A 1.0L flask is filled with 1.8 mol H2 and 1.2 mol I2. The equilibrium reaction that takes place (shown below) has a Kc = 4.86. Determine the equilibrium concentration of HI. H2 (g) + L (g) = 2 HI(g) O0.75 O 1.0 1.5 0.50

3. Nitrogen gas and oxygen gas can combine to produce nitrogen monoxide. At 1500 K the equilibrium constant, Ke, is 1.0 x 10 . Suppose a sample of air has [N2] = 0.80 M and [O2] = 0.20 M before any reaction occurs. Calculate the equilibrium concentrations of product and reactants at equilibrium at this temperature.

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N₂(g) + 3 H₂ (g) 2 NH₂ (g) K₂= 6. × 10¯6 He fills a reaction vessel at this temperature with 5.0 atm of nitrogen gas and 2.4 atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NH3 at right. Round your answer to 1 significant digit. yes no atm x₁ x10 × Ś

For the chemical equation: SO2(g) + NO2(g) SO3(g) + NO(g) The equilibrium constant at a certain temperature is 8.80. At this temperature, calculate the number of moles of NO2(g) that must be added to 6.20 mol SO2(g) in order to form 4.40 mol SO3(g) at equilibrium.

For the chemical equation 2SO2(g) + NO2(g) 2SO3(g) + NO(g) The equilibrium constant at a certain temperature is 5.50. At this temperature, calculate the number of moles of NO2(g) that must be added to 1.20 mol SO2(g) in order to form 0.80 mol SO3(g) at equilibrium.

A mixture of 0.100 mol of SO2 and 0.100 mol of O2 is placed in a reaction container and allowed to react until equilibrium is established. 2 SO2 (g) + O2 (g)  ->  2 SO3 At equilibrium, 0.0916 mol of SO3 is present. a. What is the composition of the equilibrium mixture in terms of moles of each substance present? (Hint: Stoichiometry!)   b. If the container size is 3.0 L, what is the value of the equilibrium constant?

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N2(g) + 2H2O(g) 2 NO(g) + 2 H2(g) K=2.x 10 -10 He fills a reaction vessel at this temperature with 6.0 atm of nitrogen gas and 11. atm of water vapor. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of H2, using only the tools available to you within ALEKS? ○ yes x10 O no If you said yes, then enter the equilibrium pressure of H₂ at right. Round your answer to 1 significant digit. atm 5

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 NO(g) + Cl₂(g) = 2 NOC1 (g) K₁₂=4.×100 He fills a reaction vessel at this temperature with 8.0 atm of nitrogen monoxide gas and 7.5 atm of chlorine gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NOC1, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NOC1 at right. Round your answer to 1 significant digit. O yes O no 0 atm X

Consider the following equilibrium: 2 HCl ↔ H2 + Cl2      K = 0.04 In order to have 0.02 moles of Cl2 at equilibrium, how many moles of HCl should be initially placed in an empty 1 L flask?

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: N₂(g) + 2 H₂O(g) 2 H₂(g) + 2NO(g) = -9 K₂=3.x 107 He fills a reaction vessel at this temperature with 15. atm of nitrogen gas and 7.8 atm of water vapor. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NO, using only the tools available to you within ALEKS? If you said yes, then enter the equilibrium pressure of NO at right. Round your answer to 1 significant digit. O yes O no 0 atm 0 10 X