1.9264*10^23 is the answer
B. False
It was created in 1869
A negative ΔH and ΔS suggests that the reaction is exothermic and the leads to a decrease in the entropy of the system. In this case, the spontaneity of the reaction depends on the temperature and reaction is spontaneous at low temperature and non-spontaneous at a high temperature.
x = = 0.50 M
Answer:
In order to produce some SbCl5, a 1.00 mole sample of SbCl3 is first placed in an empty 2.00 liter container maintained at a temperature different from 182oC. At this temperature, Kc, equals 0.117. How many moles of Cl2 must be added to this container to reduce the number of moles of SbCl3 to 0.700 mole at equilibrium
Moles Cl2 that must be added = 0.40 mol
Explanation:
K = ( = 0.117
Equilibrium concentrations:
= (1.00 - 0.70) mol / 2.00 L = 0.15 M <<---why is it 1.00-0.70???
= 0.700 mole / 2.00L = 0.350 M
= x
Kc = ÷ (0.15) = 0.117
Moles Cl2 at equilibrium = 0.050 mol L x 2.00 L = 0.10 mol
Moles Cl2 needed to make 0.300 mol SbCl3 into SbCl5 = 0.30 mol
Moles Cl2 that must be added = 0.40 mol