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An environmental engineer analyzes a sample of air contaminated with sulfur dioxide. To a 500. mL sample of air at 700. torr and 38°C, she adds 20.00 mL of 0.01017 M aqueous iodine, which reacts as follows:2SO2(g) + I2(aq) + 2H2O(l) → 2HSO41-(aq) + 2I1-(aq) + 4H+(aq)The excess I2(aq) left over from the above reaction was titrated with 11.37 mL of 0.0105 M thiosulfate (S2O32-) as follows: I2(aq) + 2S2O32-(aq) → 2I1-(aq) + S4O62-(aq)What is the volume % of SO2 in the original air sample?
What is the final temperature when 125 g of iron at 92.3 °C is dropped into 50.0 g of water at 27.7 °C? The specific heat of iron is 0.444 J g-1 °C-1 and the specific heat of water is 4.184 J g-1 °C-1.
Write a balanced equation for the conversion of C6H5CHOHCH3 to the methyl ketone in the presence of I2 and NAOH
Important information about Conceptual Organic chemistry and What chemical tests might be used to distinguish between pentanal and 2- pentanone; between benzyl alcohol and diphenylmethanol?
If 3.8kcal of energy is released when 1 gram of glucose is combusted, how many kcals are released when 0.689 moles of glucose are combusted
calculate the amount of heat transfered when 24.0 g of CH3OH decompose at constant pressure. delta H is 126.4 kJ
An unknown compound has the empirical formula CH2. A 0.050-mol sample of this compound weighs 4.20 g. What is the molecular formula of this compound?
Total pressure in kPa 10 seconds after initiation of the reaction if initially there was 88.3kPa of pure N 2 O 5 vapor Enter the total pressure in kPa 10 minutes after initiation of the reaction.
The solubility of CaSO4 in pure water at 0.0 C is 1.13 gram per liter; what is the value of solubility product
12.0 moles of gas are in a 8.00 L tank at 23.2 C. Calculate the difference in pressure between methane and an ideal gas under these conditions.
How many milliliters of 0.200 M NaOH will be required to titrate 14.5 mL of 0.479 M H2SO4?
Acid Mixture Problem, From a full 50-liter container of a 40% concentration of acid, x liters is removed and replaced with a 100% acid.
A first order reaction has an activation energy of 65.7 kJ/mol and a frequency factor (Arrhenius constant) of 2.36 x 1013 sec -1. Calculate the rate constant at 18 oC
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