Answer:
Explanation:
P = Pressure = 
V = Volume = 
R = Gas constant = 
T = Temperature = 
The reaction is
From ideal gas equation we have
Moles of 
produced is
Molar mass of = 64.066 g/mol
Production rate is
The rate at which sulfur dioxide is being produced .
The question is incomplete, the complete question is;
The heat of vaporization ΔHv of acetic acid HCH3CO2 is 41.0 /kJmol. Calculate the change in entropy ΔS when 954.g of acetic acid condenses at 118.1°C. Be sure your answer contains a unit symbol. Round your answer to 3 significant digits.
Answer:
-1.67 JK-1
Explanation:
Since Heat of vaporization of acetic acid = 41.0 kJ/mol
Therefore:
Heat of condensation of acetic acid = -41.0 kJ/mol
Mass of acetic acid = 954 g
Temperature of condensation = 118.1 °C or 391.1 K
Number of moles of acetic acid = 954 g/60g/mol = 15.9 moles
Heat evolved during condensation = 15.9 moles * -41.0 kJ/mol = -651.9 KJ
Entropy change (ΔS) = Heat evolved/ Temperature = -651.9 KJ/391.1 K
Entropy change (ΔS) = -1.67 JK-1
Answer:
The resulting pressure is 2.81 atm
Explanation:
According to Dalton's Law of Partial Pressure, each of the gases (A and B) will exert their pressure independently. If we use Boyle's Law to calculate the pressure of each of the gases separately we have:
Pressure of gas A:
p1V1 = p2V2
p1 = 2.4 atm
V1 = 722 mL
V2 = 722 + 169 = 891 mL
p2 =?
Clearing p2:
p2 = (p1V1)/V2 = (2.4*722)/891 = 1.94 atm
Pressure of gas B:
p1 = 4.6 atm
V1 = 169 mL
V2 = 169+722 = 891 mL
p2=?
Clearing p:
p2 = (4.6*169)/891 = 0.87 atm
Dalton's expression for total partial pressures is equal to:
ptotal = pA + pB = 1.94+0.87 = 2.81 atm
The chemical equilibrium will shift to the left.
Since NH4+ ions are a product of the original reaction, increasing their concentration will shift the equilibrium toward the reactants.
What are you making a hypothesis for
