Initial (M) Change (M) Equilibrium (M) -0.00875 0.0209 Consider the reaction of SO₂ and O₂ described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 SO₂(g) + O₂(g) = 2 SO3(g) NEXT > A 2.00 L reaction vessel was filled 0.0432 mol SO₂ and 0.0296 mol O₂ at 900 K and allowed to react. At equilibrium, the concentration of SO3 was found to be 0.0175 M. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. 0 0.00875 2.00 1 2SO₂(g) 0.0216 2.00 0.0432 0.0148 0.0296 2 0.0041 O₂(g) 0.0175 0.0129 -0.0175 0.0061 2SO₂(g) RESET 00350 0.0257

Find the equilibrium pressure of NOCl at right. Round your answer to 1 significant digit. thank you!!

Consider the synthesis of laughing gas, which you might have experienced at the dentist’s office:2 N2 + O2 ↔ 2 N2O Kc = 2.0 * 10-13a) Without doing any math, predict whether there will be more products or reactants at equilibrium. Explain your answer.b) If 0.0482 moles of nitrogen and 0.0933 moles of oxygen are introduced into a 1.0L flask, what will be the equilibrium concentrations of each of the three species?c) Without doing any real math – what is the sign of ∆Gº, and how do you know?

Suppose a 250. mL flask is filled with 1.0 mol of NO₂, 0.20 mol of NO and 1.7 mol of CO₂. The following reaction becomes possible: NO₂(g) +CO(g) NO(g) +CO, (g) The equilibrium constant K for this reaction is 5.54 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M Images X

Consider the following exothermic reaction system at equilibrium: N2(g) + 3H2(g) ⇒ 2NH3(g) Predict how the following changes affect the number of moles of each component of the system after equilibrium is reestablished by completing the table below: Note: Use I for increase, D for decrease, NC for no change Add N2(g) Remove H2(g) Add NH3(9) Add Ne(g) Increase the temperature (constant P) Decrease the volume (constant T) Add a catalyst Submit NH3 N₂ H2

For the chemical equation SO2(g) + NO2(g) SO3(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 2.86 mol SO2(g) in order to form 1.30 mol SO3(g) at equilibrium. moles of NO2(g): x10 TOOLS mol

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Chemistry

Suppose a 500. mL flask is filled with 0.80 mol of NO and 1.8 mol of NO2. The following reaction becomes possible: NO3(g) + NO(g) - 2NO2(g) The equilibrium constant K for this reaction is 4.37 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places.

Write the pressure equilibrium constant expression for this reaction. 2 H,(g)+O,(9)→2H,0(1)