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The alcoholic blue solution from part I of your experiment is commonly utilized in weather-forecasting devices. Based on your observations in the lab define how this reaction can indicate coming rain.
at what temperature should the tube be maintained to have a partial pressure of 1.0mm of O2 in the exit gas? Assume that the total pressure of the gas in the tube is 1.30atm.
What is the maximum mass, in gram, of Fe3O4, that can be produced from this reaction? B)If 3.26 g of Fe3O4 are actually made, what is the percent yield of this process
Find the heat of combustion in kJ/g for each gas. These values are valid at 25°C, where the water produced by the reaction is in the liquid state.
How might you use 13C NMR spectroscopy to determine if the brominated product is contaminated with some unreacted starting material (during the bromination of trans-cinnamic acid)
pure benzene has a normal freezing point of 5.5degc. a solution containing 11.4g of a molecular substance dissolved in
Consider the following reaction: SO2Cl2 (g) SO2 (g) + Cl2 (g). K = 2.99*10^-7 at 227 degrees celsius. If a reaction mixture initially contains 0.159 , what is the equilibrium concentration.
A system that had work done on it but which receives or loses no heat from or to the surroundings has
A solution of acetic acid is 40% m/m with density = 1.045 g/mL. Calculate molarity, molality, and mole percent of the acid. Molecular weight of acetic acid = 60.05 g/mol
Calculate the concentration of the acid solution after all teh metal has reacted. Assume that the volume remains unchanged.
What must the Celsius temperature be if 2.0 moles of a gas in a 4.0 L steel container has a measured pressure of 100 atm
the pH of a saturated solution of a metal hydroxide MOH is 10.85 calculate the Ksp for the compound
Provide calculations and explain how 100 ml of 0.5 M NaCl in 25 mM sodium phosphate buffer, ph 8, will be prepared.
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