A 208 g of C6H6 (78 g/mol.) burns in air according to the equation: CSH6 + O2 C02 +H2O What mass of CO2 (44 g/mol.) is produced?
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- The change in internal energy for the combustion of 1.0 mol of octane at a pressure of 1.0 atm is -5084.3 kJ . If the change in enthalpy is -5074.0 kJ , how much work is done during the combustion? Express the work in kilojoules to three significant figures.Chloroform, CHCl3 a volatile liquid, was once used as an anesthetic but has been replaced by safer compounds. Chloroform boils at 61.7°C and has a heat of vaporization of 31.4 kJ/mol. What is its vapor pressure at 37.2°C?(a) What is the physical significance of energy of activation ? Explain with diagram.(b) In general, it is observed that the rate of a chemical reaction doubles with every 10 degree rise in temperature. If the generalization holds good for the reaction in the temperature range of 295 K to 305 K, what would be the value of activation energy for this reaction ?[R = 8.314 J mol-1 K-1]
- Determine the theoretical oxygen demands for the following chemicals and show the balanced stoichiometric equations with your work: a) 150 mg/L ethanol, b) 0.5 mg/L pentachlorophenol (chloride will end up being OCl- when oxidized), and c) 100 mg/L isopropanolThe Bunsen burner in your labs are fueled by natural gas, which is mostly methane, CH4. The thermochemical equations for the combustion of methane (burning in oxygen) is: CH4(g) + 2 O2(g) ➔ CO2(g) + 2 H2O (g) ΔH = – 890.3 kJ/mole Calculate ΔH in kJ when 5.00 g CH4 react with an excess oxygen.Cellulose is to be burned in a waste to energy facility. The chemical equation for cellulose is C6H10O5. The atomic weights of C, H, and O are 12, 1, and 16, respectively. The ideal equation for the combustion of cellulose is C6H10O5 +6O2à6CO2 + 5H2O. Calculate the stoichiometric oxygen necessary for the combustion of cellulose. Calculate the stoichiometric air supply. The air is 23.15% oxygen by weight. If the facility operates at 1.5 tons/hour at 100% excess air. How much air is required?
- Environmental Engineering When methanol is used to generate hydrogen, it reacts with the following reaction: CH3OH>>>>CO+2H2 The reaction is second order in methanol, and it is observed that 100g of carbon monoxide can be produced in one day in a batch reactor, if you start with 200g of methanol. What is the rate constant for this reaction?Please solve and show all work with units Determine the total Theoretical oxygen demand for both carbon and nitrogen compound containing a total oxygen required for NO2- of 100 mg/l and the sample Nh4+ originally having 14 mg/l as N. C6H12O6N2 + O2 + H+ ➔ CO2 + H2O + NH4 + NH4 + + O2 ➔ NO2 - + H+ + H2O NO2 - + O2 ➔ NO3 -Convert the following species from mg/L as the ion to mg/L as CaCO3 83 mg/L Ca2+ 48 mg/L CO2 220 mg/L HCO3- 15 mg/L CO32-
- Write down the chemical formulae for the combustion of the alkanes in Table 3.2 with n = 2 to n = 8. Determine the mass of CO2 produced per megajoule of energy.The ideal equation for the combustion of cellulose is C6H10O5 + 6O26O2 + 5H2O. What is a similar idealized equation for pyrolysis? What end products might you expect?The combustion of pure hydrogen by the reaction 2H2+O22H2O produces 142 MJ per kg of hydrogen. Compare the energy per kg of octane and the total energy from the individual combustion of its carbon and hydrogen atoms.