The heat required to increase the temperature of 1.20 g of water is 80,256 k/j
<h3>What is specific heat?</h3>
The amount of energy needed to raise the temperature of one gram of a substance by one degree Celsius.
4. 18 J heat is required to change the temperature of 1.20 kg of water from 23. 00 °c to 39. 00 °c.
The heat required to raise temperature is the product of mass, specific heat and temperature change
1,200 × 4.18 × (39 − 23) = 80,256
Thus, the heat required to increase the temperature of 1.20 g of water is 80,256 k/j
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Answer:
The value of final volume inside the vessel 
= 5.17 ml
Explanation:
Initial pressure 
= 6263 mm Hg = 8.24 atm = 835 K pa
Initial temperature 
= 50.1 ° c = 323.1 K
Initial volume 
= 461.1 ml = 0.0004611 
Final temperature 
= - 95.8 ° c = 177.2 K
Finial pressure 
= 411 atm = 41644.6 K PA
We know that
Put all the values in the above equation
⇒ 835 × 
= 41644.6 × 
⇒ = 5.07 × 
⇒ = 5.17 ml
This is the value of final volume inside the vessel.
Answer:
The wood is oak.
Explanation:
Given data:
Mass of wood = 70 g
Volume of wood = 103 cm³
Wood is oak = ?
Solution:
We will calculate the density of wood then we will compare it with literature value.
Density = mass/ volume
d = 70 g/ 103 cm³
d = 0.68 g/cm³
The density of oak is 0.59 - 0.90 g/cm³.
So its true, wood is oak.
