Rubber gloves and other chemical resistant protective clothing are necessary when handling concentrated ammonium hydroxide.
Why it is necessary to handle concentrated solution of ammonium hydroxide with care ?Ammonia is an irritant and corrosive to the skin, eyes, respiratory tract and mucous membranes. May cause severe chemical burns to the eyes, lungs and skin.The extent of injury produced by exposure to ammonia depends on the duration of the exposure, the concentration of the liquid or vapor and the depth of inhalation.
Hence, Rubber gloves and other chemical resistant protective clothing are necessary when handling concentrated ammonium hydroxide.
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Chromium (III) oxide reacts with hydrogen sulfide gas to form chromium (III) sulfide and water. To produce 421 g of cr2s3, how many moles of cr2o3 and grams of cr2o3 are required?
Cr₂O₃ ( s ) + 3H₂S ( g ) → Cr₂S₃ ( s ) + 3H₂O ( l )
mol Cr₂S₃ = 421 : 200.19 g/mol = 2.103
mol Cr₂O₃ ≈ mol Cr₂S₃ = 2.103 ( equivalent coefficient)
mass Cr₂O₃ = 2.103 x 151.99 g/mol = 319.63 gr
The physical matter of which living or nonliving things are composed is called a ___
(Fill in the blank one word)
100 POINTS TO WHO EVER IS CORRECT!
Answer:
Substance
Explanation:
Any physical matter despite of living or non living things are composed by a set of molecules or atoms commonly known as substance
On specific living things are composed of biomolecules or cells where as non living things are composed of molecules and atoms
Answer:
Substances
Physical matters are divided into 3 states
solid stateLiquid stateGaseous stateAs per randomness of particles the order is
Gaseous>Liquid>SolidA
Calculate the number of C atoms in 0.524 mole of C.
B
Calculate the number of SO2 molecules in 9.87 moles of SO2
C
Calculate the moles of Fe in 1.40x10^22 atoms of Fe
D
Calculate the moles of C2H6O in 2.30x10^24 molecules of C2H6O
The number of C atoms in 0.524 moles of C is 3.15 atoms.
The number of [tex]SO_2[/tex] molecules in 9.87 moles [tex]SO_2[/tex] is 59.43 molecules.
The moles of Fe in 1.40 x [tex]10^{22}[/tex] atoms of Fe is 0.23 x [tex]10^{-1}[/tex]
The moles of [tex]C_2H_6O[/tex] in 2.30x[tex]10^{24}[/tex] molecules of [tex]C_2H_6O[/tex] is 3.81.
What are moles?A mole is defined as 6.02214076 × [tex]10^{23}[/tex] of some chemical unit, be it atoms, molecules, ions, or others. The mole is a convenient unit to use because of the great number of atoms, molecules, or others in any substance.
A. The number of C atoms in 0.524 mole of C:
6.02214076 × [tex]10^{23}[/tex] x 0.524 mole
3.155601758 atoms =3.155 atoms
B. The number of [tex]SO_2[/tex] molecules in 9.87 moles of [tex]SO_2[/tex]:
6.02214076 × [tex]10^{23}[/tex] x 9.87
59.4385293 molecules= 59.43 molecules
C. The moles of Fe in 1.40 x [tex]10^{22}[/tex] atoms of Fe:
1.40 x [tex]10^{22}[/tex] ÷ 6.02214076 × [tex]10^{23}[/tex]
0.2324754694 x [tex]10^{-1}[/tex] moles.
0.23 x [tex]10^{-1}[/tex] moles.
D. The moles of [tex]C_2H_6O[/tex] in 2.30x[tex]10^{24}[/tex] molecules of [tex]C_2H_6O[/tex]:
2.30x[tex]10^{24}[/tex] ÷ 6.02214076 × [tex]10^{23}[/tex]
3.819239854 moles=3.81 moles
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Hydrogen and iodine vapour exist in equilibrium with hydrogen iodide at a constant temperature in a gas syringe.
H2 + I2
2HI
Which of the following will increase when the pressure is increased at constant temperature? [Assume that the mixture shows ideal behavior.]
The pressure has no effect on the equilibrium constant.
What is Equilibrium ?Equilibrium is a state when the forward reaction rate is equal to the backward reaction rate .
The equation given is
H₂ + I₂ ⇄ 2HI
The Equilibrium constant depends only upon temperature and nature of reaction ,
It is independent of catalyst presence , initial concentration of reactants,and pressure.
The pressure has no effect on the equilibrium constant.
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Select the correct answer.
In a given chemical reaction, the energy of the products is greater than the energy of the reactants. Which statement is true for this reaction?
A. Energy is absorbed in the reaction.
B. Energy is released in the reaction.
C. No energy is transferred in the reaction.
D. Energy is created in the reaction.
E. Energy is lost in the reaction.
Which data are shown on topographic maps?
Answer:
Topographic maps generally shows Natural features such as Rivers and Lakes.
sometimes they also show some features made by humans like brodges, elevations etc.
Answer:
Topographic maps show contours, elevation, forest cover, marsh, pipelines, power transmission lines, buildings, and various types of boundary lines such as international, provincial, and administrative, and many others.
please give me brainliest
Under which conditions of temperature and pressure, the real gas behave ideally?
Answer:
A real gas will act as an ideal gas under high temperature and at a low pressure.
Real gases are non-ideal gases whose molecules occupy space and have interactions, consequently, they do not adhere to the ideal gas law.
An ideal gas has molecules that occupy negligible space and have no interactions, and which consequently obeys the gas laws exactly.
Explanation:
25. What is the equilibrium constant expression for the following? 2Hg (g) + O₂(g) → 2HgO (s) A. K= [Hg] [0₂]. B. K= [HgO]/([Hg]²[0₂]) M C. K=[2HgO]/([2Hg][0₂]). D. K=1/([Hgl [02]) 25. What is the equilibrium constant expression for the following ? 2Hg ( g ) + O₂ ( g ) → 2HgO ( s ) A. K = [ Hg ] [ 0₂ ] . B. K = [ HgO ] / ( [ Hg ] ² [ 0₂ ] ) M C. K = [ 2HgO ] / ( [ 2Hg ] [ 0₂ ] ) . D. K = 1 / ( [ Hgl [ 02 ] )
Answer:
2 Hg (g) + o2 ---> 2 H2o
equilibrium constant
K = (c) (d) / (a)(b)
K= ( H2o)²/(He) ²(o2)
Explain how to get it Thanks
The Ammonia present in 2.5 mole of Ammonia is 42.5grams.
What is a mole ?A mole is a measuring unit in Chemistry to measure the number of atoms in certain molar mass of a substance.
It is given that 2.5 mole of Ammonia is present
Grams of Ammonia present in 2.5 mole of Ammonia = ?
Molecular weight of Ammonia = 17 grams.
1 mole of Ammonia = 17 grams of Ammonia
2.5 mole of Ammonia = 17 * 2.5
= 42.5 grams
Therefore 42.5 grams of Ammonia is present in 2.5 mole of Ammonia.
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How many grams of solid barium sulfate form when 32.0 mL of 0.160 M barium chloride reacts with 70.0 mL of 0.065 M sodium sulfate? Aqueous sodium chloride forms also.
Considering the reaction's stoichiometry and the notion of molarity, 1.167 grams of solid barium sulfate form when 32.0 mL of 0.160 M barium chloride reacts with 70.0 mL of 0.065 M sodium sulfate.
The balanced reaction is:
BaCl₂(aq) + Na₂SO₄(aq) → BaSO₄(s) + 2 NaCl(aq)
What is a Limiting Reagent?The reactant that is consumed first in a chemical reaction is the limiting reagent because it stops any more reactions from taking place. The limiting reagent controls how much product is produced during the reaction.
Utilizing the reaction stoichiometry and the estimated number of moles, it is possible to identify the limiting reagent.
According to reaction stoichiometry, which describes the proportions of reagents and products in a chemical reaction, the following numbers of moles of each component are involved in the reaction:
BaCl₂: 1 moleNa₂SO₄: 1 moleBaSO₄: 1 moleNaCl: 2 molesMolarity, on the other hand, refers to how many moles of solute are dissolved in a certain volume.
Molarity is determined by the expression:
[tex]Molarity=\frac{number of moles of solute}{volume}[/tex]
Molarity is expressed in units[tex]\frac{moles}{L}[/tex].
In this case, 32.0 mL= 0.032L (being 1000 mL= 1 L) of barium chloride reacts. So, by definition of molarity, the number of moles that participate in the reaction is calculated as:
[tex]0.160 M=\frac{No. of moles of solute}{0.032L}[/tex]
No of moles of barium chloride(solute) = 0.160M × 0.032L
No of moles of barium chloride(solute) = 0.00512moles
On the other side,70.0mL= 0.070 L of 0.065 M sodium sulfate reacts. So, by definition of molarity, the number of moles that participate in the reaction is calculated as:
[tex]0.065 M =\frac{No of moles of solute}{0.070L}[/tex]
No of moles of Sodium sulfate= 0.065M × 0.070L
No of moles of Sodium sulfate = 0.0045moles
if by stoichiometry 1 mole of barium chloride reacts with 1 mole of sodium sulfate, 0.00512moles of barium sulfate reacts with how many moles of sodium sulfate?
No. of moles of sodium sulfate=
[tex]\frac{ 0.00512moles of barium sulfate * 1 mole of sodium sulfate}{1 mole of barium chloride}[/tex]
amount of moles of sodium sulfate= 0.00512 moles
But 0.00512moles of sodium sulfate are not available, 0.0045moles moles are available. Since you have fewer moles than you need to react with 0.00512moles of barium chloride, sodium sulfate will be the limiting reagent.
Then, it is possible to determine the number of moles of barium sulfate produced by another rule of three: if by stoichiometry 1 mole of sodium sulfate produces 1 mole of barium sulfate, 0.00512 moles of sodium sulfate produces how many moles of barium sulfate?
[tex]Amt of mole of barium sulfate=\frac{0.00512 moles of sodium sulfate* 1mole of barium sulfate}{1 mole of sodium sulfate}[/tex]
amount of moles of barium sulfate= 0
Being the mass molar of barium sulfate is 233.34 g/mole, the mass-produced of the compound is calculated as:
= [tex]\frac{0.00512 moles * 233.34 gm}{1 mole}[/tex]
=1.167 gm
Hence, 1.167 gm of solid barium sulfate is formed.
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A doctor prescribed a tablet to a patient suffering from iron deficiency. The tablet does not look like iron. Explain.
Answer:
Tablets are made from salts of iron hence it does not look like iron.
Explanation:
Use the chemical equation to answer the question.
2H₂(g) + O₂(g) → 2H₂O(1)
Which statement describes the breaking and forming of bonds in the reaction?
The reaction requires breaking one H-H bond and two O=O bonds, and then forming four O-H bonds.
The reaction requires breaking one O=O bond and two H-H bonds, and then forming four O-H bonds.
The reaction requires breaking four O-H bonds, and then forming one H-H bond and two O=O bonds.
The reaction requires breaking four O-H bonds, and then forming one O=O bond and two H-H bonds
Answer: The reaction requires breaking one O=O bond and two H-H bonds, and then forming four O-H bonds.
Which of the following alkali metal is expected to melt if the room temperature
rise to 30oc (a) Na (b) K (c) Rb (d) Cs
What type of reaction is illustrated?
Answer:
Synthesis
Explanation:
Carbon + Difluorine = Tetrafluoromethane.
1 mole of Carbon [C] reacts with 2 moles of Difluorine [F2] to form 1 mole of Tetrafluoromethane [CF4]
Determine the mass of SO₂ that contains 6.075 × 10^26 S atoms.
Avogadro's law states that in a mole of any substance, there are [tex]6.022 \times 10^{23}[/tex] atoms. This means that in the given sample, there are
[tex]\frac{6.075 \times 10^{26}}{6.022 \times 10^{23}}=1008.8010627 \text{ mol}[/tex]
The atomic mass of sulfur is 32.06 amu.The atomic mass of oxygen is 15.9994 amu.So, the atomic mass of sulfur dioxide is
[tex]32.06+2(15.9994=64.0588 \text{ g/mol}[/tex]
Therefore, the mass is:
[tex](64.0588)(1008.8010627)=\boxed{64620 \text{ g (to 4 sf)}}[/tex]
What would most likely happen when a metal is heated?
It will melt.
It will solidify.
Its temperature will decrease.
Its particles will move slower.
Answer: it is A i took the test i got it right
Explanation: i took the test
Write and balance molecular equations for the following reactions between aqueous solutions. You will need to decide on the formulas and phases of the products in each of the cases.
An aqueous solution of barium hydroxide is mixed with an aqueous solution of sulfuric acid.
Answer:
Ba(OH)2(aq) + H2SO4(aq) ----> BaSO4(s) + 2H2O(l)
Which buffer can be suitable to prepare a solution that needs to be buffered at ph 4?
Answer:
For pH= 4.00 :
Add 0.1 ml of 0.1 molar NaOH to 50 ml of 0.1 molar potassium hydrogen phthalate .
B. Flourine is the right answer
Answer:
Whts ur question??
..?
Explanation:
Was this by mistake or smthin
How many grams of glucose (C6H12O6) are contained in 555 mL of a 1.77 M glucose solution?
Why is a low concentration of CO2 in our blood good while a high concentration is bad?
Carbon dioxide in your blood usually causes no problems. But if you have too much or too little of it, you may have a disease or a health emergency.
What is carbon dioxide?Carbon dioxide (CO2) is an odourless, colourless gas.
A high concentration can displace oxygen in the air. If less oxygen is available to breathe, symptoms such as rapid breathing, rapid heart rate, clumsiness, emotional upsets and fatigue can result.
As less oxygen becomes available, nausea and vomiting, collapse, convulsions, coma and death can occur.
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An unknown compound contains only C , H , and O . Combustion of 6.80 g of this compound produced 16.0 g CO2 and 4.37 g H2O . What is the empirical formula of the unknown compound?
Answer:
I am a small palm-sized pointing device
Which of the following statements about carbon dioxide is not true?
Increased carbon dioxide in the atmosphere increases the Greenhouse Effect.
Carbon dioxide is a greenhouse gas.
Atmospheric carbon dioxide levels have slowly declined over the last 50 years.
Burning fossil fuels can increase carbon dioxide levels in the atmosphere.
explain how magic numbers are related to nuclear stabilize
Answer:
A magic number is a number of nucleons (either protons or neutrons, individually) that form complete bands within the atomic nucleus. As a result, atomic nuclei with a magic number of protons or neutrons are significantly more persistent than other nuclei.
Determine how many kilojoules are absorbed when 341 g of Ca(OH)2 reacts via the following reaction:
Ca(OH)2(s)→CaO(s)+H2O(l),ΔH=+65.3kJ
305.6KJ are absorbed when 341 g of [tex]Ca(OH)_2[/tex]reacts via the following reaction.
What is enthalpy?The sum of the internal energy and the product of the pressure and volume of a thermodynamic system.
Given data:
[tex]Ca(OH)_2[/tex] (s) → [tex]CaO(s)+H_2O(l)[/tex], ΔH=+65.3kJ
Moles of [tex]Ca(OH)_2[/tex]= [tex]\frac{mass}{molar \;mass}[/tex]
Moles of [tex]Ca(OH)_2[/tex] = [tex]\frac{341 g }{74g/mol}[/tex] =4.68 moles
Since, 1 mol [tex]Ca(OH)_2[/tex] absorbs 65.3kJ.
Therefore, 4.68 moles [tex]Ca(OH)_2[/tex] produce energy = 65.3kJ X 4.68 moles
=305.6KJ
Hence, 305.6KJ are absorbed when 341 g of [tex]Ca(OH)_2[/tex] reacts via the following reaction.
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You need to measure out exactly 6.7 mL of water for an experiment. Which of the following would be the best tool for the job?
a. A 250 mL beaker
c. A 50 mL graduated cylinder
b. A 10 mL graduated cylinder
d. A 150 mL Erlenmeyer flask
Answer:
The answer for this problem would be "b. A 10 mL graduated cylinder".
Explanation:
The reason for this is because with a instrument that is closer to the value you're trying to measure, the more precise it will be.
For example using a teaspoon to measure something rather than a cup.
How many grams of copper
How would you draw the ionic compound Beryllium Arsenide lewis structure?
Answer:
[Na]^+ [Cl]^-
Explanation:
Lets say its sodium, its number of electrons is 11, but when its stable (an ion), it is 10. and chloride, number of electrons is 17, but when its stable (an ion) it is 18. So the lewis structure for that is, remember with the straight brackets (not sure what it's called, but you know what I mean I guess) its this one: [ ]
Sodium will be + because it has more protons (11-10 = +1), and chloride will be - because it gained an electron, so has more electrons than protons (17-18 = -1)
So the lewis structure would be:
[Na]^+ for sodium
and
[Cl]^- for chlorine
Sodium chloride:
[Na]^+ [Cl]^-
Also just to add, only 1 of each atom (Na and Cl) was needed for the bonding, but if let's say example; 2 Cl was needed to bond with sodium, there would be 2 Cl (same) and 1 Na.
Use Table B in your Student Guide to answer the questions about ion concentrations.
A solution with a pH = 13 has approximately how many moles of OH ions per liter?
How many moles of H* would this same solution have per liter?
(Use the decimal form of your answer.)
A different solution with an H+ concentration of 1.0 x 10-4 would have a pH =
Question 1
[tex]\text{pH}=-\log(\text{H}^{+})\\\\13=-\log(\text{H}^{+})\\ \\ \text{[H}^{+}]}=1 \times \boxed{10^{-13} \text{ moles per liter}} \\ \\ \text{[H}^{+}] \times \text{[OH}^{-}] =1 \times 10^{-14} \text{ M}\\\\\text{[OH}^{-}]=\boxed{1 \times 10^{-1} \text{ moles per liter}}[/tex]
Question 2
[tex]\text{pH}=-\log(\text{H}^{+})\\\\\text{pH}=-\log(1.0 \times 10^{-4})=\boxed{4}[/tex]
For the reaction below determine the ▲H for the reaction and state whether the reaction was endothermic or exothermic. Show your work.
C2H5OH + 3 O2 → 2 CO2 + 3H2O
C-C = 83 kcal; C-H = 99 kcal; C-O = 84 kcal; O-H = 111 kcal; C=O 192 kcal; O=O = 119 kcal
I got stuck on this and need help please, thank you so much!
Answer:exothermice
Explanation: it is relaeing heat not keeping it in