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3 years ago

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Silver can be electroplated at the cathode of an electrolysis cell by the half-reaction. Ag+(aq)+e−→Ag(s) Part A Silver can be e

lectroplated at the cathode of an electrolysis cell according to the following half-reaction: Ag+(aq)+e−→Ag(s) What mass of silver plates onto the cathode when a current of 8.5 A flows through the cell for 68 min ?

1 answer:

dmitriy555 [2]3 years ago

3 0

Answer: Mass of silver deposited at the cathode is 37.1g

Explanation: According to Faraday Law of Electrolysis, the mass of substance deposited at the electrode (cathode or anode) is directly proportional to quantity of electricity passed through the electrolyte

Faraday has found that to liberate one gm eq. of substance from an electrolyte, 96500C of electricity is required.

$Ag^+$ +e− ==> Ag(s)

Given that

Current (I) = 8.5A

Time (t) = 65 *60 = 3900s

Quantity of electricity passed = 8.5*3900 =33150C

Molar mass of Ag= 108g

96500C will liberate 108g

33150C will liberate Xg

Xg= (108*33150)/96500

=37.1g

Therefore the mass of Ag deposited at the cathode is 37.1g.

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Match the following reactions with the reaction type. You may use each type more than once.

vaieri [72.5K]

Answer:

1) Decomposition

2)Double-replacement reaction

3)synthesis

4)Double-replacement reaction

5)single-replacement reaction

6)Double-replacement reaction

Explanation:

Step 1: Data given

Synthesis: This is a reaction where two or more reactants will combine to form a new, single product. This is occurs when two or more reactants combine to form a single product. This can be shown with the following equation.

A + B → C

A and B are the reactants to form a new product C

Decomposition: This is a reaction where 1 (more complex) compound will be broken down into 2 or more (more simple) products.

This can be shown by the following equation:

AB → A + B

A single replacement: This is a reaction where one element wil be replaced by another element in the same compound. This can be shown by the following equation:

A + BC → B + AC

Here is the elemnt B in the compound BC, replaced by the element A, to form a new compound AC

A double-replacement: This is a reaction where the positive and negative ions of two ionic compounds will be exchanged and 2 new compounds willbe formed. This can be shown by the following equation:

AB+CD→AD+BC

A combustion reaction requires oxygen gas (O2) to produce the products CO2 and H2O

Step 2:

1) 2HgO(s) → 2Hg(l) + O2(g)

⇒ Decomposition

2) KCl(aq) + AgNO3(aq) → AgCl(s) + KNO3(aq)

⇒ Double-replacement reaction

3) 2Na(s) + H2(g) → 2NaH(s)

⇒ synthesis

4) Mg(OH)2(aq) + 2HNO2(aq) → Mg(NO2)2(aq) + 2 H2O(l)

⇒ Double-replacement reaction

5) Ca(s) + 2AgNO3(aq) → Ca(NO3)2(aq) + Ag(s)

⇒ Single-replacement reaction

6) Al2O3(s) + H2SO4(aq) → Al2(SO4)3(aq) + H2O(l)

⇒ Double-replacement reaction

8 0

3 years ago

Look at the diagram. Which shows the correct arrangement of electrons in water?

mariarad [96]

Answer:

Option 4

Explanation:

In water molecule, oxygen has -2 charge on it while the hydrogen has +1 charge and one atom of oxygen combines with two hydrogen atoms. A hydrogen need only two electrons to complete its octet (one electron is its own the second electron is shared by oxygen) and a oxygen needs 8 electrons (It has six of its own and two are shared by two hydrogen atom).

Hence, option 4 is correct

6 0

3 years ago

Read 2 more answers

A helium-filled balloon at 310.0 K and 1 atm, contains 0.05 g He, and has a volume of 1.21 L. It is placed in a freezer (T = 235

trapecia [35]

Answer : The value of $\Delta E$ of the gas is 2.79 Joules.

Explanation :

First we have to calculate the moles of helium.

$\text{Moles of helium}=\frac{\text{Mass of helium}}{\text{Molar mass of helium}}$

Molar mass of helium = 4 g/mole

$\text{Moles of helium}=\frac{0.05g}{4g/mole}=0.0125mole$

Now we have to calculate the heat.

Formula used :

$q=nc_p\Delta T\\\\q=nc_p(T_2-T_1)$

where,

q = heat

n = number of moles of helium gas = 0.0125 mole

$c_p$ = specific heat of helium = 20.8 J/mol.K

$T_1$ = initial temperature = 310.0 K

$T_2$ = final temperature = 235.0 K

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

$q=nc_p(T_2-T_1)$

$q=(0.0125mole)\times (20.8J/mol.K)\times (235.0-310.0)K$

$q=-19.5J$

Now we have top calculate the work done.

Formula used :

$w=-p\Delta V\\\\w=-p(V_2-V_1)$

where,

w = work done

p = pressure of the gas = 1 atm

$V_1$ = initial volume = 1.21 L

$V_2$ = final volume = 0.99 L

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

$w=-p(V_2-V_1)$

$w=-(1atm)\times (0.99-1.21)L$

$w=0.22L.artm=0.22\times 101.3J=22.29J$

conversion used : (1 L.atm = 101.3 J)

Now we have to calculate the value of $\Delta E$ of the gas.

$\Delta E=q+w$

$\Delta E=(-19.5J)+22.29J$

$\Delta E=2.79J$

Therefore, the value of $\Delta E$ of the gas is 2.79 Joules.

3 0

3 years ago

What Can You Tell About The Shape Of The Compound Made Of Magnesium & Nitrogen ?

earnstyle [38]

3. I am not sure what is meant by shape, it could be to do with structure.

4. It is magnesium nitride, as adding nitrogen makes a nitride

3 0

3 years ago

How many moles are in 8.32 times 1024 molecules of CO2

Svetradugi [14.3K]

Answer:

13.8 mol CO₂

General Formulas and Concepts:

<u>Chemistry - Atomic Structure</u>

Using Dimensional Analysis
Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.

Explanation:

<u>Step 1: Define</u>

8.32 × 10²⁴ molecules CO₂

<u>Step 2: Identify Conversions</u>

Avogadro's Number

<u>Step 3: Convert</u>

<u /> $8.32 \cdot 10^{24} \ molecules \ CO_2(\frac{1 \ mol \ CO_2}{6.022 \cdot 10^{23} \ molecules \ CO_2} )$ = 13.816 mol CO₂

<u>Step 4: Check</u>

<em>We are given 3 sig figs. Follow sig fig rules and round.</em>

13.816 mol CO₂ ≈ 13.8 mol CO₂

3 0

3 years ago