A proper fuel-air mixture is most critical in the production of an efficient, nonluminous flame. For the ignition of an efficient Bunsen burner flame in the laboratory, identify the (most common) fuel and the required air component

Liquid pentane is burned with dry air and products are measured on a dry basis: CO2 10.1%, CO 0.2%, O2 9.5% remaining. N2 Find the enthalpy of formation for fuel and the true equivalence ratio.

The costs of petroleum and natural gas have increased dramatically since the early 1970s, and there is some question about their continued long-term availability. List as many alternative energy sources as you can think of, being as creative as you can, and then go back and suggest possible drawbacks to each one.

Differentiate the two types of flame produced by the Bunsen burner. Which type of flame is good for heating? Why? Under what conditions will the flame strike back? In what part of the Bunsen burner does the fuel burn when itstrikes back?

The air has a dry ball temperature of 34 ° C and a wet bulb temperature of 24 ° C is initially heated in a heater so that the dry ball temperature increases to 90 ° C. Then the air is passed through the pile of corn kernels to dry. The air that comes out of the corn kernels is at 60 ° C. Then this air is passed to the dehumidifier to reduce the RH to 10%. Draw the course of the process of changing the air on the psychometric chart. The airflow rate through the corn kernels pile and dehumidifier is 4.0 m / s and the pile cross-sectional diameter is 0.5 m. a. Determine the amount of moisture lost from the corn kernels pile (in grams of water / second) b. Determine the amount of water lost from the air when passing through the dehumidifier (in grams of water / second)

Gasoline contains a mixture of alkanes, some of which are octanes, C8H18 (l). The heat of the reaction is -5471 kJ/mol of energy.  The per mole is the coefficient in front of the compound in the equation.  If your tank holds 10 gallons of gasoline, how much energy of combustion is available, assuming the gasoline was pure octane? Density octane = 0.7025 g/mL and 1 gallon = 3.785 L

An empty coffee-cup calorimeter weighs 10 grams. It is filled with water, whose temperature is 31 degrees Celsius, and is weighed again. The weighing scale displayed 50 grams.A metal sample is heated to 90 degrees Celsius and then placed into the coffee-cup calorimeter. The cover, with a thermometer, is quickly put on top of the calorimeter. The temperature reading on the thermometer stabilized at 34 degrees Celsius. The mass of the metal is 6.54 grams. Use 4.184 J/g∙°C for the specific heat of water. What is the specific heat in J/g∙°C of the metal sample?

A student performed the procedure described in the lab manual using 48.9 mL of 1.0 M HCl and 49.9 mL of 1.0 M NaOH. Reaction caused the temperature inside the calorimeter to increase from 17.9 oC to 24.7 oC. What is the value of the enthalpy change for this reaction (ΔHaqueous) in units of kJ/mol? (Enter your answer as a number without units.)

How many moles of O2 are needed to burn 1.45 mol of C8H18? Express the amount in moles to three significant digits. The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2C8H18(l)+25O2(g)→16CO2(g)+18H2O(g)   Relevant volumetric equivalencies 1 gal = 3.785 L 1 L = 1000 mL

The amount of energy released by burning a fuel source, measured in energy per mass, is called the fuel value. If all of the energy obtained from burning 1.28 lb1.28 lb of methane (fuel value is 11.97 kcal/g)11.97 kcal/g) is used to heat 124.0 kg124.0 kg of water at an initial temperature of 18.7 ∘C,18.7 ∘C, what is the final temperature?