When you assume that the gas is behaving ideally, the gas molecules are very far from each other that they do not have any intermolecular forces. If it behaves this way, you can assume the ideal gas equation:
PV = nRT, where
P is the pressure
V is the volume
n is the number of moles
R is a gas constant
T is the absolute temperature
When the process goes under constant pressure (and assuming same number of moles),
P/nR = T/V = constant, therefore,
T₁/V₁=T₂/V₂
If V₂ = V₁(1+0.8) = 1.8V₁, then,
T₂/T₁ = 1.8V₁/V₁
Cancelling V₁,
T₂/300=1.8
T₂ =540 K
If you do not assume ideal gas, you use the compressibility factor, z. The gas equation would now become
PV =znRT
However, we cannot solve this because we don't know the value of z₁ and z₂. There will be more unknowns than given so we won't be able to solve the problem. But definitely, the compressibility factor method is more accurate because it does not assume ideality.
In classifying salts as neutral, acidic, or basic, it is important to take note of the strength of the acids and bases that they come from. A strong acid and strong base produce a neutral salt. A weak acid and strong base produce a basic salt. A strong acid and weak base produce an acidic salt. So the answers must be:
KCl = neutral (from HCl and KOH)
NH4Br = acidic (from NH4 and HBr)
K2CO3 = basic (from KOH and H2CO3)
NaCN = basic (from NaOH and HCN)
LiClO = basic (from LiOH and HClO)
They have the same number of "protons" but a different number of "neutrons" therefore their "atomic number" weight(or mass) is different
<u>Answer:</u>
of the reaction will be negative,
of the reaction will be positive and
of the reaction will be negative.
<u>Explanation:</u>
Thermodynamic properties are enthalpy change
, entropy change
and Gibbs free energy![(\Delta G)](https://tex.z-dn.net/?f=%28%5CDelta%20G%29)
Exothermic reactions are defined as the reactions in which energy is released in the form of heat. The enthalpy change
of the reaction comes out to be negative for this kind of reaction.
Entropy change is defined as the change in the measure of randomness in the reaction. It is represented as
. Randomness of gaseous particles is more than that of liquid which is further more than that of solids.
For the given exothermic reaction:
![2C_2H_6(g)+7O_2(g)\rightarrow 4CO_2(g)+6H_2O(g)](https://tex.z-dn.net/?f=2C_2H_6%28g%29%2B7O_2%28g%29%5Crightarrow%204CO_2%28g%29%2B6H_2O%28g%29)
As, number of gaseous particles on the product side is more than the number of gaseous particles on the reactant side. So, the entropy change is positive. Hence,
is positive.
The above reaction is spontaneous. Thus, the Gibbs free energy will be negative.
For the given reaction: