What is your question? HIGH SCHOOL CHEMISTRY 5+3 pts To ensure that the air in the shuttle remains free of excess CO2, engineers test the air-purification system. They combine 1.000 × 103 g LiOH with 8.80 × 1 02 g CO2. The reaction produces 3.25 × 102 g H2O. What is the limiting reactants in this test reaction

Answers

Answer 1

Answer:

The balanced reaction is:

2LiOH + CO2 = Li2CO3 + H2O

We are given the amount of the reactants to be reacted. This will be the starting point of our calculations. To determine the limiting reactant, we convert the amounts from grams to moles.

1.000 × 10^3 g LiOH (1 mol / 25.95 g) = 38.54 mol LiOH

8.80 × 10^2 g CO2 ( 1mol / 44.01 g) = 20.00 mol CO2

From the balanced reaction, the molar ratio of the reactants is 2:1. This means that every two mole of lithium hydroxide, 1 mole of carbon dioxide is needed. It is clear that, from the given amounts, CO2 is the limiting reactant.

Answer 2

Answer:

CO2 is the limiting molecule.

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The process of a material going through a change of state from a gas to a liquid is called _____. melting freezing condensation vaporization

Answers

Condensation is the change in state of matter from gas to liquid.

The process of a material going through a change of state from a gas to a liquid is called _____.

condensation

Which volume of 2.0M NaOH(aq) is need to completely neutralize 24 milliliters of 1.0M HCl(aq)?(1) 6.0mL (2) 12mL (3) 24mL (4) 48mL

Answers

The answer is (2) 12mL. The reaction equation is NaOH + HCl = NaCl + H2O. So the mol number of NaOH is equal to HCl. The concentration of NaOH is twice of HCl so the volume of HCl is twice of NaOH.

What are the electrons is the outer shell of an atom called?What charge will elements in Group 2 form when they are involved in an ionic bond?

Answers

The answer to your first question is valence electrons. The answer to your second is positive.

8.00*10^-5 mol was diluted to 500ml what is the concentration in Mol/L?

Answers

Make sure all units are consistent. Convert ml to L first. (500ml = 0.5L). Then divide the mole by the volume which would result to 1.6*10^-4mol/L. This can also be expressed as interms of molarity (M). 1 M = 1 mol/L hence the final answer is 1.6*10^-4 M.

Answer : The concentration in mol/L is $1.6* 10^(-4)mol/L$

Explanation : Given,

Moles = $8.00* 10^(-5)mol$

Volume of solution = 500 mL

Formula used :

$\text{Concentration}=\frac{\text{Moles of solute}* 1000}{\text{Volume of solution (in mL)}}$

Now put all the given values in this formula, we get:

$\text{Concentration}=(8.00* 10^(-5)mole* 1000)/(500mL)=1.6* 10^(-4)mol/L$

Therefore, the concentration in mol/L is $1.6* 10^(-4)mol/L$

The chemical formula for emerald is Be3Al2(SiO3)6. An emerald can be described asa pure substance because it is a compound.
a pure substance because it is an element.
an impure substance because it is chemically combined.
an impure substance because it is a mixture.

Answers

Answer is: a pure substance because it is a compound.

Pure substance is made of only one type of atom or only one type of molecule, it has definite and constant composition with distinct chemical properties.

Emerald (beryl) is chemical compound (beryllium aluminium cyclosilicate) with the chemical formula Be₃Al₂(SiO₃)₆. Pure beryl is colorless.

An emerald can be described as an impure substance because it is a mixture. Therefore, option D is correct.

The chemical formula for emerald is Be₃Al₂(SiO₃)₆, indicating that it is a compound composed of beryllium (Be), aluminum (Al), and silicon (Si) atoms bonded to oxygen (O) atoms.

However, emeralds can also contain impurities or trace elements such as chromium (Cr) or vanadium (V), which give them their characteristic green color.

These impurities or trace elements are present in small amounts and are incorporated into the crystal structure of the emerald.

To learn more about the emerald, follow the link:

brainly.com/question/27913527

#SPJ6

CH₃OH(l) + CO(g) → CH₃CO₂H(aq) What mass in grams of CO would be required for the complete carbonylation of 14.35 grams of methanol to acetic acid?

Answers

CO has a molar mass of 44.01 g/mol, which means that 1 mole of CO weighs 44.01 grams.

We want to convert 14.35 grams of ethanol to acetic acid, so we need to know how many moles of ethanol there are. Let's first multiply the given mass of ethanol by its molar mass:

14.35 (g) x 32.06 (g/mol) = 45.85 mol

So, we have 45.85 moles of methanol. If methanol reacts with CO to produce acetic acid, we need to know how many moles of CO we need to use, based on the stoichiometry of the reaction. The reaction equation gives us a 2:1 ratio for CO and methanol:

2 CH₃OH(l) + CO(g) → CH₃CO₂H(aq)

So, for every mole of CH₃OH we react, we will need 0.5 mole of CO. Therefore, we need 23.92 moles of CO to convert all the methanol to acetic acid.

Using the mass of 1 mole of CO, we can convert moles of CO to grams:

23.92 (mol) x 44.01 (g/mol) = 1050.93 (g)

So, we need 1051 grams of CO to completely convert 14.35 grams of methanol to acetic acid.

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