Answer:
183.6kg
Explanation:
Given parameters:
Specific heat of the substance = 0.246J/g°C
Change in temperature = 15.5°C
Amount of energy released = 700J
Unknown:
Mass of the sample = ?
Solution:
To solve this problem we used the energy equation:
H = m c Δt
H is the energy released
m is the unknown mass
c is the specific heat
Δt is the change in temperature
Now insert the parameters and find m;
700 = m x 0.246 x 15.5
700 = 3.8m
m = 183.6kg
Answer:
here's your answer
Explanation:
Molar mass of CH3CH2OH = 46.06844 g/mol
This compound is also known as Ethanol.
Convert grams CH3CH2OH to moles or moles CH3CH2OH to grams
Molecular weight calculation:
12.0107 + 1.00794*3 + 12.0107 + 1.00794*2 + 15.9994 + 1.00794
Percent composition by element
Hydrogen H 1.00794 6 13.128%
Carbon C 12.0107 2 52.143%
Oxygen O 15.9994 1 34.730%
Answer: {1102.91}
Given: K= °C + 273.15
K = 1,376.06
Since you’re trying to find C (Celsius) you want to get C by itself in the problem. So you subtract 273.15 from that side. Anything you do to one side of the equal sign you have to do to the other side, so also subtract 273.15 from K (1,376.06).
1,376.06 - 273.15 = {1102.91°C}