Part A
N2(g)+3Br2(g)⇌2NBr3(g)
K=[NBr3]2[N2][Br2]3 |
K=[N2][Br2]3[NBr3]2 |
K=[NBr3][N2][Br2] |
K=[NBr3]2[N2][Br2]3 |
Part B
C(s)+O2(g)⇌CO2(g)
K=[CO2][O2] |
K=[O2][CO2] |
K=[CO2][O2] |
K=[CO2][O2][C] |
When heated, carbon reacts with water to produce carbon monoxide and hydrogen.
C(s)+H2O(g)+heat⇌CO(g)+H2(g)
Part C
What effect does each of the following changes have on the equilibrium?
Drag the appropriate stresses to their respective bins.
add H2O, Add heat, lower temperature, remove CO
Categories:
Equilibrium shifts to products, Equilibrium shifts to reactants, Equilibrium doesn't shift
Part A N2(g)+3Br2(g)⇌2NBr3(g) K=[NBr3]2[N2][Br2]3 K=[N2][Br2]3[NBr3]2 K=[NBr3][N2][Br2] K=[NBr3]2[N2][Br2]3 Part B C(s)+O2(g)⇌CO2(g) K=[CO2][O2] K=[O2][CO2] K=[CO2][O2] K=[CO2][O2][C] When heated,...
2NO2(g)--2NO(g)+O2(g) (endothermic) H2(g)--2H(g) H2O(g)--H2O(l) CO2(s)--CO2(g) cem 15 Part A Predict the conditions (high temperature, low temperature, all temperatures, or no temperatures) under which each of the following reactions will be spontaneous Drag the appropriate items to their respective bins. Reset Help 2NO3(e)--2NO(g) + Os(e) (endele) - 1.00 H.) - 24(e) CO.() - CO. High temperature Low temperature All temperatures No temperatures
PART A For the reaction N2(g)+O2(g)?2NO(g) classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the reaction. a) half oxygen b) double oxygen c) double nitrogen d) half nitrogen e) double nitrogen monoxide f) half nitrogen monoxide PART B For the reaction C(s)+H2O(g)?H2(g)+CO(g) classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of...
Consider the reaction C(s)+CO2(g)⇌2CO(g). When 1.66 mol of CO2 and an excess of solid carbon are heated in a 21.2 L container at 1100K, the equilibrium concentration of CO is 7.19×10−2 M . Part A What is the equilibrium concentration of CO2? Part B What is the value of the equilibrium constant Kc at 1100 K?
For the reaction N2(g)+O2(g)<---- --->2NO(g) classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the reaction. Double(nitogen monoxide) halve (nitrogen monoxide) double(nitrogen) halve(oxygen) double(oxygen) halve(nitrogen) Question 2) For the reaction C(s)+H2O(g)<--- --->H2(g)+CO(g) classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the reaction. remove some water, add some hydrogen, remove some solid...
Consider the reaction: NiO(s)+CO(g)⇌Ni(s)+CO2(g) Kc=4000.0 at 1500 K When calculating the answer, do not round to the appropriate number of significant figures until the last calculation step. Part A If a mixture of solid nickel(II) oxide and 0.11000 M carbon monoxide is allowed to come to equilibrium at 1500 K, what will be the equilibrium concentration of CO2?
5. Given the following chemical equilibria, N2(g) + O2(g) = 2 NO(g) N2(g) + 3 H2(g) = 2 NH3(g) H2(g) + 1/2 O2(g) =H2O(g) Determine the method used to calculate the equilibrium constant for the reaction below. 4 NH3(g) + 5 O2(g) = 4 NO(g) + 6 H2O(g) K
1. 2 KO2(S) + CO2(g) K2CO3(S) + 3/2 O2(g) K = 0.0198 at 315 K AH = -183.6 kJ a. Calculate the value of K at 315 K, for reaction 2: 2. 2 K2CO3(s) + 3 O2(g) 4 KO2(s) + 2 CO2(g) b. Write the K equilibrium expression for reaction 1. c. Calculate the value of Kp for reaction 1 at 315 K.
N2(g) + O2(g) equilibrium reaction arrow 2 NO(g); Kc = 5.6 ✕ 10−4 at 2098 K (a) What is the value of Kc for the reaction 2 NO(g) equilibrium reaction arrow N2(g) + O2(g) at the same temperature? (b) What is the value of Kc for the reaction 1/2 N2(g) + 1/2 O2(g) equilibrium reaction arrow NO(g) at the same temperature? (c) Does the equilibrium in (a) favor the reactant or the products? reactant products (d) Does the equilibrium in...
At 850°C, the equilibrium constant K for the reaction 2CO(g) = C(s) + CO2(g) has a value of 0.0935. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?
R Part A Classify each of the following reactions: A CH(g)+202(g)->CO2 (g) + 2H20®) B. MgCOs(s) MgO(s) +CO2(g) C. 2K(s)+S(s)K,S() D. 2Na(s)+H20(1) +2NaOH(aq) E. 2CH OH( 2C(s) +4H2(g) + 0, (B) Drag the appropriate items to their respective bins. View Available Hint(s) Reset Help Decomposition Combination Combustion D