4. A technician needs to determine the concentration of a sulfuric acid solution. In an experiment, a 10.0 mL sample of sulfuric acid reacts completely with 15.9 mL or 0.150 M potassium hydroxide solution. Calculate the molar concentration of the sulfuric acid solution.
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- c. A mixture of propane and methane occupied 122 mL at 25⁰C and 1.0 atm. This mixture was totally burned in excess O2 to produce CO2(g) and H2O(g). The mass of the CO2 produced was 0.506 g. What is the mass % composition of the original mixture? Show all work.Use only the first decimal points (X.X) for atomic masses. R = 8.314 L*kPa/mole*K . In a 2.50 L reactor at 27 *C, sodium oxide captures CO2 from the gas phase by the following reaction:Na2O(s) + CO2(g) --> Na2CO3(s)36.2 g of Na2O(s) and 26.1 g of CO2(g) are placed into the reactor. What is the limiting reagent? Na2O(s) CO2(g) What is the final pressure of the system? kPaA gasification plant of MSW produces syngas of the following Component Composition (dry volume %) CO 30 H2 40 CO2 30 Determine the weight percentage of syngas component. (MW: CO =28; H2 = 2; CO2 = 44) (Hints: It is easier to start with 100 moles syngas and volume ratio is equal to molar ratio)
- A fuel contains 78wt% carbon and 22wt% hydrogen (H). Combustion results in the following composition by volume (dry basis): CO2 : 9.41 CO : 1.69 O2 : 3.8 N2: 85.1 The following equations describe the chemical reactions taking place: CO+0.5 O2→ CO2 C+O2→ CO2 H2 + 0.5 O2 → H2O C+0.5O2→ CO On the basis of 120 lb moles of dry flue gas, the O2 required (lb moles) for complete combustion is most nearly. Find the amount of O2 needed for the completion of combustionTo evaluate the use of renewable resources, an experiment was carried out with rice hulls. After pyrolysis, the product gas analyzed 6.4% CO2, 0.1% O2, 39% CO, 51.8% H2, 0.6% CH4, and 2.1% N2. It entered a combustion chamber at 90 °F and a pressure of 35.0 in. Hg and was burned with 40% excess air (dry) at 70 °F and an atmospheric pressure of 29.4 in. Hg; 10% of the CO remains. a. How many cubic feet of air were supplied per cubic foot of entering gas? b. How many cubic feet of product gas were produced per cubic foot of entering gas if the exit gas was at 29.4 in. Hg and 400 °F?The last calculation we need to do is find the %acetic acid (a.k.a the "acidity"). We can average all of the acetic acid masses from the completely reacted samples in the previous step. For now, let's assume we ended up with a final average mass of 2.37 g acetic acid consumed. If the initial volume of acetic acid used was 50.0 mL, what's the %m/v of acetic acid?
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- Eugenol, the main component of clove oil, can be prepared by heating 2-allyl guaiacol (in the absence of oxygen) to temperatures >205 °C. In practice, however, it is most cost-effective to extract eugenol from cloves, its natural source. Given a weight percentage of eugenol in cloves at 15.0%, calculate the minimum mass of cloves one needs to obtain 8.00 g of eugenol as a product. Report your answer (as a mass in grams, without units) with three significant digits.Gypsum (plaster of Paris : CaSO,. 2H,0) is produced by the reaction of calcium carbonate and sulfuric acid. A certain lime stone analyzes: CaCO, 96.89 %; MgCO, 1.41 %; inerts 1.70 %. For 5 metric tons of limestone reacted completely, determine: a. kg of anhydrous gypsum (CaSO,) produced. b. kg of sulfuric acid solution (98 wt%) required.What is the Molecular weight of a certain volatile liquid which is placed in 225 g flask which has total capacity volume of 251.07 ml where after the liquid was heated to 94.5 oC, the gas volatilized and the weight of the flask measured 227.08g.? Round you answer in one decimal place