Suppose a 500.mL flask is filled with 1.7mol of H2 and 0.80mol of HI . The...

Suppose a 500.mL flask is filled with 1.7mol of H2 and 0.80mol of HI . The following reaction becomes possible: +H2gI2g 2HIg The equilibrium constant K for this reaction is 0.638 at the temperature of the flask. Calculate the equilibrium molarity of H2 . Round your answer to one decimal place.

Expert Solution

queen_honey_blossom answered 2 years ago

Suppose a 500. mL flask is filled with 0.20 mol of NO3 and 2.0 of NO...

Suppose a 500. mL flask is filled with 0.20 mol of NO3 and 2.0 of NO the following reaction becomes possible NO3(g) + NO (g) =2NO2(g) the equilibrium constant K for this reaction is 4.05 at the themperature of the flask .calculate the equilibrium Molarity of NO round to two decimal places final answer in Molarity .

Suppose a 500.mL flask is filled with 1.5mol of CO , 0.60mol of H2O and 1.8mol...

Suppose a 500.mL flask is filled with 1.5mol of CO , 0.60mol of H2O and 1.8mol of CO2 . The following reaction becomes possible: +COgH2Og +CO2gH2g The equilibrium constant K for this reaction is 3.35 at the temperature of the flask. Calculate the equilibrium molarity of H2 . Round your answer to one decimal place.

Suppose a 250.mL flask is filled with 2.0mol of O2 and 1.6mol of NO . The...

Suppose a 250.mL flask is filled with 2.0mol of O2 and 1.6mol of NO . The following reaction becomes possible: N2g+O2g =2NOg The equilibrium constant K for this reaction is 0.469 at the temperature of the flask. Calculate the equilibrium molarity of N2 . Round your answer to one decimal place.

Suppose a 250.mL flask is filled with 0.20mol of N2 and 1.4mol of O2 . The...

Suppose a 250.mL flask is filled with 0.20mol of N2 and 1.4mol of O2 . The following reaction becomes possible: N2(g)+O2(g)= 2NO(g )The equilibrium constant K for this reaction is 4.94 at the temperature of the flask. Calculate the equilibrium molarity of O2 . Round your answer to two decimal places.

A 500-mL flask of Ne at 500 torr is connect ed to a 300 mL flask...

A 500-mL flask of Ne at 500 torr is connect ed to a 300 mL flask of Xe at 700 torr. If the gases are allowed to mix and fill both flasks, what will be the partial pressure of each gas and what will be the total pressure of the mixture?

Suppose a 250.mL flask is filled with 0.90mol of Br2 , 0.60mol of BrOCl and 1.9mol...

Suppose a 250.mL flask is filled with 0.90mol of Br2 , 0.60mol of BrOCl and 1.9mol of BrCl . The following reaction becomes possible: Br2(g)+OCl2(g) +BrOCl(g)+BrCl(g) The equilibrium constant K for this reaction is 0.571 at the temperature of the flask. Calculate the equilibrium molarity of OCl2 . Round your answer to two decimal places.

Suppose a 480. mL flask is filled with 0.720 mol of N2 and 1.32 mol of...

Suppose a 480. mL flask is filled with 0.720 mol of N2 and 1.32 mol of NO. This reaction becomes possible: N2 (g) + O2 (g) ⇌ 2 NO(g) The equilibrium constant Kc is 7.62 at the reaction temperature. • Calculate the equilibrium molarity of O2 . • (Round final answer to two decimal places.)

A 1.500 L flask is filled with a mixture of 1.20 g H2 and 8.40 g...

A 1.500 L flask is filled with a mixture of 1.20 g H2 and 8.40 g O2, at 25°C. The mixture is ignited, and hydrogen and oxygen combine to form water. What is the total pressure inside the flask before the reaction? (Report your answer in units of atmospheres.) What is the total pressure after the reaction, once the flask is returned to 25°C? (Vapour pressure of water at 25°C is 23.8 mm Hg.)

A flask is filled with 4.0 atm of gaseous H2 and 3.0 atm of gaseous N2....

A flask is filled with 4.0 atm of gaseous H2 and 3.0 atm of gaseous N2. When a lit match is thrown into the flask, the gases react and form gaseous NH3. What is the pressure in the flask after the reaction? Answer: 4.33 atm. Please provide step by step on how to solve.

Suppose a 500. mL flash is filled with 1.1 mol of CO, 1.6 mol of NO...

Suppose a 500. mL flash is filled with 1.1 mol of CO, 1.6 mol of NO and 0.90 mol of CO2. The following reaction becomes possible: NO2(g)+CO(g)=NO(g)+CO2(g). the equilibrium constant K for this reaction is 0.209 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round to the nearest two decimals.

Question