The equilibrium constant K for the reaction H₂(g) + CO₂(g) H₂O(g) + CO(g) is 4.20 at 1650.00 °C. Initially 0.800 mol H₂ and 0.800 mol CO₂ are injected into a 2.20 L flask. Calculate the concentration of each species at equilibriur sure each of your answer entries has the correct number of significant digits. Part 1 of 4 [H₂] = M X S

Write the expression for the equilibrium constant K, for the following reaction. Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH; )2 as (P NH3)² . If either the numerator or denominator is 1, please enter 1 2 NO(g) + Cl2(g) 2 NOCI(g) K

Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 7.45 × 10-5: NO₂(g) + CO(g) ⇒ NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 20. L reaction vessel is filled with 1.5 mol of NO and 1.5 mol of CO₂. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. NO(g)+CO,(9) NO₂(9)+CO(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 3 NO₂(g) + 3 CO(g) P 3 NO(g)+ 3 CO₂(9) There will be very little NO2 and CO. There will be very little NO and CO₂. Neither of the above is true. K = 0 K = 0 x10 Ś ? ollo 18 Ar BA

Solve correctly please. (Gpt/ai wrong answer not allowed)

14). For the reaction below: 2NH3(g) = N2(g) + 3H2(g) We initially mixed 1 M of N2 gas and 2 M of H2 gas in a 1.0 L sealed flak and allowed the reaction to reach equilibrium. When equilibrium is established what are the terms representing each of the concentration of the gases? Or, another word, what are the terms at the Line E? + 3H2(g) 2 + 2x b. 2NH3(g) = N2(g) + 3H2(g) 1 + x 2NH3(g) = N2(g) 1 + x а. Line E: -2x 2 + x Line E: -2x + ЗН-(9) 2 - 3x d. c. Line E: 2x 2NH3(g) = N½(g) 1- x 2NH3(g) = N2(g) + 3H2(g) 2 - 2x 3H2(g) 2 - 3x 1-x Line E: 2x 2NH3(g) = N½(g) + 1 - 2x е. Line E: 2x

A chemical engineer is studying the following reaction: BF3(aq)+NH3(aq) → BF3NH3(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 1.3. The engineer charges ("fills") three reaction vessels with boron trifluoride and ammonia, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel compound concentration expected change in concentration A BF3 NH₂ 0.99 M O increase Odecrease O (no change) 0.72 M O increase O decrease O (no change) BF3NH3 0.92 M O increase O decrease O (no change) BF3 1.25 M O increase Odecrease O (no change) B NH₁ 0.91 M O↑ increase Odecrease O(no change) BF3NH3 1.48 M O increase Odecrease O (no change) BF 0.52 M O increase Odecrease O (no change) C NH, 0.25 M O↑ increase Odecrease O (no…

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Suppose a 500. mL flask is filled with 1.3 mol of NO and 0.90 mol of NO2. The following reaction becomes possible: NO3(g)+NO(g) — 2NO₂(g) The equilibrium constant K for this reaction is 0.720 at the temperature of the flask. Calculate the equilibrium molarity of NO₂. Round your answer to two decimal places. M X Ś

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 CH₂(g) ⇒ C₂H₂(g) + 3 H₂ (g) K₂=1.x10-5 He fills a reaction vessel at this temperature with 15. atm of methane gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of C₂H₂, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of C₂H₂ at right. Round your answer to 1 significant digit. O yes no atm X

Suppose a 500. mL flask is filled with 0.90 mol of NO, 1.6 mol of NO and 1.4 mol of CO,. The following reaction becomes possible: NO,(g) + CO (g) = NO (g)+ CO,(g) The equilibrium constant K for this reaction is 3.12 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. IM