All substances are matter but all matters are not substance. Matter is generally a loose term used in respect to a substance. Matter and substance are sometimes used for the same context, this is certainly not correct. Various examples have already proved that a matter will not always be a substance depending on its physical nature, but a substance is always a matter.
(cc/ to Taskmasters , I just switched it up a little bit.)
Answer:
Option (A) : Positive
Explanation:
A combustion reaction will always be associated with a change in entropy that is Positive due to the gaseous products released. Hence, there is a large positive entropy change.
Answers:
G. -; H. -; I. +
Step-by-step explanation:
ΔE = q + w
Anything going into the system is positive (+), and anything leaving the system is negative (-).
G. Cooling with expansion
q: Heat is leaving; q is -
w: The system is doing work on the surroundings. Energy is leaving the system. w is -.
ΔE is -.
H. Heating a little, expanding a lot
q: Heat is entering; q is +.
w: The system is doing work on the surroundings. Energy is leaving the system. w is -.
However, the expansion work is the major factor.
ΔE ≈ w. ΔE is -.
I. Endothermic, no expansion
q: Heat is entering; q is +.
w: No expansion. w = 0.
ΔE = q. ΔE is +.
Hydrogen bonding occurs when hydrogen is bonded to an oxygen or nitrogen or fluorine atom. In this case, the hydrogen atom in a hydrogen fluoride molecule will be able to bond to the fluoride atom of another hydrogen fluoride molecule, forming a hydrogen bond.
Since the question manages to include moles, pressure, volume, and temperature, then it is evident that in order to find the answer we will have to use the Ideal Gas Equation: PV = nRT (where P = pressure; V = volume; n = number of moles; R = the Universal Constant [0.082 L·atm/mol·K]; and temperature.
First, in order to work out the questions, there is a need to convert the volume to Litres and the temperature to Kelvin based on the equation:
250 mL = 0.250 L
58 °C = 331 K
Also, based on the equation P = nRT ÷ V
⇒ P = (2.48 mol)(0.082 L · atm/mol · K)(331 K) ÷ 0.250 L
⇒ P = (67.31 L · atm) ÷ 0.250 L
⇒ P = 269.25 atm
Thus the pressure exerted by the gas in the container is 269.25 atm.