Consider the following reaction: N2(g) + 3H2(g) ⇌ 2NH3(g) In a given experiment, 1.21 moles of N2(g) and 4.01 moles of H2(g) were placed in a 4.63 L vessel. Complete the following table by entering numerical values in the Initial row and values containing the variable "x" in the Change and Equilibrium rows. Define x as the amount (mol/L) of N2 that reacts to reach equilibrium. Include signs in the Change column to indicate a gain or loss of concentration. (Omit units and spaces, use 3 sig. fig. and write concentration less than 1 as 0.###, not as .###. If nothing is present initially, enter 0 for the molarity.) [N2] (M) [H2] (M) [NH3] (M) Initial Change Equilibrium At a particular temperature, the equilibrium concentration of NH3 is found to be 0.279 M. Given this information, determine the numerical value of K for this reaction, at this temperature. (If you want to enter your answer in scientific notation, use the format as shown below: 2.5 x 10-3 = 2.5E-3)
Consider the following reaction:
N2(g) + 3H2(g) ⇌ 2NH3(g)
In a given experiment, 1.21 moles of N2(g) and 4.01 moles of H2(g) were placed in a 4.63 L vessel. Complete the following table by entering numerical values in the Initial row and values containing the variable "x" in the Change and Equilibrium rows. Define x as the amount (mol/L) of N2 that reacts to reach equilibrium. Include signs in the Change column to indicate a gain or loss of concentration. (Omit units and spaces, use 3 sig. fig. and write concentration less than 1 as 0.###, not as .###. If nothing is present initially, enter 0 for the molarity.)
| [N2] (M) | [H2] (M) | [NH3] (M) | |
| Initial | |||
| Change | |||
| Equilibrium |
At a particular temperature, the equilibrium concentration of NH3 is found to be 0.279 M.
Given this information, determine the numerical value of K for this reaction, at this temperature.
(If you want to enter your answer in scientific notation, use the format as shown below:
2.5 x 10-3 = 2.5E-3)
K =
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