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Calculate the mass of CaCO3 (MM = 100.0 mg/mmol) produces from heating 400.0 mg of CaC2O4•H2O (MM = 146.00 mg/mmol).
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- i) Calculate the amount of potassium chloride that is needed to prepare two litres of a 1.45 molar potassium hydroxide solution. ii) Write a balanced equation for the combustion reaction of butanePart C in Liters (L) At 25 °C and 1.0 atm pressure, what is the minimum quantity of dry air needed to combust 1.2 L of CH4 (g) completely to CO2(g)? Remember that oxygen is present in the atmosphere to the extent of 209,480 parts per million. Express your answer using two significant figures.How many moles of NO2 would be required to produce 5.63 moles of HNO3 in the presence of excess water in 3 NO2(g)+H2O(I)—>2 HNO3(g)+NO(g)
- If cobalt(II) sulfate is heated too strongly, the following reaction will occur CoSO4(s) à CoO(s) + SO3(g) If you are heating a sample of CoSO4·6H2O and this reaction occurs along withdehydration, what will happen to the experimental percent water? Explain your answer.At 1.00 atm and 0 °C, a 5.04 L mixture of methane (CH4) and propane (C₂H₂) was burned, producing 16.5 g CO₂. What was the mole fraction of each gas in the mixture? Assume complete combustion. Xmethane = XpropaneWhat volume of groundwater containing 2 mg l−1 dissolved oxygen (DO) would be required to oxidize 23 liters of octane that leaked out of an underground storage tank (UST) and into an unconfined aquifer?
- What mass of carbon dioxide is formed from burning one gallon of octane, C8H18? Octane has a density of 703 kg/m3.1 L = 0.2642 gal 1 lb = 453.592 gAn average tree absorbs 48 pounds of CO2 in one year. How many trees would you need to plant to offset the CO2produced from burning one gallon of octane every day for one year (365 days)?What mass of silver oxide, ag2o, is required to produce 25.0 g of silver sulfadiazine, agc10h9n4so2, from the reaction of silver oxide and sulfadiazine?2C10H10N4SO2 + Ag2O ==> 2AgC10H9N4SO2 + H2OEqual length of magnesium ribben are taken in two test tubes ‘A’ and ‘B\ H2SO4 is added to test tube ‘A’ and H2CO3 in the test tube ‘B’ in equal amounts:(a) Identify the test tube showing vigorous reaction.(b) Give reason to support your answer.(c) Name the gas liberated in both the tubes. How will you prove its liberation?(d) Write chemical equations for both reactions.(e) Out of the two acids taken above(i) which one will have lower pH value.(ii) lowerH+ concentration respectively.