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4 years ago

Which of the following substances heats the fastest?

Chemistry

1 answer:

Aneli [31]4 years ago

7 0

Answer:

Zinc

Explanation:

The specific heat capacity can be described as the amount of heat required to raise the temperature of a substance by one degrees Celsius. It is represented by C or S. The greater the carrying capacity of a substance, the more will be the heat required for that substance.

As we can see in the information given in the question, the specific heat capacity of zinc is the lowest as compared to steel, water and aluminium. Hence, zinc is the correct option.

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Given the enthalpies of reaction

Tju [1.3M]

2SO₂+O₂⇒2SO₃ ΔH=-197 kJ

<h3>Further explanation</h3>

Based on the principle of Hess's Law, the change in enthalpy of a reaction will be the same even though it is through several stages or ways

Reaction

2SO₂+O₂⇒2SO₃

Given :

1. S(s)+O₂(g)→SO₂(g) ΔH = -297 kJ

Reverse

SO₂(g) ⇒S(s)+O₂(g ΔH = +297 kJ (sign change to +) x 2

2SO₂(g) ⇒2S(s)+2O₂(g ΔH = +594 kJ

2.2S(s)+3O2(g)→2SO3(g) ΔH=-791kJ

Add both reactions and remove/subtract the same compound for different sides

1. 2SO₂(g) ⇒2S(s)+2O₂(g) ΔH = +594 kJ

2.2S(s)+3O₂(g)→2SO₃(g) ΔH=-791kJ

--------------------------------------------------------+

2SO₂+O₂⇒2SO₃ ΔH=-197 kJ

5 0

3 years ago

Which sample contains the fewest atoms? a. 10 g of c b. 10 g of ne c. 10 g of f d. 10 g of n e. 10 g of o

Lerok [7]

The molar mass and the mass of the substance give the moles of the substance. The 10-gram sample of neon (Ne) has the fewest atoms. Thus, option b is correct.

<h3>What are moles?</h3>

Moles of the substance are the ratio of the molar mass and the mass of the substance. The moles of each atom with respect to the Avagadro's number (Nₐ) is given as,

Moles = mass ÷ molar mass

Moles of carbon (C) = 10 ÷ 12

= 0.83 Nₐ atoms

Moles of neon (Ne) = 10 ÷ 20

= 0.5 Nₐ atoms

Moles of fluorine (F) = 10 ÷ 19

= 0.52 Nₐ atoms

Moles of nitrogen (N) = 10 ÷ 14

= 0.7 Nₐ atoms

Moles of oxygen (O) = 10 ÷ 16

= 0.63 Nₐ atoms

Therefore, option b. 10 gm neon has the fewest atoms.

Learn more about moles here:

brainly.com/question/11884840

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7 0

2 years ago

Africa’s largest lake is Lake __________.

Tresset [83]

Lake Victoria

Explanation:

4 0

3 years ago

Read 2 more answers

What is the solution's freezing point: 15 g of CH4N2O (Molar mass = 60.055 g/mol) in 200. g of H2O? (Kf = 1.86 (°C·kg)/mol)

AURORKA [14]

Ok to answer this question we firsst need to fin the number of mol of Urea (CH4N2O). to do this we simply :

1 mol of urea =15/60.055 = 0.25mol

therefore 200g of water contain 0.25mol

the next step is to determine the malality of our solution in 200g of water, to do this we say:

200 g = 1Kg/1000g = 0.2kg

therefor 0.25mol/0.2Kg = 1.25mol/kg

and from the equation:

we know that i = 1

we are given Kf

b is the molality that we just calculated

therefore;

the solutions freezing point is -2.325°C

8 0

2 years ago

A sample of mercury(II) oxide is placed in a 5.00 L evacuated container and heated until it decomposes entirely to mercury metal

Burka [1]

Answer:

There was originally placed 153 grams of mercury(II) oxide in the container

Explanation:

<u>Step 1:</u> The balanced equation

2HgO → 2Hg + O2

<u>Step 2:</u> Data given

Volume of the container = 5.00L

Temperature in the container = 25°C = 298.15 Kelvin

The gas pressure inside = 1.73 atm

<u>Step 3: </u>Calculate number of moles of O2

We use the ideal gas law for this

p*V = n * R * T

with p = the pressure of the gas = 1.73 atm

with V = the volume of the gas = 5.00 L

with n = the number of moles of the gas = TO BE DETERMINED

with R = the gas constant = 0.0821 L*atm*K^−1*mol^−1

T = The temperature in the container = 25°C = 298.15 Kelvin

p*V = n * R *T

n = P*V / R*T

n = 1.73 atm * 5.00 L / (0.0821 L*atm*K^−1*mol^−1 * 298.15 K)

n = 0.353 moles O2

<u>Step 4</u>: Calculate moles of HgO

In the equation 2HgO → 2Hg + O2 we can see that for 1 mole O2 produced, we need to consume 2 moles of HgO

if there is produced 0.353 moles of O2, we need to consume 2*0.353 = 0.706 moles of HgO

<u>Step 5:</u> Calculate mass of HgO

Mass of HgO = number of moles of HgO * Molar mass of HgO

Mass of HgO = 0.706 moles * 216.591 g/mole = 152.9 grams ≈ 153 grams of HgO

There was originally placed 153 grams of mercury(II) oxide in the container

7 0

4 years ago