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lorasvet [3.4K]
3 years ago
5

The heat of combustion of wood is approximately 16 kJ/g. What is the final temperature that 500.0 mL of water, initially at 25.0

°C, will reach in a bomb calorimeter if 1.20 g of wood is burned?
a. 9.2 °C
b. 34.2 °C
c. 186 °C
d. No right answer.
Chemistry
1 answer:
marissa [1.9K]3 years ago
8 0

Answer:

The final temperature is 34,2 ºC when 1,20 g of wood is burned inside the calorimeter.

Explanation:

The heat of combustion of wood which is approximately 16 kJ/g means that 1 g requires 16 kJ of heat so let's calculate about 1,20 g which is the value of wood you have.

1 g ________ 16 kJ

1,20 g ______ 1,20 g x 16 kJ = 19,2 kJ = 19200 J

Now let's apply the calorimetry formula

Q = m . C . ΔT

19200 J = 500 g . 4,186 J/ gºC ( Tfinal - 25ºC)

<em>Look that we don't have the mass of water, instead we have the volume so as you know water density is 1 g/ml, we conclude that in 500 ml, we have 500 g.</em>

On the other hand we convert the 19.2 kJ into J (* 1000) by the units in the value of the specific heat of the water, it is in Joule

19200 J = 500 g . 4,186 J/ gºC ( Tfinal - 25ºC)

19200 J = 2093 J/ºC ( Tfinal - 25ºC)

19200 J = 2093 J/ºC .Tfinal - 52,325 J

19200 J + 52325 J = 2, 093 J/ºC .Tfinal

71525 J = 2093 J/ºC .Tfinal

71525 J /2093 ºC / J = Tfinal = 34,17ºC

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A piece of wood has a mass of 36g and measures 3cm X 6cm X 4cm. What is the density of the wood? Would the piece of wood float o
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3 years ago
How much heat (kJ) is absorbed by 229.1 g of water in order for the temperature to increase from 25.00∘C to 32.50∘C?
hammer [34]

Answer:

(Q1) 9.42 kJ.

(Q2) 1.999 kJ

Explanation:

Heat: This is a form of Energy that brings about the sensation of warmth.

The S.I unit of Heat is Joules (J).

The heat of a body depend on the mass of the body, specific heat capacity, and temperature difference. as shown below

Q = cm(t₂-t₁) ........................ Equation 1

(Q1)

Q = cm(t₂-t₁)

Where Q = amount of heat absorbed, c = specific heat capacity of water, m = mass of water, t₁ = initial temperature, t₂ = final temperature.

Given: m = 229.1 g = 0.2991 kg, t₁ = 25.0 °C, 32.50 °C

Constant: c = 4200 J/kg.°C

Substituting into equation 1

Q = 0.2991×4200(32.5-25)

Q = 1256.22(7.5)

Q = 9421.65 J

Q = 9.42 kJ.

Hence the heat absorbed = 9.42 kJ

(Q2)

Q = cm(t₂-t₁)

Where Q = amount of heat required, c = specific heat capacity of water, m = mass of water, t₁ = initial temperature, t₂ = final temperature.

Given: m = 34 g = 0.034 kg, t₁ = 9 °C, t₂ = 23 °C

Constant: c = 4200 J/kg.°C

Q = 0.034×4200(23-9)

Q = 142.8(14)

Q = 1999.2 J

Q = 1.999 kJ.

Thus the Heat required = 1.999 kJ

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