Aerobic cells
Calculate the volume of oxygen required at STP to metabolize 0.025 kg of glucose
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Thermodynamics, Statistical Thermodynamics, & Kinetics
- a 1.2 mol sample of oxygen is placed in a 20L tank at 100kPa, whta is tthe tank temperature?arrow_forwardGaseous ammonia is injected into the exhaust stream of a coalburning power plant to reduce the pollutant NO to N2 according to the reaction:4 NH3( g) + 4 NO( g) + O2( g)----> 4 N2( g) + 6 H2O( g)Suppose that the exhaust stream of a power plant has a flow rate of 335 L/s at a temperature of 955 K, and that the exhaust contains a partial pressure of NO of 22.4 torr. What should be the flow rate of ammonia delivered at 755 torr and 298 K into the stream to react completely with the NO if the ammonia is 65.2% pure (by volume)?arrow_forwardConsider a mixture of H2 (g) and I2 (g). Determine the ratio of the root-mean-square speed of H2(g) and I2 (g) molecules in the reaction mixturearrow_forward
- The mole fraction of neon in dry air near sea level is 0.00001818, where the molar mass of neon is 20.183. The partial pressure of neon when the total atmospheric pressure (dry air) is 97.5 kPa is_____ kPa.arrow_forwardA reservoir contains 2.83 m3 of carbon monoxide at 6895 kPa and 23.6oC. An evacuated tank is filled from the reservoir to a pressure of 3497 kPa and a temperature of 12.4oC,while the pressure in the reservoir decreases to 6105 kPa and the temperature to 18.3oC.What is (a) the volume of the evacuated tank? How much mass of CO transferred from the reservoir.arrow_forwardChemistry Calculate the mass of barium iodate that can disolve in 500 mL of water at 25ºC. Kps(Ba(IO3)2)= 1.57 x 10-1 PM (Ba(IO3)2) = 487.13 g*mol-1arrow_forward
- Nitric oxide (NO) reacts with molecular O2. determine the partial pressures of gases remaining at the end of the reaction. Given 4.00L and 0.500atm NO and 2.00L and 1.00atm O2. The temperature remains constant at 25Carrow_forwardname and define K,Kc and K1c .explain the differences and conditions under which each parameter applies.state the units for each parameter.arrow_forwardCombustible vapor-air mixtures are flammable over a limitedrange of concentrations. The minimum volume % of vapor thatgives a combustible mixture is called the lower flammable limit(LFL). Generally, the LFL is about half the stoichiometric mix-ture, the concentration required for complete combustion of thevapor in air. (a) If oxygen is 20.9 vol % of air, estimate the LFL forn-hexane, C₆H₁₄. (b) What volume (in mL) of n-hexane (d=0.660 g/cm³) is required to produce a flammable mixture of hexane in 1.000 m³of air at STP?arrow_forward
- 4a Assume that worldwide combustion of fossil fuel accounts for an energy use of 500 x 1015 kJ/year. Also, assume that all fossil fuels can be represented by the formula C3H5 with energy content of 32,500 kJ/kg.Finally, assume that air is 79% N2 and 21% O2 , and has a molecular weight of 29 kg/kmol. i. Estimate the annual release of CO2 to the atmosphere by burning fossil fuels, in kg/yr ii. If all that CO2 entered the atmosphere (and none was removed), estimate the increase in atmospheric concentration, in ppm by volume. Assume the atmosphere contains 6.7 x 1018 kg of air.arrow_forward1.) Clouds of hydrogen molecules have been detected deep in an interstellar space. It is estimated that these clouds contain about 1 x 1010 hydrogen molecules per m3, and have a temperature of just 25 K. Using these data, find the approximate pressure in such a cloud. 2.) A vessel of volume 22.4 L contains 2.0 mol H2 and 1.0 mol N2 at 273.15 K initially. All the H2 reacted with sufficient N2 to form NH3. Calculate the partial pressures and the total pressure of the final mixture.arrow_forwardThe oxidation of nitrogen oxide produces nitrogen dioxide. As shown : 2NO(g) + O2(g) -> 2NO2 (g) if 0.400 moles of NO(g) and 0.140 moles of O2 (g) are reacted in a 2.50m3 vessel at 298 K how many moles of NO2 (g) will be produced?arrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning