Given the values of K shown below, determine the value of K for the reaction,
2 NOCl <=> O2(g) + N2(g) + Cl2(g)
1/2 N2 + 1/2 O2(g) <=> NO(g) K = 0.0848
NO(g) + 1/2 Cl2(g) <=> NOCl(g) K = 0.0388
Give your answer to the nearest whole number
Given the values of K shown below, determine the value of K for the reaction, 2...
0 out of 1 points Given the values of K shown below, determine the value of K for the reaction, 2 NO2(g) <=> N2O4(g). N2(g) + 2 O2(g) <=> 2 NO2(g) K = 8,569 N2(g) + 2 O2(g) <=> N2O4(g) K = 1,497 Give your answer to 3 decimal places Selected Answer: Incorrect [None Given] Correct Answer: Correct 0.175 ± 1%
Given the values of K shown below, determine the value of K for the reaction, Ca(s) + 1/2 O2(g) + CO2(g) <=> CaCO3(s) Ca(s) + 1/2 O2(g) <=> CaO(s) K = 2,501 CaCO3(s) <=> CaO(s) + CO2(g) K = 8,808 Give your answer to 3 or 4 decimal places
Determine the value of K for the balanced reaction, 2 NOCl(g) ↔ N2(g) + O2(g) + Cl2(g) at 291 K given the following information, 2 N2(g) + 2 O2(g) ↔ 4 NO(g); K = 5.397×10-61 NO + 1/2 Cl2(g) ↔ NOCl(g); K = 2.432×104
Determine the value of K for the balanced reaction, 2 NOCl(g) ↔ N2(g) + O2(g) + Cl2(g) at 279 K 2 N2(g) + 2 O2(g) ↔ 4 NO(g); K = 6.503×10-62 NO + 1/2 Cl2(g) ↔ NOCl(g); K = 4.122×104
18. Given the following system, determine the K values for each reaction below: 2 Cl2(g) + 2 H2O(g)- 4 HCl(g) + O2(g) Kc = 7.9x10-11 一73 12
Given the following equations and Ho values given below, determine the heat of reaction at 298 K for the reaction: 2 N2(g) + 5 O2(g) 2 N2O5(g) 2 H2(g) + O2(g) 2 H2O(l) Ho/kJ = -571.6 N2O5(g) + H2O(l) 2 HNO3(l) Ho/kJ = -73.7 N2(g) + 3 O2(g) + H2(g) 2 HNO3(l) Ho/kJ = -348.2
10 Use the following reactions and given ΔH values: 1/2 N2 (g) + 1/2 O2 (g) -> NO (g) ΔH = 90.3 kJ NO (g) + 1/2 Cl2 (g) -> NOCl (g) ΔH = -38.6 kJ Enter your answer with the appropriate significant figures and in terms of kJ. Do not include the unit in your answer.
1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M 2. Calculate the equilibrium concentration of Cl2 in that results from the decomposition of COCl2 with an initial concentration of 0.3166 M. COCl2(g) ⇌ CO(g)...
1. The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and use it to determine the direction in which each system will proceed to reach equilibrium. Write "R" if the reactions shifts to the right towards products or "L" if it shifts left towards reactants. A. {NO} = 1.00 M, {Cl2} = 1.00 M, {NOCl} = 0.00 M; K = 4.6 x 104 2NO(g)+Cl2(g)<->2NOCl(g) B. {SO3} = 2.00...
The reaction shown below has an equilibrium constant value of K, 8.84 at a certain temperature. 2 NO (g) N2 (g) + O2 (g) Kc = 8.84 0 moles of NO are sealed in a 2.00 L container. Calculate the concentration of Nz in the container when equilibrium is reached