Which of the following is TRUE about limiting and excess reactants?
A
The reactant that has the largest given mass will be the excess reactant
B. The excess reactant will be completely consumed after the reaction is complete.
CO The limiting reactant determines the maximum amount of product that can be formed,
D
Some of the limiting reactant is left over after the reaction is complete,

Balanced equation: C₂H₄ + 3O₂ → 2CO₂ + 2H₂O

O₂ required: 3/1 x moles C₂H₄ = 3/1 x 6.51 = 19.53 moles

Answer:

Polonium-207

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The amount of W(OH)2 needed would be 448.126 g

From the equation of the reaction:

W(OH)2 + 2 HCl → WCl2 + 2 H2O

The mole ratio of W(OH)2 to HCl is 1:2

Mole of 150g HCl = 150/36.461

                                 = 4.11 moles

Equivalent mole of W(OH)2 = 4.11/2

                                           = 2.06 moles

Mass of 2.06 moles W(OH)2 = 2.06 x 217.855

                                                = 448.188g

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Answer:

I don't know how to do right now

The pressure of the carbon dioxide that is allowed to sublime in atm, is 2.463 atm

The pressure of the gas can be obtained by using the ideal gas equation as illustrated below:

PV = nRT

P × 1 = 0.1 × 0.0821 × 300

P = 2.463 atm

Thus, the pressure of the gas is 2.463 atm

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Answer:

the energy possessed by a body by its value of its position relative to others, stresses within itself, electric charge, and other factors.

Explanation:

Answer:

4s

4p

4d

4f

these are the four quantum numbers

Answer:

the answer is I'm pretty that it's

Explanation:

Ur Wellcome

Hope it helps ~

Answer:

a. Calcium

Explanation:

Strontium and Calcium are both in the same group, Group 2.

Answer:

Calcium and strontium are in the same group.

Group 2a of the perodic table are the alkaline earth metals

Answer:

4.4 × 10^-7

3 × 10^5

Explanation:

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Answer:

The  percent  composition  of barium  in  barium chloride   is 65.9%

Explanation:

percent   composition  =  molar weight  of barium/molar weight  of barium chloride  x 100

from  periodic table the molar weight of barium = 137.3

and the  molar weight  of   BaCl2  = 137.3 +( 35.5 x 2)=208.3

% composition  is therefore = 137.3/208.3 x 100=65.9%

Answer:

Which of the following is NOT a property of Alkali Metals?

A) They form ions with a charge of +2.

B) They are lustrous.

C) They are extremely reactive with water.

D) They are good conductors of heat and electricity. Previous

Explanation:

The Answer is D.

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hi these are the answers :)

Answer:

Carbon monoxide is harmful when breathed because it displaces oxygen in the blood and deprives the heart, brain and other vital organs of oxygen. Large amounts of CO can overcome you in minutes without warning — causing you to lose consciousness and suffocate.

please please please please please please

Answer:

the more hydrogen ions present, the lower the pH; conversely, the fewer hydrogen ions, the higher the pH.

Answer:

1)

[tex]24 \times 60 \times 60 \\ 86400[/tex]

STP (Standard Temperature and Pressure):

At STP, 1 mole of an ideal gas will occupy a volume of 22.4 liters (Note: the new defined STP volume is 22.7 liters).

The volume is 77 L .

3 moles of oxygen at STP will occupy a volume of 3×22. 4=67. 2 L.

1.5 moles of oxygen at stp = 22.4 x 1.5 = 33.6 litres.

Therefore , number of moles of oxygen is : Now , we know volume of 1 mole of gas at S.T.P is 22.4 liters . Therefore , volume of 0.1 mole of oxygen at S.T.P is : Therefore , the volume of 3.2 gram atom of oxygen at S.T.P is 2.24 liters .

Helium is the largest, so that’s going to have the largest volume. Because at STP, volume was going to be equivalent to moles of gas.

Therefore, chemists introduced the concept of molar volume. Molar volume of a gas is defined as the volume of one mole of the gas. Thus, the molar volume is also the volume occupied by 6.02 x 1023 particles of gas. The molar volume of any gas is 22.4 dm3 mol–1 at STP or 24 dm3 mol–1 at room conditions.

oxygen gas

One mole of oxygen gas occupies 22.4 l volume at STP.

67.2 liters

The answer depends on the temperature and pressure. If the gas is at STP, THE 1 mole is 22.4 liters. 3 moles x 22.4 L/mol = 67.2 liters.

Well, assuming that the hydrogen gas is contained at STP , then the molar volume would be 22.7⋅3=68.1 L .

0.5 moles⋅22.4 L/mol=11.2 L , and so on.

The molar volume of any gas at S.T.P. is 22.4L .

So, the volume of an ideal gas is 22.41 L/mol at STP. This, 22.4 L, is probably the most remembered and least useful number in chemistry.

At STP, one mol of Ideal Gas occupies 22.4 L and one mmol of Ideal Gas occupies 22.4 mL.

Answer:

A. 22.41

Explanation:

goodluck man, just typing a little bit more for the 20 words

Answer:

22.4liters

Explanation: I did it in a quiz.

Answer:

100grams

Explanation:

law of conservation of mass

if the chemical or whatever, quantity is given then it stay the same in the beginning and the end. Just add them in the end and if something is missing that means you have done something wrong i am just telling for experiment

Answer:

A

Explanation:

Mixing chemicals does not always lead to a chemical change.

Mixing chemicals always leads to a chemical change would not provide the student with evidence that a chemical reaction has occurred.

In a chemical reaction, one or more substances also known as reactants are changed into one or more additional substances also known as products. Chemical elements or chemical compounds make up substances.

When substances or compounds undergo a chemical transformation to create new substances or compounds, a chemical reaction takes place. Chemical equations use symbols and the chemical formulae of the molecules involved in the reaction to express chemical processes.

Cells, animals, people, and insects may all grow, develop, reproduce, and adapt thanks to chemical processes.

Thus, option A is correct.

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Answer:

The change from a liquid phase to a gaseous phase.

so the answer would be it changed to a gaseous phase

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This is what occurs when the vapor pressure of the liquid is equal to the atmospheric pressure exerted on the liquid.

Answer:

2 Gc + 1 Mm + 3 Ch → 1 Gc2MmCh3

Note:

is this the s'more reaction?

-If not might there be a typo?

- if so, might it be one of these?

Answer: When two light bulbs are connected in parallel, which is true? A. The total resistance is less than the resistance of either bulb alone. B. The Voltage provided

Explanation:

Answer:

D. Only the top two bulbs would be lit.

Explanation:

When you connect the top light bulb, both the top and middle light bulbs will be lit. But, the bottom light bulb will not be lit because it is not connected. In order for a light bulb to be lit, it has to be connected on both sides by wire.

< Hope this helps! :)

This question is asking for the pH of a buffer solution between ammonia and nitric acid, with given volumes and concentrations. At the end, the result turns out to be 10.488.

In chemistry, buffers are known as substances attempting to hold a relatively constant pH by mixing and acid and a base (weak and strong). In such a way, for the substances given, the first step will be to calculate the consumed moles as they are mixed:

[tex]n_{NH_3}=0.1L*0.1mol/L=0.01mol\\\\n_{HNO_3}=0.09L*0.1mol/L=0.009mol[/tex]

Now, since ammonia is in a greater proportion, one can calculate how much of it is left after being consumed by the nitric acid:

[tex]n_{NH_3}^{left}=0.01mol-0.009mol=0.001mol[/tex]

And its new concentration:

[tex][NH_3]=\frac{0.001mol}{0.1L+0.09L} =0.00526M[/tex]

Next, with ammonia's ionization:

[tex]NH_3+H_2O\rightleftharpoons NH_4^++OH^-[/tex]

We set up the equilibrium expression based on ammonia's Kb:

[tex]Kb=\frac{[NH_4^+][OH^-]}{[NH_3]}[/tex]

Which can be solved by introducing x and using ammonia's Kb:

[tex]1.8x10^{-5}=\frac{x^2}{0.00526M}\\ \\[/tex]

Then, we solve for x which is also equal to the concentration of ammonium and hydroxide ions in the solution:

[tex]x=\sqrt{0.00526*1.8x10^{-5}}=0.000308M[/tex]

Ultimately, we calculate the pOH and then turn it into pH with:

[tex]pOH=-log(0.00308)=3.512\\\\pH=14-3.512=10.488[/tex]

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Answer:

12, 12, 12, edge 2022!

Explanation:

Answer:

How many electrons does the iron half-reaction lose? 12

How many electrons does the oxygen half-reaction gain? 12

What is the total number of electrons that are moved in this oxidation-reduction reaction? 12

Answer:

there are 4 moles in 223.2 g Iron (Fe)