A coal sample having the following composition: C = 80%, H = 4%, O = 3%, S = 2%, N = 3%, ash = 5% and moisture = 3%. Calculate the quantity of air needed for the complete combustion of 1 kg of coal, if 60% excess air is supplied. %3D
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- Dodecane C12H26 is burned at constant pressure with 150% excess air. What is the air-fuel for this process.Using the standard heats of formation values from the data booklet and the following reaction equation: N2H 4(1) + 3O2(g) 2 NO2(g) + 2 H2O(l) + 555.2 kJ a Calculate the standard heats of formation of N2H4 liquid. b. Using the reaction equation, calculate the amount of heat energy released on the combustion of 100.0 g of hydrazine (N2H4). c. Sketch the energy profile for the above reaction and label the Ea and AH rxn on the graph.PLEASE ESTABLISH BASIS ON THE STACK GAS A burner used Pittsburgh coal analyzing 14.1% ash, 2.1% N, 4.3% S. Excess air is supplied dry at 22⁰C and 1 atm. The stack gases at 285⁰C, 765 mmHg analyzes 9.65% CO2, 1.16% CO, 0.24% SO2, 0.58% H2 and 9.16% O2. Calculate: a) % excess air b) complete ultimate analysis of the coal, c) m3 air/kg coal and d) m3 stack gas /kg coal.
- If to a solution of NaOH, in water and ethanol (20 ° C) 3 mmol of A (106.11 g / mol) and 2 mmol of B (58.06 g/ mol) and stirred magnetically for 10 minutes. After the reaction is completed, we proceed to isolate (work- up) and purify at C (246.29 g/ mol) yielding 0.300 g of the pure product. Calculate the% return for C showing his work. please show every single step and calculationsCarbon dioxide gas, CO2(g), is generated in the combustion of a sample of ethane (C2H6). This CO2 is all bubbled into aqueous barium hydroxide to be absorbed to produce 0.506 g of solid barium carbonate precipitate. How many grams of ethane (C2H6) were initially burned? The absorption-precipitation reaction is given by [CO2(g) + Ba(OH)2(aq) BaCO3(s) + H2O(l)].Mass analysis of a fuel is 84.6% carbon, 11.4% hydrogen, 0.4% sulphur, 2.4%oxygen, and 1.2% impurities. Calculate the heating value of the fuel and the theoretical mass of air required for complete combustion of 1kg of fuel.Take mass analysis of air as oxygen 23% and nitrogen 77%Element/heating value(MJ/kg)/relative atomic masshydrogen/144/1carbon/33.7/12sulphur/9.3/32oxygen/0.0/16
- The following reaction using hydrogen and oxygen is carried out in a bomb calorimeter: 2H2(g) + O2(g) → 2H2O(l) The specific heat of the reaction vessel is 0.200 kcal/0C-kg and the specific heat of water is 1.00 kcal/0C-kg. Assuming that m is 0.1 mole of water was formed in the experiment and Q is 7.2 kcal, calculate the heat of the reaction per mole of liquid water.In an Orsat analysis the % CO2 of the product of the combustion is 20% . If percent excess air is 30% . find the maximum percentage of CO2 attainable.Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 3.06 g/L at 14 °C and 0.974 atm. Calculate the average molecular mass for this sample
- Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and difluorormethane (CH2F2) has a density of 1.43 g/L at 26 °C and 0.405 atm. Calculate the average molecular mass for this sample. Calculate the volume percentage of CH2F2 in the sample.Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and 111-trifluoroethane (C2H3F3) has a density of 2.39 g/L at 23 °C and 0.593 atm. 1. Calculate the average molecular mass for this sample. 2. Calculate the volume percentage of C2H3F3 in the sample.Chlorodifluoromethane (CHF2Cl) was widely used in the compression/cooling circuits of refrigeration or air-conditioning systems. Since the discovery that such compounds (HCFCs and CFC's) released into the atmosphere were a major cause of depletion of stratospheric ozone, newer refrigeration systems make use of certain hydrofluorocarbons (HFCs), which are degraded in the lower atmosphere, instead. Often, mixtures of such compounds are used. Suppose a sample of refrigerant gas consisting of a simple mixture of the gases pentafluoroethane (C2HF5) and 111- trifluoroethane ((C2H3F3) has a density of1.95 g/L at 23 °C and 0.432 atm. Calculate the average molecular mass for this sample. Calculate the volume percentage of C2H3F3 in the sample.