1. A 50.0 L gas mixture at T = 500 K contains 123.0 g H2 and 855.0 g CO. What is the total pressure of the mixture? Assume ideal-gas behavior. Molar masses: M(H2) = 2.016 g/mol, M(CO) = 28.01 g/mol.
(A) 116 atm (B) 75.1 atm (C) 50.1 atm (D) 34.1 atm (E) 25.0 atm
2. KCl and K2SO4 are strong electrolytes. How do the concentrations of K+ ions, c(K+), in 2M KCl and 1M K2SO4 aqueous solutions compare?
(A) c(K+) is the same in both solutions.
(B) c(K+) in the KCl solution 2 times the concentration in the
K2SO4 solution.
(C) c(K+) in the KCl solution 1/2 times the concentration in the K2SO4 solution.
(D) c(K+) in the KCl solution 4 times the concentration in the K2SO4 solution.
(E) c(K+) in the KCl solution 1/4 times the concentration in the K2SO4 solution.
3. Nb2O5 and Al can react as follows: 3Nb2O5(s) + 10Al(s) = 6Nb(s) + 5Al2O3(s). Theoretically, how many grams of Nb can a mixture of 11.60 g Nb2O5 and 2.60 g Al produce? Molar masses: M(Nb2O5) = 265.8 g/mol, M(Al) = 26.98 g/mol, and M(Nb) = 92.91 g/mol.
(A) 14.9 g (B) 8.95 g (C) 8.10 g (D) 5.37 g (E) 2.03 g
A 50.0 L gas mixture at T = 500 K contains 123.0 g H2 and 855.0 g CO. What is the total pressure of the mixture? Assume ideal-gas behavior. Molar masses: M(H2) = 2.016 g/mol, M(CO) = 28.01 g/mol. (A) 116 atm (B) 75.1 atm (C) 50.1 atm (D) 34.1 atm (E) 25.0 atm
Nb2O5 and Al can react as follows: 3Nb2O5(s) + 10Al(s) = 6Nb(s) + 5Al2O3(s). Theoretically, how many grams of Nb can a mixture of 11.60 g Nb2O5 and 2.60 g Al produce? Molar masses: M(Nb2O5) = 265.8 g/mol, M(Al) = 26.98 g/mol, and M(Nb) = 92.91 g/mol. (A) 14.9 g (B) 8.95 g (C) 8.10 g (D) 5.37 g (E) 2.03 g
Exercise 16.56 Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.135 M CO and 0.135 M H2O. Part A What will be the equilibrium concentration of [CO]? [CO] = M SubmitMy AnswersGive Up Part B What will be the equilibrium concentration of [H2O]? [H2O] = M SubmitMy AnswersGive Up Part C What will be the equilibrium concentration of [CO2]? [CO2] = M SubmitMy AnswersGive Up Part D What will be the equilibrium concentration of [H2]?...
Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.150 M CO and 0.150 M H2O. What will be the equilibrium concentration of [CO2]? What will be the equilibrium concentration of [H2]?
The following reaction was carried out in a 3.75 L reaction vessel at 1100 K: C(s)+H2O(g)⇌CO(g)+H2(g) If during the course of the reaction, the vessel is found to contain 8.50 mol of C, 12.7 mol of H2O, 4.00 mol of CO, and 6.20 mol of H2, what is the reaction quotient Q? Enter the reaction quotient numerically. Q = Consider the reaction CO(g)+NH3(g)⇌HCONH2(g), Kc=0.810 If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M and 2.00...
1)Calculate the molar mass of a gas if 2.40 g occupies 0.885 L at 680 torr and 35 ∘C. 2) Consider three gases all at 298 K: HCl, H2, and O2. List the gases in order of increasing average speed. Express your answers as chemical formulas separated by commas. 3)A mixture containing 0.770 mol He(g), 0.300 mol Ne(g), and 0.115 mol Ar(g) is confined in a 10.00-L vessel at 25 ∘C. Calculate the partial pressure of He in the mixture...
5-7 (ACS-style) A mixture of 2.0 mol of CO (g) and 2.0 mol of H20 (g) was allowed to come to equilibrium in a 10.0-L flask at a high temperature. If Kc = 4.0, what is the molar concentration of H2 (g) in the equilibrium mixture? The equation for the reaction is: CO(g) + H20 (g) 5 CO2(g) + H2 (g) A) 0.67 M B) 0.40 M C) 0.20 M D) 0.13 M
Determine the volume of O_2 (at STP) formed when 50.0 g of KClO_3 decomposes according to the following reaction. The molar mass for KClO_3 is 122.55 g/mol. 2 KClO_3 (s) rightarrow 2 KCl(s) + 3 O_2(g) A) 12.3 L B) 9.14 L C) 14.6 L D) 8.22 L E) 13.7 L A gas mixture consists of N_2, O_2, and Ne, where the mole fraction of N_2 is 0.55 and the fraction of Ne is 0.25. If the mixture is at...
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