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Nady [450]
3 years ago
7

7. A 28.4 g sample of aluminum is heated to 39.4 °C, then is placed in a calorimeter

Chemistry
1 answer:
klio [65]3 years ago
4 0

Answer:

The specific heat of aluminum is 0.214 calorie /gram °C

Explanation:

Specific heat:The heat requires to increase 1°C temperature of that object per unit gram.

When the aluminum comes in contact of of water then

The heat lose by aluminum = The heat gain by the water.

Q₁=Q₂

Where,

Q = m ×s× ΔT

m= mass of an object

s= specific heat of the object

ΔT= change of temperature.

The mass of aluminum(m₁)= 28.4 gram,  

ΔT for aluminum=(initial temperature - final temperature)= (39.4-23)°C=16.4°C

s₁=?

The mass of water(m₂) = 50 gram

ΔT for water =( final temperature-initial temperature)=(23-21)°C= 2°C

S₂=1 calorie /gram °C

Q₁=Q₂

⇒m₁s₁ΔT=m₂s₂ΔT

⇒(28.4×s₁×16.4)= 50×1×2

\Rightarrow s_1 =\frac{50\times 2}{28.4\times 16.4}

\Rightarrow s_1= 0.214 calorie /gram °C

The specific heat of aluminum is 0.214 calorie /gram °C

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Answer:

The solidifying/cooling and crystallizing of magma causes igneous rocks to form.

6 0
2 years ago
When water vapor condenses high in the sky what is formed
Goryan [66]
A cloud is formed because the water vapor gathers in groups
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Differences between mixtures and elements
EastWind [94]

Mixtures are a group of elements that are mixed together but not chemically combined

Elements are the fundamental materials of which all matter is composed.

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5 0
3 years ago
A 0.708 g sample of a metal, M, reacts completely with sulfuric acid according to the reaction M ( s ) + H 2 SO 4 ( aq ) ⟶ MSO 4
ollegr [7]

Answer:

The metal has a molar mass of 65.37 g/mol

Explanation:

Step 1: Data given

Mass of the metal = 0.708 grams

Volume of hydrogen = 275 mL = 0.275 L

Atmospheric pressure = 1.0079 bar = 0.9947 atm

Temperature = 25°C

Vapor pressure of water at 25 °C = 0.03167 bar = 0.03126 atm

Step 2: The balanced equation

M(s) + H2SO4(aq) ⟶ MSO4 (aq) + H2(g)

Step 3: Calculate pH2

Atmospheric pressure = vapor pressure of water + pressure of H2

0.9947 atm = 0.03126 atm + pressure of H2

Pressure of H2 = 0.9947 - 0.03126

Pressure of H2 = 0.96344 atm

Step 4: Calculate moles of H2

p*V=n*R*T

⇒ with p = The pressure of H2 = 0.96344 atm

⇒ with V = the volume of H2 = 0.275 L

⇒ with n = the number of moles H2 = TO BE DETERMINED

⇒ with R = the gas constant = 0.08206 L*atm/K*mol

⇒ with T = the temperature = 25°C = 298 Kelvin

n = (p*V)/(R*T)

n = (0.96344 * 0.275)/(0.08206*298)

n = 0.01083 moles

Step 5: Calculate moles of M

For 1 mole of H2 produced, we need 1 mole M

For 0.0108 moles of H2 we need 0.01083 moles of M

Step 6: Calculate molar mass of M

Molar mass M = Mass M / moles M

Molar mass M = 0.708 grams / 0.01083 moles

Molar mass M = 65.37 g/mol

The metal has a molar mass of 65.37 g/mol

5 0
3 years ago
Copper has average atomic mass of 63.546 amu. It's two isotopes are Cu-63 (which is 69.17% abundant and has a mass of 62.9296 am
garri49 [273]

Answer: 69.152% → 63^Cu

30.848% → 65^Cu

Explanation:

As you know, the average atomic mass of an element is determined by taking the weighted average of the atomic masses of its naturally occurring isotopes.

Simply put, an element's naturally occurring isotopes will contribute to the average atomic mass of the element proportionally to their abundance.

Explanation:

6 0
2 years ago
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