Answer:
The answer to your question is n = 0.838 moles
Explanation:
Data
Volume = 2.15 l
Pressure = 8.91 atm
Temperature = 5.81°C
moles = ?
Gas constant = 0.082 atm l / mol°K
Process
1.- Convert temperature to °K
Temperature = 5.81 + 273 = 278.81°K
2.- Write the Ideal gas formula
PV = nRT
-Solve for moles (n)
n = PV / RT
3.- Substitution
n = (8.91 x 2.15) / (0.082 x 278.81)
4.- Simplification
n = 19.16 / 22.86
5.- Result
n = 0.838 moles
The correct answer is a oxidizer
<span>Molar mass is the mass of a given substance divided by the amount of that substance, measured in g/mol. So probably A.)</span>
Answer:
A
Explanation:
How many moles of HCI will just react with 0.424 g Ba(OH)2?
A) 4.94 x 10 mol
Answer: B. endergonic, not spontaneous
Explanation:
Endergonic reactions are defined as the reactions in which energy of the product is greater than the energy of the reactants. The total energy is absorbed in the form of heat and 
for the reaction comes out to be positive.
The Gibbs equation is:
= Gibb's free energy change
= enthalpy change
T = temperature
= entropy change
A reaction is non spontaneous when = Gibb's free energy change is positive
Thus the reaction has to be endergonic.
