers

3). 150°C and 100 kPa

Gases behave ideally at high temperatures and low pressures (less intermolecular forces)

Which is NOT an indicator of a chemical change? Heat or light is produced. State of matter changes. A new substance is formed. A gas is formed.

Answers

The choice that is not an indicator of a chemical change is "State of matter changes". More common than not, chemical reactions produce energy in the form of light or heat. Along with energy, they also produce a new substance called the product that could be in any state of matter (solid, gas, or liquid). Technically, a change in state is a physical change unless it also involves one of the other choices.

Answer:

State of matter changes.

Explanation:

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