A 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)
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A 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)
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- Determine the quantity of energy given 10.95 dm³ of oxygen gas at STP reacts in this equation" 3O2(g) + 4AlBr3(s) --> 2Al2O3(s) + 6Br2(l) + 90.23kJ kJ = (10.95dm³ O2 / 1) * (A/B) * (C/D) = E 1. Regarding (A/B) which statements may be used? 1 L 3 mol O2 +90.23 kJ 22.4 dm³ O2 -90.23 kJ 1 dm³ 1 mol O2 2. Regarding (C/D), what are the values of these variables?Methane (CH4) is burned with air (79% N2 and 21% O2 by volume) at atmospheric pressure. The molar analysis of the flue gas yields CO, %3D 10.00%, O2 = 2.41%, C0= 0.52%, and N2 = 87.07%. Balance the combustion %3D equation and determine the mass air-fuel ratio, the of stoichiomet- percentage ric air, and the of excess air. percentageA fuel composed entirely of methane (CH 4 ) and nitrogen (N 2 ) is burned withexcess air. The flue gases analyze 7.5% CO 2 , 7% O 2 and the remainder, N 2 .Calculate:(a) percentage of excess air(b) analysis of fuel gas(c) analysis of flue gas (wet basis)
- To 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?1. 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).Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin (C,H;(NO3),) into gaseous dinitrogen, 5 gaseous dioxygen, gaseous water and gaseous carbon dioxide. x10 2. Suppose 30.0 L of carbon dioxide gas are produced by this reaction, at a temperature of -7.0 °C and pressure of exactly 1 atm, Calculate the mass of nitroglycerin that must have reacted. Round your answer to 3 significant digits. g
- - = T C 54°F Humid % Explanation O CHEMICAL REACTIONS Percent yield of chemical reactions 2 W |HC|HL| (@F11218HCHIHUSI https://www-awu.aleks.com/alekscgi/x/Isl.exe/10_u-IgNslkr7j8P3jH-IBMBkpcnaFu0F7Uj... FAX S Check بهر 3 * E $ X Gaseous ethane (CH₂CH3) reacts with gaseous oxygen gas (O₂) to produce gaseous carbon dioxide (CO₂) and gaseous water (H₂O). If 0.469 g of water is produced from the reaction of 0.90 g of ethane and 5.2 g of oxygen gas, calculate the percent yield of water. Round your answer to 2 significant figures. 4 0 d R DE C Ś 96 % 5 T 6 G H "4+ & 7 B N U 144 * 00 C | 141 | a A 8 1 D-II ( 9 r K M || a ✓ DDI O s ) B Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | | O F ▬▬▬▬▬▬ fo 1 11² a P MC - MC insert C + 3/5 = prt sc } ♡ 4 Privacy Center Privacy Center | Acces 1 0 Chisom Seve E d 11:10 10/22/20Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. The Swedish chemist Alfred Nobel (1833-1896) founded the Nobel Prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. 1. Write a balanced chemical equation, including physical state symbols, for the On decomposition of liquid nitroglycerin (C;H;(NO3),) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide. 2. Suppose 74.0 L of carbon dioxide gas are produced by this reaction, at a temperature of - 13.0 °C and pressure of exactly 1 atm. Calculate the mass of nitroglycerin that must have reacted. Round your answer to 3 significant digits.How many of the following are found in 15.0 kmol of xylene (C3H10)? (a) kg C3H10; (b) mol C3H10; (c) Ib-mole C3H10: (d) mol (g-atom) C; (e) mol H; (f) g C; (g) g H; (h) molecules of C3H10.
- 1. A boiler burns fuel oil with the following analysis by mass : 80% C 18% H2 2%S 30% excess air is supplied to the process. Calculate the stoichiometric ratio by mass and the % Carbon Dioxide present in the dry products. (15.62/1 14.9% CO2) 2. A boiler burns coal with the following analysis by mass : 75% C 15% H2 7%S remainder ash Calculate the % Carbon Dioxide present in the dry products if 20% excess air is supplied. (16.5% CO2) 3. Calculate the % of each dry product when coal is burned stoichiometrically in air. The analysis of the coal is: 80% C 10% H2 5% S and 5% ash. (76.7%N, 22.5% CO2 0.8% SO2)Example 1: Ethane (C2H6) is burned with atmospheric air and the volumetric analysis of the dry products of combustion yields the following: 10% CO2, 1% CO, 3% 02 and 86% N2. Develop the combustion equation and determine (a) the percentage of the excess air (b) the air fuel ratio. (Solve for 100 kmol of dry products).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.