the equilibrium pressure of Bf2(8) 15.54 At 218 °C, K̟ = 1.2 × 10-4 for the equilibrium NH4SH(s) = NH3(g) + H2S(g) Calculate the equilibrium concentrations of NH3 and H2S if a sample of solid NH SH is placed in a closed vessel at 218 °C and decomposes until equilibrium is reached. 15.55 Consider the reaction CaSO4(s) = Ca2+(aq) + SO,² (aq) At 25 °C, the equilibrium constant is K, = 2.4 × 10¯³ for this reaction. (a) If excess CASO.(s) is mixed with water at 25 °C to produce a saturated solution of CaSO4, what are the equilibrium concentrations of Ca²+ and SO7? (b) If the resulting solution has a volume of 1.4 L, what is the minimum mass of CASO.(s) needed to achieve equilibrium? 4. 15.56 At 80 °C, K̟ = 1.87 × 10-3 for the reaction %3D PH3BCI3(s) = PH3(g) + BC13(g) (a) Calculate the equilibrium concentrations of PH3 and BCI3 if a solid sample of PH3BC13 is placed in a closed ves- sel at 80 °C and decomposes until equilibrium is reached. (b) If the flask has a volume of 0.250 L, what is the mini- mum mass of PH3BC13(s) that must be added to the flask to achieve equilibrium? 15.57 For the reaction I2(g) + Br2(g) 2 IBr(g), K. = 280 at 150 °C. Suppose that 0.500 mol IBr in a 2.00-L flask is allowed to reach equilibrium at 150°C. What are the equilibrium concentrations of IBr, I2, and Br,? 15.58 At 25 °C, the reaction CaCrO4(s) Ca2 (aq)+ CrO2 (aq) has an equilibrium constant K = 7.1 × 10-4. What are the equilibrium concentrations of Ca?+ saturated solution of CaCrO4? %3D oo and CrO,2- in a 4 15.59 Methane, CH4, reacts with I, according to the reactio
the equilibrium pressure of Bf2(8) 15.54 At 218 °C, K̟ = 1.2 × 10-4 for the equilibrium NH4SH(s) = NH3(g) + H2S(g) Calculate the equilibrium concentrations of NH3 and H2S if a sample of solid NH SH is placed in a closed vessel at 218 °C and decomposes until equilibrium is reached. 15.55 Consider the reaction CaSO4(s) = Ca2+(aq) + SO,² (aq) At 25 °C, the equilibrium constant is K, = 2.4 × 10¯³ for this reaction. (a) If excess CASO.(s) is mixed with water at 25 °C to produce a saturated solution of CaSO4, what are the equilibrium concentrations of Ca²+ and SO7? (b) If the resulting solution has a volume of 1.4 L, what is the minimum mass of CASO.(s) needed to achieve equilibrium? 4. 15.56 At 80 °C, K̟ = 1.87 × 10-3 for the reaction %3D PH3BCI3(s) = PH3(g) + BC13(g) (a) Calculate the equilibrium concentrations of PH3 and BCI3 if a solid sample of PH3BC13 is placed in a closed ves- sel at 80 °C and decomposes until equilibrium is reached. (b) If the flask has a volume of 0.250 L, what is the mini- mum mass of PH3BC13(s) that must be added to the flask to achieve equilibrium? 15.57 For the reaction I2(g) + Br2(g) 2 IBr(g), K. = 280 at 150 °C. Suppose that 0.500 mol IBr in a 2.00-L flask is allowed to reach equilibrium at 150°C. What are the equilibrium concentrations of IBr, I2, and Br,? 15.58 At 25 °C, the reaction CaCrO4(s) Ca2 (aq)+ CrO2 (aq) has an equilibrium constant K = 7.1 × 10-4. What are the equilibrium concentrations of Ca?+ saturated solution of CaCrO4? %3D oo and CrO,2- in a 4 15.59 Methane, CH4, reacts with I, according to the reactio
Chemistry: The Molecular Science
5th Edition
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Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 51QRT: At room temperature, the equilibrium constant Kc for the reaction
2 NO(g) ⇌ N2(g) + O2(g)
is 1.4 ×...
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Question
Question 15.56 part A only
Transcribed Image Text:the equilibrium pressure of Bf2(8)
15.54 At 218 °C, K̟ = 1.2 × 10-4 for the equilibrium
NH4SH(s) = NH3(g) + H2S(g)
Calculate the equilibrium concentrations of NH3 and H2S
if a sample of solid NH SH is placed in a closed vessel at
218 °C and decomposes until equilibrium is reached.
15.55 Consider the reaction
CaSO4(s) = Ca2+(aq) + SO,² (aq)
At 25 °C, the equilibrium constant is K, = 2.4 × 10¯³ for
this reaction. (a) If excess CASO.(s) is mixed with water
at 25 °C to produce a saturated solution of CaSO4, what
are the equilibrium concentrations of Ca²+ and SO7?
(b) If the resulting solution has a volume of 1.4 L, what
is the minimum mass of CASO.(s) needed to achieve
equilibrium?
4.
15.56 At 80 °C, K̟ = 1.87 × 10-3 for the reaction
%3D
PH3BCI3(s) = PH3(g) + BC13(g)
(a) Calculate the equilibrium concentrations of PH3 and
BCI3 if a solid sample of PH3BC13 is placed in a closed ves-
sel at 80 °C and decomposes until equilibrium is reached.
(b) If the flask has a volume of 0.250 L, what is the mini-
mum mass of PH3BC13(s) that must be added to the flask
to achieve equilibrium?
15.57 For the reaction I2(g) + Br2(g)
2 IBr(g), K. = 280
at 150 °C. Suppose that 0.500 mol IBr in a 2.00-L flask
is allowed to reach equilibrium at 150°C. What are the
equilibrium concentrations of IBr, I2, and Br,?
15.58 At 25 °C, the reaction
CaCrO4(s) Ca2
(aq)+ CrO2 (aq)
has an equilibrium constant K = 7.1 × 10-4. What are
the equilibrium concentrations of Ca?+
saturated solution of CaCrO4?
%3D
oo
and CrO,2- in a
4
15.59 Methane, CH4, reacts with I, according to the reactio
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