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The reaction 2 NO2(g) + O3(g) N2O5(g) + O2(g) was studied at a certain temperature with the following results: Experiment [NO2(g)] (M) [O3(g)] (M) Rate (M/s) 1 0.835 0.835 47900 2 0.835 1.67 95800 3 1.67 0.835 95800 4 1.67 1.67 1.92e+05 (a) What is the rate law for this reaction? A) Rate = k [NO2(g)] [O3(g)] B) Rate = k [NO2(g)]2 [O3(g)] C) Rate = k [NO2(g)] [O3(g)]2 D) Rate = k [NO2(g)]2 [O3(g)]2 E) Rate = k [NO2(g)] [O3(g)]3 F) Rate = k [NO2(g)]4 [O3(g)] (b) What is the value of the rate constant? (c) What is the reaction rate when the concentration of NO2(g) is 0.842 M and that of O3(g) is 1.82 M if the temperature is the same as that used to obtain the data shown above?
How many grams of sulfur (S) are needed to react completely with 326 g of mercury (Hg) to form HgS?
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Determine the concentration of the sodium hydroxide solution? Considering this balanced equation given as :
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Suppose that 180 g of ethanol at 26 ? C is mixed with 225 g of ethanol at 83 ? C at constant atmospheric pressure in a thermally insulated vessel.
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draw a lewis structure of the molecule and indicate the number of bonds and orbitals used in bonding. Show electron configurations of the central bonding atom in both the unhybridized and hybridized states.
determine the number of stereoisomers for the following. Sketch these isomers and identify pairs of enantiomers ABA,
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