3. Given: Soda and lime are added to a glass batch in the form of soda ash (Na₂CO,) and limestone (CaCO₂). During heating, these two ingredients decompose to give off carbon dioxide (CO₂), the resulting products being soda and lime. Find: Compute the weight of soda ash and limestone that must be added to 110 lb of quartz (SiO;) to yield a glass of composition 72 wt% SiO₂, 16 wt% Na:0, and 12 wt% Cao. Solution:
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- When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction CaCO3(s)→CaO(s) + CO₂(g) What is the mass of calcium carbonate needed to produce 35.0 L of carbon dioxide at STP? Express your answer with the appropriate units. View Available Hint(s) mass of CaCO3 Submit = Part B 0 370.8 HÅ atm Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining ? Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C4H10 (9) + 1302 (g)→8CO2 (g) + 10H₂O (1) At 1.00 atm and 23 °C, what is the volume of carbon dioxide formed by the combustion of 2.20 g of butane? Express your answer with the appropriate units.• Two methanol-water mixtures are contained in separate flasks. The first mixture contains 40 wt% methanol and the second contains 70 wt% methanol. If 300g of the first mixture is combined with 400g of the second, what is the mass fraction of the methanol in the product? O a. 0.119 O b. 0.571 O c. 0.276 О с. O d. 0.765To 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?
- 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.Q4/ In the process for the manufacture of chlorine, HCI and O₂ react to form Cl₂ and H₂O. Sufficient air is fed to provide 35% excess oxygen, and the conversion of HCI is 85%. Determine the amount of air fed into the process. And calculate the mole fractions of the product stream components.A chemical manufacturer produces ethylene oxide by burning ethylene gas with air in the presence of catalyst. If the conditions are carefully controlled, a substantial fraction of ethylene remains unconverted and some is completely oxidized to form carbon dioxide and water. Formation of carbon monoxide is negligible. After the gases leaving the absorber is as follows: 9.6%CO2, 3.0%O2 and 6.4% ethylene. Of the ethylene entering the reactor, what percentage is converted to ethylene oxide?
- + |/ 00 %24 D. Two bulbs are connected by a stopcock. The 7.50 L bulb contains nitric oxide (NO) at a pressure of 0.340 bar, and the 2.50 L bulb contains oxygen (O,) at a pressure of 0.510 bar. 02 ON After the stopcock is opened, the gases mix and react to produce nitrogen dioxide (CON) 2 NO(g) + 0,(g) – 2 NO,(g) Considering that the volume remains unchanged during the experiment, how does the total pressure in the bulbs change if the reaction is allowed to go to completion? The total pressure will remain constant. O There is not enough information to determine how the total pressure will change. O The total pressure will decrease. O The total pressure will increase. MacBook Pro ( The %23 %24 7. 4. 5. 3. R %3D K. H. B C. option command MOSISO1. In a 100mL sealed flask, 0.1 g of H2 gas reacts with 0.15 g of N2 gas to generate NH3 gas at 25 oC . Note: Consider that i) the initial and final temperatures are 25 oC; ii) all of the limiting reagent is converted to NH3; and iii) the gases behave as ideal. a) Balance the chemical equation :N2(g) + H2(g) ---> NH3(g) b) Calculate the initial pressure inside the flask (before N2 and H2 react). Calculate the initial partial pressures of N2 and H2 (before N2 and H2 react) c) Calculate the final pressure inside the flask (after N2 and H2 react to generate NH3). Calculate the final partial pressures for N2, H2 and NH3 (after N2 and H2 react to generate NH3).The production of cement results in significant GHG emissions. The emissions are caused by the decomposition of calcium carbonate (limestone) to calcium oxide (lime) and carbon dioxide. This process known as calcination, is carried out in kilns. Therefore, additional GHGs are emitted as a result of heating the kilns. A large cement manufacturer uses a mix of coal, natural gas, and biomass in its boiler. This mix produces the following amounts of GHGs per Million BTUs of energy: • 250 lbs CO2/MMBtu • 5 lbs CH4/MMBtu • 0.36 lbs N2O/MMBtu Process carbon emissions from the calcination process produce 925 lbs of carbon dioxide per metric ton of cement. In addition, the plant uses 1.7 Million BTUs of energy per metric ton of cement. If the plant produces 180,000 metric tons of cement annually, how many metric tons of CO2e does it emit?
- The liquefied petrolieum gas(LPG) is composed of 80% C;Hg and 20% C4H10 in mass basis. (1). Determine the molar fraction of C3H8 and C4H10 in LPG. (2). Determine the stoichiometric air fuel ratio of the LPG. (3). Determine the lower heating value of LPG in kJ/m³ at 25°C and 100 kPa. (4). LPG is mixed with excess air to burn in a boiler at 100 kPa. The CO2 in burned gas is 7% on dry basis. Determine the equivalence ratio of the mixture.Q3-A stream of humid air enters a condenser in which 95% of the water vapor in the air is condensed The flow rate of the condensate (the liquid leaving the condenser) is measured and found to be 225 L/h. Dry air may be taken to contain 21 mole% oxygen, with the balance nitrogen. Calculate the flow rate of the gas stream leaving the condenser and the mole fractions of oxygen, nitrogen, and water in this stream. (mol dry air/h) 0.21 mol 02/mol 0.79 mol N/mol nglmol H,0/h) na(mol 02/h) ig(mol N/h) ng(mol H20 (v)/h) 225 liters H20 (1)/h nz(mol H20 (1)/h) (95% of water in feed)A sample of unknown gas was heated to 125°C in a round bottom flask at standard pressure (1.00 atm), and its weight in a 100 ml round bottom flask was taken to be 30.098g. The round bottom flask weighs 30.0g. The gas was determined to be pure so that it can only be composed of a single element (N2, O2, F2, He, Ne, Ar, P2, S2, Cl2). Identify the gas.