Answer : The correct option is, (C) spontaneous only at low temperatures.
Explanation :
According to Gibb's equation:
= Gibbs free energy
= enthalpy change
= entropy change
T = temperature in Kelvin
As we know that:
= +ve, reaction is non spontaneous
= -ve, reaction is spontaneous
= 0, reaction is in equilibrium
The given chemical reaction is:
As we are given that, the given reaction is exothermic that means the enthalpy change is negative.
In this reaction, the randomness of reactant molecules are more and as we move towards the formation of product the randomness become less that means the degree of disorderedness decreases. So, the entropy will also decreases that means the change in entropy is negative.
Now we have to determine the spontaneity of this reaction when ΔH is negative and ΔS is negative.
As,
(at high temperature) (non-spontaneous)
(at low temperature) (spontaneous)
Thus, the reaction is spontaneous only at low temperatures.
It means the system absorbs energy from surrounding objects; usually, but not always, involving heat
Answer:
72.2 moles of water is spilled
Explanation:
as moles=mass/mr
so mr of water is 16+2=18
13000/18=72.2
for the second one you can work out the moles of o2
by using moles= number of particles /6.02*10^23
so 4.65*10^26/6.02*10^23
so i got 772.4 on my calculator to work out the amount of mass
u use the equation mass=moles*mr
so 777.2*16=12435g of oxygen gas
hope it helps :)
Non of them seem right... but I think C could be correct cause it definitely cant be A.
Molar mass H₂O = 18.0 g/mol
number of moles :
1.0 / 18.0 => 0.055 moles
1 mole -------------- 6.02 x 10²³ molecules
0.055 moles -------- ? molecules
molecules = 0.055 x ( 6.02 x 10²³) / 1
molecules = 3.311x10²² / 1
= 3.311 x 10²² molecules
hope this helps!
