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1. Determine the adiabatic flame temperature of methane (CH4) burned in 400.% theoretical air in a steady flow process.
2. Determine the adiabatic flame temperature of acetylene (C2H2) burned in a steady flow process with (a) 100.% theoretical air, (b) 200.% theoretical air, and (c) 400.% theoretical air.
Calculate the pH of a solution formed by mixing 10.0 mL of 0.100 M HBr with 20.0 mL of 0.200 M HCl.
How many joules of heat are required to heat 143 g of aluminum from 55.0 oC to 66.5oC?
a 1.00 liter solution contains 1.00 mol of weak acid HX. After 0.60 mol of Oh- is added to this olution, the pH of the solution is 4.00. Calculate the Ka for the acid HX.
Consider the reaction CaCN2 + 3 H2O ! CaCO3 + 2 NH3 . How much CaCO3 is produced if 47.5 moles NH3 are produced?
When lithium oxide (Li2O) is dissolved in water, the solution turns basic from the reaction of the oxide ion (O^2-) with water. Write the equation for this reactionand, identify the conjugate acid-base pairs.
What is the pH (to nearest 0.01 pH unit) of a solution prepared by mixing 52.0 mL of 0.125 M HF and 78.0 mL of 0.0465 M NaOH
In standardizing an unknown NaOH solution, 21.50 mL of NaOH solution are found to reach the endpoint in a titration with 0.792 g of KHP. (MW= 204.32.0 g/mol) What is the molarity of the NaOH solution
Calculate the mass of nitrogen dissolved at room temperature in an 92.0L home aquarium. Assume a total pressure of 1.0 atm and a mole fraction for nitrogen of 0.78.
Calculate the pH of a solution that is formed when 25.0 mL of 0.24 M ammonia (Kb = 1.8 x 10-5) is mixed with 25.0 mL of 0.20 M ammonium chloride.
The variation of stress-concentration factor for a bar with fillet that is axially loaded shows that the kt approached infinity as the r/d ratio decrease.
Calculate the average absorbance and use this value for an absorbance point on your graph. Use the printed graph from above, find the average Absorbance of the unknown on the y-axis
A gaseous compound containing carbon and hydrogen was analyzed and found to consist of 83.65% carbon by mass. What is the empirical formula of this compound
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