The balanced chemical equation for the reaction of copper (Cu) and silver nitrate (AgNO3) is shown below. Cu + 2AgNO3 mc001-1.jpg 2Ag + Cu(NO3)2 How many moles of copper must react to form 3.50 mol of Ag?
Answers
Cu + 2AgNO3 = 2Ag + Cu(NO3)2
We are givent the amount of silver to be produced. This will be the starting point. Calculations are as follows:
3.50 mol Ag ( 1 mol Cu / 2 mol Ag ) = 1.75 mol Cu
Therefore, we need 1.75 mol of copper in order to produce 3.50 mol of silver.
Answer:
1.75 moles of copper must react to form 3.50 mol of Ag.
Explanation:
According to reaction 2 moles of silver are obtained from 1 mole of copper.
Then 3.50 mole of Silver will be obtained from:
1.75 moles of copper must react to form 3.50 mol of Ag.
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The density of aluminum is 2.70 g/cm3. What is the mass of 235 cm3 of aluminum? 634.5 g635 g635 g/cm3634.5 ml
Answers
H2O + CO2 --> H2CO3
Ratio between water and CO2 is 1:1. So we can say that for every Mole of CO2, we need 1 Mole of water to produce 1 Mole of H2CO3. Thus as n=m/M we can find n = 528/44.01 = 11.997 ~ 12Mol.
Therefore, we need 12 moles of water.
Answer:
12 moles
Explanation:
The reaction will form carbonic acid:
CO₂ + H₂O ⇒ H₂CO₃
For 528 g of CO₂, the number of moles (n) will be:
n = mass/molar mass
n = 528/44.01
n = 12 moles of CO₂
The stoichiometry is 1 mol of CO₂ reacts with 1 mol of H₂O, so 12 moles of CO₂ need 12 moles of H₂O.
It is the type of cell used in electroplating
It uses an electric current to make a nonspontaneous reaction go.
All of the above
18. The products formed in the net reaction of the electrolysis of water are ____.
aqueous hydrogen ion and hydroxyl ion
hydrogen gas and oxygen gas
liquid hydrogen and oxygen gas
liquid oxygen and hydrogen gas
19. What occurs in electroplating?
decomposition of a metal layer
decomposition of a salt layer
deposition of a metal layer on a material
deposition of a salt layer on a metal
Answers
17. All of the above
18. hydrogen gas and oxygen gas
19. deposition of a metal layer on a material
Electrolytic cells use electric currents to drive a non-spontaneous reaction forward. This is also used in electroplating which involves the movement of metal cations to the surface of another metal. Water can also undergo electrochemical reactions by splitting it into its gaseous components, hydrogen and oxygen.
Final answer:
An electrolytic cell uses an electric current to make a nonspontaneous reaction go and is used in electroplating. The products formed in the electrolysis of water are hydrogen gas and oxygen gas. Electroplating involves the deposition of a metal layer on a material.
Explanation:
An electrolytic cell is a type of cell that uses an electric current to make a nonspontaneous reaction go. This means it can drive a chemical reaction in a direction that does not occur naturally. Electrolytic cells are commonly used in electroplating, where a metal layer is deposited onto a material. Therefore, all of the given options in question 17 are true about an electrolytic cell. For question 18, the products formed in the net reaction of the electrolysis of water are hydrogen gas and oxygen gas. Electrolysis of water involves the decomposition of water into its elemental components. In electroplating, the process involves the deposition of a metal layer on a material. This is achieved by passing an electric current through a solution containing metal ions, causing the metal ions to be reduced and deposit onto the material's surface.
Learn more about Electrolytic cell here:
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b. natural gas
c. petroleum
d. methanol
Answers
A.
It is not possible to press down on the chest of a CPR mannequin.
B.
It is not possible to breathe into the mouth a CPR mannequin.
C.
It is not possible to check for a real pulse on a CPR mannequin.
D.
It is not possible to lay a CPR mannequin on the floor.
Answers
Answer: The answer is C cause a CPR doll can do the rest
Explanation: pls mark as brainliest
Answers
Reaction 1: S(s) + O₂(g) → SO₂(g) ΔrH₁ = -296.8 kJ/mol.
Reaction 2: H₂(g) + ½ O₂(g) → H₂O(l) ΔrH₂ = -285.8 kJ/mol.
Reaction 3: H₂(g) + S(s) → H₂S(g) ∆rH₃ = -20.6 kJ/mol.
Reaction 4: 2H₂S(g) + 3O₂(g) → 2H₂O(l) + 2SO₂(g) ΔrH₄ = ?
Using Hess's law reaction number 4 is sum of reaction number 1 multiply with two, reaction number 2 multiply with two and reaction 3 reversed and multiply with two:
ΔrH₄ = 2 · (-296.8 kJ/mol) + 2 · (-285.8 kJ/mol) + 2 · 20.6 kJ/mol.
ΔrH₄ = -1124 kJ/mol.
b. production of a gas
c. formation of a precipitate
d. change in shape