Chemistry

Chemistry, 13.07.2019 18:40, parbridg

Calculate the standard entropy change for the dimerization of no2: 2 no2(g) → n2o4(g) at 298 k, if s ◦ ∆h◦ f j k·mol kj mol no2(g) 240.06 33.18 n2o4(g) 304.29 9.16 answer in units of j k · mol

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Chemistry, 25.07.2019 07:00, zetrenne73

Consider the reaction 2no2(g) → n2o4(g) and δg∘(no2(g)) = 51.84 kj/mol, δg∘(n2o4(g)) = 98.28 kj/mol. calculate δg at 298 k if the partial pressures of no2 and n2o4 are 0.38atm and 1.64atm , respectively.

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Chemistry, 06.08.2019 02:20, NoodlesYT

The brown gas no2 and the colorless gas n2o4 exist in equilibrium,2no2 n2o4.in an experiment, 0.625 mole of n2o4 was introduced into a 5.00 l vessel and was allowed to decompose until equilibrium was reached. the concentration of n2o4 at equilibrium was 0.0750 m. calculate kc for the reaction.0.0500.07500.100.1257.5

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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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Calculate the standard entropy change for the dimerization of no2: 2 no2(g) → n2o4(g) at 298 k, if...

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