CHEMISTRY HIGH SCHOOL

What gas is removed from inhaled air

Answers

Answer 1

Answer:

ur answer is oxygen (O2)!!

Answer 2

Answer: What gas is removed from inhaled air?

oxygen (O2)

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Which of the following characteristics is not a property of an acid? Has a sour taste Accepts an H+ ion in reaction May cause damage to buildings, statues, and rivers Increases the concentration of hydronium ions in an aqueous solution

Answers

Answer : Option B) Accepts an H+ ion in reaction

Explanation : Acid is a lewis acid which forms a bond by accepting a pair of electrons. Acids, when dissolved increase the concentration of hydronium ion in the solution. So, the statement which is Acid accepts H+ ion is irrelevant here, as base accepts the H+ ion in a reaction.

Answer : The incorrect option is, Accepts an H⁺ ion in reaction.

Explanation :

Acid : It is a type of species which contains hydrogen ion.

Properties of an acid :

The taste of an acid is sour.

An acid does not feel slippery.

Acid reacts with the active metal to form a gas and a salt.

It change the color of litmus paper to red or pink.

It conduct electricity.

It react with carbonates to give salt.

It react with a metal to give compound and hydrogen gas.

Base : It is a type of species which contains hydroxide ion.

Properties of an base :

The taste of base is bitter.

The base feels slippery.

It does not react with the active metal.

It change the color of litmus paper to blue.

It conduct electricity.

As per question, all options are the properties of an acid while the statement accepts an H⁺ ion in reaction is in the property of an acid because it donates hydrogen ion in the solution.

Hence, the incorrect option is, Accepts an H⁺ ion in reaction.

Rutherford’s gold foil experiment provided evidence for which of the following statements?a. Negative and positive charges are spread evenly throughout an atom.
b. Alpha particles have a positive charge.
c. Gold is not as dense as previously thought.
d. There is a dense, positively charged mass in the center of an atom. Reset Selection

Answers

The answer is (c.) There is a dense, positively charged mass in the center of an atom
In 1899, Ernest Rutherford, a British physicist conducted a study of the absorption of radioactivity by thin sheets of metal foil. On this experiment, he concluded that all the positive charge and the mass of the atom is concentrated in a small fraction of the total volume of the atom which is called the Nucleus.

A sample of an iron ore is dissolved in acid, and the iron is converted to Fe2+. The sample is then titrated with 47.20 mL of 0.02240 M MnO4– solution. The oxidation-reduction reaction that occurs during titration is(a) How many moles of MnO4– were added to the solution? (b) How many moles of Fe2+ were in the sample?(c) How many grams of iron were in the sample? (d) If the sample had a mass of 0.8890 g, what is the percentage of iron in the sample?

Answers

Answer:

33.21% is the right answer.

Explanation:

0.04720 L * 0.02240 mol / L = 1.0573*10-3

mol Fe+2 = 1.0573* 10-3 mol = 5.2864*10-3

mass of Fe= 5.2864 * 10-3 = 0.29522g

% of Fe in sample = 0.29522 g Fe / 0.8890 g of sample * 100 = 33.21%

Final answer:

The number of moles of MnO4– added to the solution is 0.00106 mol. The moles of Fe2+ in the sample is 0.00530 mol. The grams of iron in the sample is 0.296 g and the percentage of iron in the sample is 33.33%.

Explanation:

The titration reaction between Fe2+ and MnO4– in acid solution is as follows: 5Fe2+ + MnO4– + 8H+ → 5Fe3+ + Mn2+ + 4H2O. Firstly, we can calculate the number of moles of MnO4– added to the solution using the formula volume X molarity. That is 0.0472 L X 0.02240 M = 0.00106 mol MnO4–. According to the balanced redox reaction, one mole of MnO4– reacts with five moles of Fe2+. Therefore, the moles of Fe2+ in the sample is 0.00106 mol MnO4– X 5 = 0.00530 mol Fe2+.

Next, we calculate the grams of iron in the sample. The molarmass of iron is approximately 55.85 g/mol, thus the grams of iron in the sample are 0.00530 mol Fe2+ X 55.85 g/mol = 0.296 g Fe2+. Finally, we find the percentage of iron in the sample by mass = (mass of iron in the sample / total mass of the sample) X 100%. Therefore, the percentage is (0.296 g / 0.8890 g) X 100% = 33.33%.

Learn more about Chemistry and Redox Reactions here:

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What is the total mass of 2.0 moles of diatomic hydrogen?

Answers

Explanation:

A diatomic molecule is defined as the molecule which contains two atoms.

For example, a $H_(2)$ molecule has two atoms of hydrogen.

Molar mass of a $H_(2)$ molecule is 2.0 g/mol. Therefore, calculate the mass of 2.0 moles of diatomic hydrogen as follows.

No. of moles = $\frac{mass}{\text{molar mass}}$

2.0 mol = $(mass)/(2.0 g/mol)$

mass = 1 g

therefore, we can conclude that total mass of 2.0 moles of diatomic hydrogen is 1 g.

diatomic hydrogen is written as H2 (2.02 grams H2) <------- if each hydrogen atom is 1.01 grams, then two hydrogen atoms are 2.02 grams 2.0 moles H2 X 2.02 grams H2 ------------- (divide to cancel moles) = 4.04 grams/mole H2 ÷ one mole = 4.04 grams H2

Answers

Two scientists wrote a paper detailing their research and conclusions and submitted it to a scientific journal. Several months later, they received the paper back from the publisher with many comments attached from several fellow scientists. It is either that they revise their study or replicate the study. Most scientists would revisit their work and the findings they had from their research. Most probable if they were successful and the comments of the publisher and the co-scientists were positive they could replicate the study to validate its accountability.

What type of substance reacts with limestone (CaCO3) and produces carbon dioxide gas?

Answers

Acids react with calcium carbonate and more specifically carbonate to form carbon dioxide. An acid will give protons to the carbonate anion to produce carbonic acid which then decomposes into carbon dioxide and water. I hope this helps. Let me know if anything is unclear.

In a bid to produce CO2 from CaCO3 Heat energy and acids(H2SO4) reacts with limestone (CaCO3) and produce carbon dioxide gas(CO2).

What type of substance reacts with limestone (CaCO3) and produces carbon dioxide gas?

Generally, the equation for the Chemical Reaction is mathematically given as,

CaCO3----->CaO +CO2

This is a decomposition reaction, it occurs when the reaction of heat energy reacts with CaCO3 in the atmosphere to produce CaO(s) +CO2(g).

Also

CaCO3(s) + H2SO4(aq) → CaSO4(s) + H2O(l) + CO2(g)

CaCO3 also reacts with acids to produce CO2 as shown in the balance equation above.

In conclusion, Acids and Heat energy reacts with limestone (CaCO3) and produce carbon dioxide gas.