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A gas mixture contains 8.10g of N2, 1.70 g of H2, and 14.70 g of CH4. what is the mole fraction of H2 in the mixture
The X compound decolors in Bromine, bubbles in Na metal, changes from orange to green in Chromic Acid, and has no reaction with Lucas reagents.
decomposition of N2O5 to NO2 and O2 at 70 degree celsius is 6.82 x 10^-3 s-1. Suppose we start with 0.300 mol of N2O5(g) in a .500L container. How many minutes will it take for the quantity of N2O5 to drop to .030 moles?
The "roasting" of 48.7 g of ZnS at constant pressure gives off 220. kJ of heat. Calculate the DH for this reaction. 2ZnS(s) + 3O2(g) ® 2ZnO(s) + 2SO2(g)
This compound sloly isomerizes completely to compund B, which has the same formula, Sketch the structures of A and B, and explain why B might be more stable than A
Acetylene gas (ethyne; HC?CH) burns in an oxyacetylene torch to produce carbon dioxide and water vapor, and the heat needed to weld metals. The heat of reaction for the combustion of acetylene is -1259 kJ/mol. (a) Calculate the C?C bond energy, and..
how many moles of H2SO$ must eb used to produce 6.5 mol of water..?? Someone posted this question before and somehow NaOH
138g of K and 448g of I react completely to form KI. What mass of KI would have been produced if 138g of potassium and 41g of iodine has been used?
RNAse is an enzyme that cleaves the P-O5\' bond in RNA. It has two His residues in the active site. Suggest a plausible explanation
Iodine-131 is a radioactive isotope. After 5.00 days, 65.0% of a sample of 131I remains. What is the half-life of 131I? please show all details on how you got the answer im really trying to understand this
The stilbene molecule has seven double bonds, yet in this reaction, only one of them undergoes addition with the Br2 generated in the reaction mixture. What functional group(s) is(are) the other six bonds in, and what can you say about the reactiv..
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction C2H6 (g)+ H2 (g) -> 2CH4
Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ? CO(g) + H2O(g) The equilibrium concentrations of the reacting species.
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