The equilibrium constant, Kc, for the following reaction is 1.80 × 10-4 at 298 K. NHHS(s) NH3(g) + H2S(g) Calculate the equilibrium concentration of H2S when 0.456 moles of NHHS(s) are introduced into a 1.00 L vessel at 298 K. [H2S] =|| M The boiling point of water is 100.00 °C at 1 atmosphere. A student dissolves 14.27 grams of magnesium acetate, Mg(CH3COO)2 (142.4 g/mol), in 201.2 grams of water. Use the table of boiling and freezing point constants to answer the questions below. Solvent Water Formula H₂O Kb (°C/m) K (°C/m) 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCI 3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 The molality of the solution is I m. The boiling point of the solution is °C.
The equilibrium constant, Kc, for the following reaction is 1.80 × 10-4 at 298 K. NHHS(s) NH3(g) + H2S(g) Calculate the equilibrium concentration of H2S when 0.456 moles of NHHS(s) are introduced into a 1.00 L vessel at 298 K. [H2S] =|| M The boiling point of water is 100.00 °C at 1 atmosphere. A student dissolves 14.27 grams of magnesium acetate, Mg(CH3COO)2 (142.4 g/mol), in 201.2 grams of water. Use the table of boiling and freezing point constants to answer the questions below. Solvent Water Formula H₂O Kb (°C/m) K (°C/m) 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCI 3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 The molality of the solution is I m. The boiling point of the solution is °C.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter13: The Chemistry Of Solutes And Solutions
Section: Chapter Questions
Problem 77QRT
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![The equilibrium constant,
Kc, for the following reaction is
1.80 × 10-4 at 298 K.
NHHS(s) NH3(g) + H2S(g)
Calculate the equilibrium concentration of
H2S when 0.456 moles of
NHHS(s) are introduced into a 1.00 L vessel at 298 K.
[H2S] =||
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd2c1d2e3-89ea-47de-ad2a-ad4f6e93129c%2Ff637cbf1-6e0a-496a-b814-1e9b997e613f%2Flpkmdg7_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The equilibrium constant,
Kc, for the following reaction is
1.80 × 10-4 at 298 K.
NHHS(s) NH3(g) + H2S(g)
Calculate the equilibrium concentration of
H2S when 0.456 moles of
NHHS(s) are introduced into a 1.00 L vessel at 298 K.
[H2S] =||
M
Transcribed Image Text:The boiling point of water is 100.00 °C at 1 atmosphere.
A student dissolves 14.27 grams of magnesium acetate, Mg(CH3COO)2 (142.4 g/mol), in 201.2 grams of water. Use the table of
boiling and freezing point constants to answer the questions below.
Solvent
Water
Formula
H₂O
Kb (°C/m) K (°C/m)
0.512
1.86
Ethanol
CH3CH2OH
1.22
1.99
Chloroform
CHCI 3
3.67
Benzene
C6H6
2.53
5.12
Diethyl ether CH3CH2OCH2CH3
2.02
The molality of the solution is I
m.
The boiling point of the solution is
°C.
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