The following reaction increases the proportion of hydrogen gas in order to use it as fuel. CO(g) + H2O(g) ↔ H2(g) + CO2(g) This reaction has been studied at various temperatures in order to find the optimum conditions. At 700 K, the equilibrium constant is 8.3. Suppose you start with 1.0 mol of CO(g) and 1.0 mol of H2O(g) in a 2.5 L container. How much of each substance will be in the container when the gases are at equilibrium, at 700 K?

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.

At a certain temperature, the equilibrium constant K for the following reaction is 0.0087: NO₂(g) + CO(g) → NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 29. L reaction vessel is filled with 0.27 mol of NO₂ and 0.27 mol of CO. 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 2 significant digits. NO(g) + CO₂(g) NO₂(g) +CO(g) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 2 NO₂(g)+2CO(g) 2NO(g)+2CO₂(g) There will be very little NO₂ and Co. There will be very little NO and CO₂. Neither of the above is true. K = 0 0 0 x10 X ?

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.

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2NO(g) +  Cl2(g)⇌ 2NOCl(g) Kp=2.x10^−1   He fills a reaction vessel at this temperature with 10.atm of nitrogen monoxide gas and 12.atm of chlorine gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NOCl, yes or no? If yes, then what is the equilibrium pressure of NOCl? Round your answer to 1 significant digit.

N2(g) and O2(g) can exist in equilibrium with NO(g), as shown below. The equilibrium constant at 25.0°C is 4.8 x 10-31. If initially there are 1.35 mol of nitrogen and 0.60 mol of oxygen in a 2.00 L vessel, find the equilibrium concentrations of each species. N2(g) + O2(g) → 2NO(g)

An equilibrium mixture contains 0.500 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g) + H,O(g) = CO,(g) + H,(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished? 6.25 moles of CO,: mol Incorrect Question Source: McOuarrie Pock And Gallogty

Calculate the equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture.

At a certain temperature, the equilibrium constant k for the following reaction is 6.3 x 10*: NO,(g) + CO(g) = NO(g) + CO,(g) Use this information to complete the following table. Suppose a 40. L reaction vessel is filled with 1.1 mol of NO2 and 1.1 mol of Co. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little NO2 and CO. There will be very little NO and CO2. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = NO(9)+CO2(9) NO2(9)+CO(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = | 3 NO,(9)+3CO(9) 3 NO(9)+3CO2(9)

CO2(g) + H2(g) « H2O(g) + CO(g) When H2(g) is mixed with CO2(g) at 2,000 K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured.                                      [H2]  = 0.20 mol/L                                   [CO2]  = 0.30 mol/L                      [H2O] = [CO]  = 0.55 mol/L (a)   What is the mole fraction of CO(g) in the equilibrium mixture? (b)   Using the equilibrium concentrations given above, calculate the value of Kc, the equilibrium constant for the reaction. (c)   Determine Kp in terms of Kc for this system. (d)   When the system is cooled from 2,000 K to a lower temperature, 30.0 percent of the CO(g) is converted back to CO2(g). Calculate the value of Kc at this lower temperature. (e)   In a different experiment, 0.50 mole of H2(g) is mixed with 0.50 mole of CO2(g) in a 3.0-liter reaction vessel at 2,000 K. Calculate the equilibrium concentration, in moles per liter, of CO(g) at this…