Answer:
–187.9 J/K
Explanation:
The equation that relates the three quantities is:
where
is the Gibbs free energy
is the change in enthalpy of the reaction
T is the absolute temperature
is the change in entropy
In this reaction we have:
ΔS = –187.9 J/K
ΔH = –198.4 kJ = -198,400 J
T = 297.0 K
So the Gibbs free energy is
However, here we are asked to say what is the entropy of the reaction, which is therefore
ΔS = –187.9 J/K
This is thermodynamics. When you increase the temperature of an object, the particles gain on kinethic energy ergo the move faster. When you decrease it, they slow down.
I am going to say it is false.
Answer:
41.67 mol
Explanation:
1 Litre of water = 1000g
Mole = mass / molar mass
Mass of 1 L of water = 1000 g
Molar mass of water (H2O) :
(H = 1, O = 16)
H2O = (1 * 2) + 16 = (2 + 16) = 18g/mol
Amount of water consumed = (3/4) of 1 litre
= (3/4) * 1000g
= 750g
Therefore mass of water consumed = 750g
Mole = 750g / 18g/mol
Mole of water consumed = 41.6666
= 41.67 mol
<u>Answer:</u>
I think it's (C)
The products are suitable for making nuclear weapons.
hope this helps!
