Dinitrogen tetroxide was used as part of the fuel for the lunar lander in the Apollo missions.  It establishes the equilibrium below. N2O4 (g)   <-->   2 NO2 (g)     Kp = 0.133 If an unknown pressure of N2O4 was added to a reaction flask, and 90.0% of the N2O4 still remains once equilibrium has been established, what was the initial pressure that was added to the reaction flask?

Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO2(g)+ H2O(1)-2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 6.6 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO₂ 8.7 g H₂O 230.3 g HNO, 10.8 g NO 10.3 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 I Don't Know Submit 5 ? olo 2024 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility

Dinitrogen tetraoxide is a colorless gas at room temperature. It can dissociate into nitrogen dioxide, which is a reddish brown gas. N2O4(g)  2 NO2(g)   Three experiments were run starting with different initial amounts of N2O4(g) ([N2O4]0 in the table). The systems were allowed to reach equilibrium and the concentrations for each gas were measured (in units of moles/Liter).For each of the boxes below, calculate the ratios indicated by the column heading. This will show the mathematical relationship that exists between the concentrations of NO2 and N2O4 at equilibrium.Be sure to round to the correct number of significant figures. Exp [N2O4]0   [NO2] [N2O4]   [NO2] / [N2O4]   2 [NO2] / [N2O4]   [NO2]2 / [N2O4] 1 3.7   2.92 2.2             2 2.8   2.49 1.6             3 2.6   2.33 1.4             Based on your calculations, indicate whether each statement is True (T) or False (F):   1. Each experiment started with a different initial concentration of N2O4.   2. The…

For the following reaction at a certain temperature H2(g) + F2(g) = 2HF(g) the equilibrium concentrations in a 10.00-L rigid container are [H2] = 0.0600 M, [F2] = 0.0200 M, and [HF] = 0.620 M. If 0.220 moles of F2 is added to the equilibrium mixture, calculate the concentration of H2 after equilibrium is reestablished.