13. Balance and set up the equilibrium constant expression for the following chemical reactions: a. SO2(g)...
The equilibrium constant for the following reaction is 1.71×10-2 at 847 °C. 2 SO3(g)2 SO2(g) + O2(g) K = 1.71×10-2 at 847 °C Calculate the equilibrium constant for the following reactions at 847 °C. (a) 2 SO2(g) + O2(g)2 SO3(g) K = (b) SO3(g) SO2(g) + 1/2 O2(g) K = Show Approach
At a certain temperature, the equilibrium constant for the following chemical equation is 3.30. SO2(g) + NO2(g) <---> SO3(g) + NO(g), At this temp, calculate the number of moles of NO2(g) that must be added to 2.64 mol of SO2(g) in order to form 1.10 mol of SO3(g) at equilibrium.
For the chemical equation SO2(g) + NO2(g) – SO2(g) + NO(g) the equilibrium constant at a certain temperature is 2.00. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.31 mol SO2(g) in order to form 1.10 mol SO3(g) at equilibrium. moles of NO2(g): _______ mol
i need 2,3,4,5,and 6. 2. (6 Pts) Write the equilibrium expression, Kp, for the reactions in problem 1. 3. (8 Pts) At 127°C, Kc = 2.6 x 10-5 for the reaction: 2 NH3(g) + N2(g) + 3 H2(g) Calculate Kp at this temperature. 4. (10 Pts) A 1.00-L flask was filled with 2.00 mol gaseous SO2 and 2.00 mol gaseous NO, and heated. After equilibrium was reached, it was found that 1.30 mol gaseous NO was present. Assume that the...
to access important values if needed for this question. Write the expression for the equilibrium constant Kp for the following reaction (Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PnH;) as (P NH3)*. If either the numerator or denominator is 1, please enter 1.) 2 SO3() 4 2 SO2(g) + O2(e) K =
More Equilibrium: Please write equilibrium expressions for the following reactions: 1. i. 2 SO2 (g) + O2 (g) 2 SO3 (g) il. NH4NOs (s) N2O (g) +2 H20 (g) i CaCO3 (s) + CaO (s) + CO2 (g) iv. HNO2 (aq) +H2O (I) HaO* (aq) + NO2 (aq) 2. Predict which way the equilibrium will shift for each of the following changes: CO (g) + H2 (g) C (s) H2O (g) + heat i. increase [H2O] ii. increase [C0] iii....
For the chemical equation SO2(g)+NO2(g)↽−−⇀SO3(g)+NO(g) the equilibrium constant at a certain temperature is 2.70. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.20 mol SO2(g) in order to form 1.00 mol SO3(g) at equilibrium. moles of NO2(g):
1. Write the equilibrium-constant expression (Kc) for the following reactions (a) H2 (g) + 12(g) = 2H1 (9) (b) 2Cl2 (g) + 2H20 (9) + 4HCI (9)+ O2 (g) (c) H2(g) + Br2(1) HBr (g) (d) Ag(CN) 2 (aq) + Agl (s) + (aq) + 2AgCN (s)
At a given temperature, the equilibrium constant Kc for the reaction 2SO2(g)+O2(g)<==>2SO3(g) is 2.99x10^-3. What is the value of the equilibrium constant for each of the following reactions at that temperature? a. SO2(g)+ 1/2 O2(g)<==> SO3(g) b. 2SO3(g)<==>2SO2(g)+O2(g) c. SO3(g)<==> SO2(g)+ 1/2 O2(g)
Balance the following chemical equations using the smallest whole number coefficients. PbO2(s) → PbO(s) + O2(g) SO2( Balance the following chemical equations using the smallest whole number coefficients. PbO2(s) → PbO(s) + O2(g) SO2(g) + O2(g) → SO3(g) H2(g) + Br2(g) → HBr(g) g) + O2(g) → SO3(g) H2(g) + Br2(g) → HBr(g)