Chemistry

Chemistry, 30.06.2019 00:40, mahaypatto

Activity b (continued from previous page) 3. gather data: experiment with a variety of initial concentrations of no2 and n2o4. for each set of initial concentrations, use the gizmo to determine the equilibrium concentrations of each substance.

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Chemistry, 26.06.2019 09:30, genyjoannerubiera

Gather data: experiment with a variety of initial concentrations of no2 and n2o4. for each set of initial concentrations, use the gizmo to determine the equilibrium concentrations of each substance. in the last column, find kc for that trial. run three trials for each set of initial conditions.

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Chemistry, 27.06.2019 09:30, Homepage10

Gather data: experiment with a variety of initial concentrations of no2 and n2o4. for each set of initial concentrations, use the gizmo to determine the equilibrium concentrations of each substance. in the last column, find kc for that trial. run three trials for each set of initial conditions.

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Chemistry, 20.08.2019 17:20, livvyr0cks

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 3.5 2.85 2.1 2 3.0 2.56 1.7 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 ratio ([no2] / [n2o4]) is equal to a constant value. 3. the ratio (2 [no2] / [n2o4]) is equal to a constant value. 4. the ratio ([no2]2 / [n2o4]) is equal to a constant value. 5. each experiment reached a different set of equilibrium concentrations.

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Chemistry, 10.09.2019 05:20, Bellaburrito

Astudent performs a kinetic experiment on the first-order kinetics of the reaction: n2o42no+o2. she calculates the first-order decomposition of the reactant using the relationship: [n2o4]t=[n2o4]0e-kt using the first-order rate constant k = 0.750 s-1 and the following data: initial mass of n2o4: 25.7  0.3 g, initial volume of n2o4: 0.22 0.01 l, and time t = 3.8  0.2 s. use error analysis to calculate her reported concentration of n2o4 including the range of uncertainty.

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