In a calorimetry experiment, it was determined that a 92.0 gram piece of copper metal released 1860 J of heat to the surrounding
1 answer:
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Answer : Option C) Atomic Size
Explanation : The atomic radius of the elements is found to be decreasing if we go from left to right in the modern periodic table. Accordingly, increases as the number of shielding electrons present in the atomic nucleus of the periodic elements which lies in the same row remains constant while the number of protons in each atomic shell increases.
The effective nuclear charge of an atom is defined as the net positive charge which is felt by the valence electron of the atomic element.
When is observed to decrease, it is seen that the atomic radius grows in size. So, it explains the inverse relationship between both. This phenomenon occurs, because there is more screening of the electrons from the nucleus taking place, which is observed due to decrease the attraction between the electron and the nucleus.
<u>Answer:</u> The above reaction is non-spontaneous.
<u>Explanation:</u>
For the given chemical reaction:
Here, nickel is getting reduced because it is gaining electrons and iron is getting oxidized because it is loosing electrons.
We know that:
Substance getting oxidized always act as anode and the one getting reduced always act as cathode.
To calculate the of the reaction, we use the equation:
Relationship between standard Gibbs free energy and standard electrode potential follows:
As, the standard electrode potential of the cell is coming out to be negative for the above cell. Thus, the standard Gibbs free energy change of the reaction will become positive making the reaction non-spontaneous.
Hence, the above reaction is non-spontaneous.
The volume of a balloon f a gas at 842 mm Hg and -23 celsius if it’s volume is 915 milliliters at a pressure of 1170 mm Hg And a temperature of 24 celsius is 0.22 litres
Explanation:
Data given:
Initial volume of the balloon having gas V1= 915ml OR 0.195 L
initial pressure of the gas P1= 1170 mm Hg OR 1.53 atm
initial temperature of the gas T1 = 24 celsius or 273.15 + 24 = 297.15 K
Final pressure of the gas P2 = 842 mm Hg or 1.10 atm
final temperature of the gas T2 = -23 degrees or 273.15 - 23 = 250.15 K
Final volume at final temperature and pressure V2=?
The formula used is of Gas Law:
=
V2 =
putting the values in the equation:
V2 =
V2 = 0.22 litres is the volume
The volume is 0.22 litres at a pressure of 1170 mmHg and temperature of -23 degrees.