Answer : The heat energy needed would be, 6486.5125 J
Explanation :
To calculate the change in temperature, we use the equation:
where,
q = heat needed = ?
m = mass of aluminum = 223 g
c = specific heat capacity of aluminum = 
= change in temperature
= initial temperature = 
= final temperature = 
Putting values in above equation, we get:
Therefore, the heat energy needed would be, 6486.5125 J
Question: The question is incomplete. Below is the complete question and the answer;
While ethanol (CH3CH2OH is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene CH2CH2) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 50.0 L tank at 22. °C with 24. mol of ethylene gas and 24. mol of water vapor. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains 15.4 mol of ethylene gas and 15.4 mol of water vapor The engineer then adds another 12. mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits.
Answer:
Number of moles of ethanol = 11 mol
Explanation:
SEE THE ATTACHED FILE FOR THE CALCULATION
The volume increases to 1.009 L.
<em>V</em>= <em>V</em>_0 +βΔ<em>T</em>
The thermal expansion coefficient (β) of water changes with temperature, so we must calculate the volume change over small (10 °C) intervals.
20 °C to 30 °C: <em>V</em> = 1 L + 0.000 207 L·°C^(-1) × 10 °C = 1.002 07 L
30 °C to 40 °C: <em>V</em> = 1.002 07 L + 0.000 303 L·°C^(-1)] × 10 °C = 1.005 10 L
40 °C to 50 °C: <em>V</em> = 1.005 10 L + 0.000 385 L·°C^(-1)] × 10 °C = 1.008 95 L
The volume increases by about 9 mL when the temperature increases from 20 °C to 50 °C.
Answer:
Intermolecular forces are the interactions that exist between molecules. Hydrogen bond typically occurs when a hydrogen atom bonded to O, N, or F, is electrostatically attracted to a lone pair of electrons on an O, N, or F in another molecule. Polarizability is a measure of how the electron cloud around an atom responds to changes in its electronic environment. London forces, also known as dispersion forces are weak interactions caused by the momentary changes in electron density in a molecule. Dipole-dipole are the attractive forces between the permanent dipoles of two polar molecules. All compounds exhibit van der Waal forces.
Explanation:
Molecules interact each other by intramolecular forces. Among them are van der Waal forces, which are weak interactions, so all compounds interacts by this kind of forces. London forces (dispersion forces) are comprised in the group of van der Waal forces, so they are weak forces. Hydrogen bond is a stronger force, which is resposible for the structure of ice and properties of liquid water (water molecules interacts each other by hydrogen bond), so they are very important forces!
Polarizability is the trend of a molecule to became more polar (when exist a net charge differences in the molecule).
