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.
12. Consider the system PCl3(g) + Cl2(g) PCl5(g) at equilibrium at 25°C, for which H° = –92.5kJ at 25°C. When some Cl2(g) is added at constant volume and temperature, the ratio of the partial pressure of PCl5 to the partial pressure of PCl3 wil
For a system PCl3(g) + Cl2(g) PCl5(g) at equilibrium at 25°C, for which H° = –92.5kJ at 25°C, the ratio of the partial pressure of PCl5 to the partial pressure of PCl3 is will increase
What is the ratio of the partial pressure of PCl5 to the partial pressure of PCl3?Generally, the equation for chemiecal reaction is mathematically given as
PC3 (g) + C₁₁₂ (g) = PC15 (g) 3
Assuming the addition of some Cl2 gas. The reaction will shift to the right at the invariant volume temperature, maintaining equilibrium. This results in a rise in P9Cl5(g) and a fall in PpCl3(g).
PpCl (g) /PpCl (g) will increase
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The ratio of the partial pressure of PCl₅ to the partial pressure of PCl₃ is will increase for a system PCl₃ (g) + Cl₂ (g) --> PCl₅ (g) at equilibrium at 25°C, for which H° = –92.5kJ at 25°C when some Cl₂ (g) is added at constant volume and temperature.
What is the ratio of the partial pressure of PCl₅ to the partial pressure of PCl₃?
Generally, the equation for chemical reaction is mathematically given as ;
PCl₃ (g) + Cl₂ (g) --> PCl₅ (g)
Assuming the addition of some Cl₂ gas,
The reaction will shift to the right at the constant volume and temperature, maintaining equilibrium.
This results in a rise in PCl₅ (g) and a fall in PCl₃(g).
Hence, the ratio of the partial pressure of PCl₅ to the partial pressure of PCl₃ is will increases
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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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A
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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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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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
A dunk tank hold 30,533 moles of water? How many grams of water are in the tank?
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)
How many grams of copper
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.
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>Solidbalance the chemical
reaction by providing the
correct coefficient
Answer:
2HBr + Ba(OH)2 ____ BaBr2 + 2H2O
The numbers placed in front of formulas to balance equations
If you have the following chemical equation and you begin balancing it as such,
C5H10 + O2 --> 5CO2 + 5H2O
How many oxygens do you have on the product side at this point in the balancing?
Answer:
15 oxygens
Explanation:
Given the partially balanced reaction: [tex]\text{C}_{\text{5}}\text{H}_{\text{10}}+\text{O}_{\text{2}} \rightarrow \text{5C} \text{O}_{2}}+\text{5H}_\text{2}\text{O}[/tex]
The subscripts (small number to the right of each element symbol) are the number of atoms of the element within each compound/molecule, and the coefficients (numbers in front of each compound) represent the number of that molecule involved in one full reaction (if the equation were balanced).
The product side of the reaction is on the right of the arrow.
To determine the total number of Oxygens on the product side, we need to identify how many Oxygens are in each molecule (the subscript on the Oxygen), and then multiply times the number of that molecule that would be involved (Coefficient of the compound containing Oxygen). There are multiple compounds on the right side of the equation that contain Oxygen, so we'll need to add together the number of Oxygens each part contributes.
[tex]\text{C}_{\text{5}}\text{H}_{\text{10}}+\text{O}_{\text{2}} \rightarrow \bold{5}\text{C} \bold{O_{2}}+\bold{5}\text{H}_\text{2}\bold{O}[/tex]
[tex]\text{\# reactant-side Oxygens}=\bold{5}\text{C} \bold{O_{2}}+\bold{5}\text{H}_\text{2}\bold{O}\\=5 \text{ CO}_{\text{2}}\text{ molecules} *\frac{\text{2 Oxygens}}{\text{1 CO}_{\text{2}}\text{ molecule}}+5 \text{ H}_{\text{2}}\text{O molecules} *\frac{1\text{ Oxygen}}{\text{1 H}_{\text{2}}\text{O molecule}}\\=10\text{ Oxygens}+5\text{ Oxygens}\\=15\text{ Oxygens}[/tex]
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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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]
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.
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]
Explain how you would determine the charge of a metal, a non
metal and a transition metal for an ion within a compound. Be
prepared to provide the charge of an element on the periodic
table from each of these categories.
Answer:
In order to determine the charge of these elements you'll have to look at their placement in the periodic table by group number.
Explanation:
To further explain this, there is 18 groups of the periodic table. These groups include:
Group 1: The alkali metals have a 1+ charge for their entire group.
For example: Sodium would have a charge of 1+.
Group 2: The earth alkali metals all have a charge of 2+. For example Mg has a charge of 2+.
Group 3-12: The transitions metals are a little harder to figure the charge of each, if given the compound they are bonded with you can use that to figure it out but only a few have distinct charges. Such as Ag (Silver) only have a 1+ charge. If you are still trying to figure the charge, try making an electron configuration to figure out it's spare electron count or charge.
Group 13: These elements in group 13 have a typical charge of 3+. For example Al has a charge of 3+.
Group 14: These elements in group 14 have a typical charge of 4+. For example Carbon has a charge 4+
Group 15: These elements start the shift towards a negative charge in the table, so for group 15 the elements have a 3- charge. For example Nitrogen has a 3- charge.
Group 16: These elements continue with a negative in group 16 with a negative charge of 2-. For example Oxygen's charge is 2-.
Group 17: The halogen elements in group 17 have a charge of 1-. For example Chlorine has a charge of -.
Group 18: The noble gases in group 18 do not have a charge because they are some of the most stable elements so they're not looking to gain or lose an electron (That is what a charge is basicaly). So, they're charge is none.
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]
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.
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
B. Flourine is the right answer
Answer:
Whts ur question??
..?
Explanation:
Was this by mistake or smthin
What type of reaction is represented by the following equation?
Mg(OH)2 (aq) + 2 HCl (aq) --> MgCl2 (aq) + 2 H2O (l)
Answer: Double replacement reaction
Explanation:
6. A sample of a gas at 77°C and 1.33 atm occupies a volume of 50.3 L. How many moles of the gas are present? (Hint: Since moles have been asked, which equation has the moles listed in the equation. Use that to solve this problem).
The number of moles of the gas at 77°C and 1.33 atm occupies a volume of 50.3 L is 2.35 moles. It can found with the help of Ideal gas equation.
What is Ideal Gas equation ?The ideal gas equation is formulated as : PV = nRT.
In this equation, P refers to the pressure of the ideal gas, V is the volume of the ideal gas, n is the total amount of ideal gas that is measured in terms of moles, R is the universal gas constant, and T is the temperature.
Given ;
Pressure = 1.33 atmVolume = 50.3 ltrTemperature = 77 (+273 k) = 350KWe know ;
Gas constant (R) = 0.081 L atm/mol KFormula used ;
n = PV / RT
n = 1.33 x 50.3 / 0.081 x 350k
= 2.35 moles.
Hence, The number of moles of the gas at 77°C and 1.33 atm occupies a volume of 50.3 L is 2.35 moles
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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:
How many grams of glucose (C6H12O6) are contained in 555 mL of a 1.77 M glucose solution?
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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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
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.
You are working with a concentrated solution of ammonium hydroxide. Which
piece of safety equipment is most important to have on hand?
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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