A reaction vessel contains an equilibrium mixture of SO2, O2, and SO3. The reaction proceeds such that: The partial pressures at equilibrium are:  PSO2​​=0.001714 atm   PO2​​=0.001919 atm   PSO3​​=0.0166 atm   Calculate KP for the reaction.

At -7.73 °C the pressure equilibrium constant K, =6.8 × 10° for a certain reaction. Here are some facts about the reaction: • The constant pressure molar heat capacity C, 1.76 J·mol -1. K¯!. • If the reaction is run at constant pressure, the volume increases by 14.%. The initial rate of the reaction is 11. mol·L - 1 -1 •S O Yes. Using these facts, can you calculate K, at 15. °C? O No. If you said yes, then enter your answer at right. Round it to 2 significant digits. Yes, and K, will be bigger. If you said no, can you at least decide whether K at Yes, and K, will be 15. °C will be bigger or smaller than K, at -7.73 °C? smaller.

Using any data you can find in the ALEKS Data resource, calculate the quilibrium constant K at 25.0°C for the following reaction.   Fe2O3(s)+  3H2(g)→  2Fe(s)+  3H2O(l) Round your answer to 2 significant digits.   delta G of Fe2O3=-742.2 kj/mol h2=0 Fe=0 H20=-237.1kj/mol

Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample of gas from the system is collected into 5.00 L flask. The flask is found to contain 8.62 g of CO, 2.60 g of H2, 43.0 g of CH4, and 48.4 g of H:O at 320.0 °C. What are the values of Kc and Kp for this reaction? CH:(g) + H2O(g) = CO(g) + 3 H2(g) 1 2 NEXT > Based on the given data, set up the expression for Kc and then evaluate it. Do not combine or simplify terms.

For the equilibrium reaction.   2IBr (g) I2 (g) + Br2 (g) Kc=.0085.  If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components.   Consider the decomposition reaction at 555 K   4POCl3 (g)    P4  (g) + 2O2  (g) + 6Cl2  (g)   If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm.  Find Kp and Kc.

A reaction vessel initially contains 6.30 atm of A and 2.10 atm of B. A reaction occurs according to the equation:2A(g)+B(g)⇆2C(g)2A(g)+B(g)⇆2C(g)When equilibrium is reached, the total pressure is found to be 6.51 atm. What is the equilibrium constant Kp?Please enter your response to three significant figures using decimal notation.

At a given temperature,  solid NH4HS is placed in a closed flask and dissociates according to the equation below. NH4HS(s) ⇄ NH3(g) + H2S(g). The total pressure of the equilibrium mixture is 2.4 atm. Determine Kp at this temperature. Express your answer using at least two significant figures. Do not use scientific notation.

Calculate the pressure equilibrium constant KP for the equilibrium between nitrogen monoxide, oxygen, and nitrogen dioxide has the final temperature of the mixture round your answer to two significant digits.