CHEMISTRY HIGH SCHOOL

In a sealed gas-liquid system at constant temperature, eventually...?there will be no more evaporation.

the rate of evaporation equals the rate of condensation.

the rate of condensation decreases to zero.

the rate of condensation exceeds the rate of evaporation.

Answers

Answer 1

Answer:

Let us study about it .

Explanation:

Evaporation

It is the process of converting liquid into vapors .

Condensation

It is the process of converting vapors back into liquid state .

Suppose if we have a sealed container and we are supplying it with no or little heat , we will see that as we increase heat , the particles starts moving faster .
When they move they also colloide and transfer energies .
The kinetic energies of certain molecule increase to an extent that they leave the other particles and escape in atmosphere .
That is evaporation occurs .At the same time when these vapors collide with each other or with the walls of container they get cooled and again get converted to liquid state .

It is seen that a equilibrium is reached when "rate of evaporation becomes equal to rate of condensation ".

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From what class(es) of elements is the following compound made? copper || chloride metal and metalloid
metal and nonmetal
metalloid and nonmetal
two metals

Answers

Answer: The correct answer is metal and non-metal.

Explanation:

Elements are mainly divided into 3 classes in the periodic table.

1.) Metals: The element which lie on the left side of the periodic table are mainly metals. These elements loose electron easily and form positively charged species. These elements are present in the highest proportion in the periodic table.

2.) Non-metals: The elements which lie on the right side of the periodic table are considered as non-metals. These elements gain electrons easily and form negatively charged species.

3.) Metalloids: These lie between metals and non-metals and show the properties of both metals and non-metals.

Copper lie in the period 4 and group 11 of the periodic table and it can easily loose electron and hence, it is considered as a metal.

Chlorine lie in the period 3 and group 17 of the periodic table and it can easily gain electron and hence, considered as a non-metal.

Therefore, the correct answer is metal and non-metal.

Metal and non metal because copper is a metal and chloride is a non metal

Copper, silver, and nickel are all classified as

Answers

Answer: currency

Explanation:

What subatomic particle(s) is/are located in the nucleus of the atom? Protons only

Electrons only

Protons and neutrons

Protons and electrons

Answers

Protons and neutrons!

Which statement describes the particles of an ideal gas based on the kinetic molecular theory?(1) The gas particles are relatively far apart and have negligible volume.
(2) The gas particles are in constant, nonlinear motion.
(3) The gas particles have attractive forces between them.
(4) The gas particles have collisions without transferring energy.

Answers

The particles are in a constant nonlinear motion.

A. They are far apart and have negligible volume. This makes it easier to calculate certain quantities such as temperature, pressure, and volume. If the gas particle volume is added, then the complex van der Waals equation has to be used to calculate these same quantities. We also assume that they are far apart because this implies that they will not collide.

Which type of stoichiometric calculation does not require the use of the molar mass?

Answers

The choices can be found elsewhere and as follows:

a. mass-mass problems
b. mass-volume problems
c. mass-particle problems
d. volume-volume problems

I believe the correct answer is option D. It is volume-volume problems that does not require the use of molar mass. Here you are dealing with molarities and volumes to determine concentrations. Molar mass is not part of any calculations.

Final answer:

The type of stoichiometric calculation that does not require the use of the molar mass is a calculation involving molar or stoichiometric ratios which are derived directly from the coefficients in a balanced chemical equation.

Explanation:

In stoichiometry, there are several types of calculations that can be performed. However, the type of stoichiometric calculation that does not require the use of the molar mass is the calculation involving the molar ratio, or stoichiometric ratio. This refers to the ratio of coefficients in a balanced chemical equation, which we use to determine the relative amounts of each substance involved in a chemical reaction.

An example of this is a balanced equation for the formation of water: H2 + 0.5O2 -> H2O. In this equation, the molar or stoichiometric ratio of hydrogen (H2) to oxygen (O2) to water (H2O) is 2:1:2. If we are given the number of moles of one substance, we can use this molar ratio to find the number of moles of any other substance in the equation, without needing to know their molar masses. This constitutes a stoichiometric calculation without the need for molar mass.

Learn more about Stoichiometric Calculations here:

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How can we determine the atomic mass of an element which posseses isotopic forms?

Answers

Answer: Here are the steps to determine the atomic mass of an element with isotopic forms:

1. Identify the isotopes: Determine the different isotopic forms of the element. Isotopes are atoms of the same element that have different numbers of neutrons but the same number of protons.

2. Determine the relative abundance: Find the relative abundance of each isotope. This information is typically given as a percentage or decimal. The relative abundance represents the proportion or percentage of each isotope in a naturally occurring sample of the element.

3. Obtain the mass of each isotope: Identify the mass of each isotope. This is usually given in atomic mass units (u) or grams per mole (g/mol).

4. Multiply the mass of each isotope by its relative abundance: Multiply the mass of each isotope by its relative abundance (expressed as a decimal). This calculates the contribution of each isotope to the overall atomic mass.

5. Sum the contributions: Add up the contributions of each isotope to obtain the atomic mass. This sum represents the weighted average of the masses of all the isotopic forms, taking into account their relative abundance.

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