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rusak2 [61]
2 years ago
10

A 59.1g sample of aluminum is put into a calorimeter (see sketch at right) that contains 250.0g of water. The aluminum sample st

arts off at 91.3°C and the temperature of the water starts off at 16.0°C. When the temperature of the water stops changing it's 19.5°C. The pressure remains constant at 1atm.
Calculate the specific heat capacity of aluminum according to this experiment.

Be sure your answer is rounded to the correct number of significant digits.
Chemistry
1 answer:
Rainbow [258]2 years ago
3 0

Answer:

The specific heat capacity of aluminum according to this experiment is 0.863 J/g°C

Explanation:

Step 1: Data given

Mass of aluminium = 59.1 grams

Mass of water = 250.0 grams

Initial temperature of aluminium = 91.3 °C

Initial temperature of water = 16.0 °C

Final temperature = 19.5 °C

Pressure remains constant

Specific heat capacity of water = 4.186 J/g°C

Step 2: Calculate specific heat of aluminium

Heat lost = heat gained

Qlost = -Q heat

Q = m*c*ΔT

heat aluminium = - heat water

m(aluminium) * c(aluminium) * ΔT(aluminium) = -m(water) * c(water) * ΔT(water)

⇒m(aluminium) = mass of aluminium = 59.1 grams

⇒c(aluminium) = the specific heat of aluminium = TO BE DETERMINED

⇒ΔT = the change in temperature = T2 -T2 = 19.5 - 91.3 = -71.8 °C

⇒ m(water) = 250.0 grams

⇒c(water) = the specific heat of water = 4.186 J/g°C

⇒ΔT = the change in temperature = T2 -T2 = 19.5 - 16.0 = 3.5 °C

59.1 * c(aluminium) * -71.8 °C = 250.0 * 4.186 J/g°C * 3.5 °C

c(aluminium) = 0.863 J/g°C

The specific heat capacity of aluminum according to this experiment is 0.863 J/g°C

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What quantity is measured in mol/dm³?
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L
M =  \frac{n}{V}  \\ M = \frac{mol}{L}  \\ or \\ M =  \frac{mol}{ {dm}^{3} }
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3 0
3 years ago
How many atoms are there in 32.45 grams of Magnesium?
levacccp [35]

Answer:

8.13 ×10²³ atoms

Explanation:

Given data:

Mass of magnesium = 32.45 g

Number of atoms = ?

Solution:

Number of moles of Mg:

Number of moles = mass/molar mass

Number of moles = 32.45 g/ 24 g/mol

Number of moles = 1.35 mol

Number of atoms:

1 mole contain 6.022×10²³ atoms

1.35 mol × 6.022×10²³ atoms/ 1mol

8.13 ×10²³ atoms

5 0
3 years ago
What compound consists of 0.248 g magnesium, 0.655 g sulfur, and 1.31 g oxygen
Ivenika [448]

Magnesium Peroxydisulphate with formula of MgS₂O₈.

<h3><u>Explanation:</u></h3>

The question clearly stands on the concept of molarity and atomic weights.

The atomic weight of magnesium = 24.

The atomic weight of sulphur = 32.

The atomic weight of oxygen = 16.

The amount of magnesium present = 0.248 g

The amount of sulphur present = 0.665 g.

The amount of oxygen present = 1.31g.

So, moles of magnesium present = 0.01 moles.

Moles of sulphur present = 0.02 moles.

Moles of oxygen present = 0.08 moles.

So, mole ratio of the compound as magnesium : sulphur : oxygen = 1:2:8.

So the compound is Magnesium Peroxydisulphate with formula of MgS₂O₈.

3 0
3 years ago
A chemistry student needs of carbon tetrachloride for an experiment. By consulting the CRC Handbook of Chemistry and Physics, th
mixer [17]

Answer:

34.6 cm³

Explanation:

<em>A chemistry student needs 55.0 g of carbon tetrachloride for an experiment. By consulting the CRC Handbook of Chemistry and Physics, the student discovers that the density of carbon tetrachloride is 1.59 g/cm³. Calculate the volume of carbon tetrachloride the student should pour out. Be sure your answer has the correct number of significant digits.</em>

Step 1: Given data

  • Mass of carbon tetrachloride (m): 55.0 g
  • Density of carbon tetrachloride (ρ): 1.59 g/cm³

Step 2: Calculate the required volume of carbon tetrachloride

Density is an intrinsic property of matter. It can be calculated as the quotient between the mass of the sample and its volume.

ρ = m/V

V = m/ρ

V = 55.0 g/(1.59 g/cm³)

V = 34.6 cm³

The chemistry student should pour 34.6 cm³ of carbon tetrachloride.

8 0
3 years ago
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