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E85 fuel is a mixture of ethanol and gasoline. What is the mass in kilograms of E85 (d=0.758g/mL) in a 14.0 gallon tank?
The _______ of a titration occurs when the indicator changes color.
How many cubic centimeters of an ore containing only 0.22% gold (by mass) must be processed to obtain $100 worth of gold.
What is the concentration of the H 2 SO 4 if a chemist titrates 300.0 mL of Sodium Hydroxide NaOH with a 5.0 M solution of NaOH and needs only 3.4 mL of the base to reach the endpoint,?
At an altitude of 45.00 km, the average atmospheric temperature is essentially 0 degrees C. What is the average number of air molecules per cubic centimeter of air at this altitude?
The tabulated mass of Cl is 35.45 amu. The two dominant isotopes of naturally occurring Cl are 35Cl (34.97 amu) and 37Cl (36.97 amu).
water has a molar heat of vaporization =40.79 kJ/mol, determine how many grams of water could be vaporized by 0.806 kilo Joules heat? Express your answer in units of g
How many grams of water can be cooled from 36 degrees celsius to 23 degrees celsius by the evaporation of 53g of water.
Discuss how to find the molar mass of a compound, percent composition of the elements of a compound and how to determine the empirical and molecular formulas from percent composition.
Write the structure of the conjugate acid of this base while consider the base monosodium phosphate, Na (HO)2P( O)O also explain why an aqueous solution of monosodium phosphate would be ineffective for extracting benzoic acid? pKa of this conjugat..
15.0 moles of gas are in a 5.00L tank at 22.2°C. compute the difference in pressure between CH4 and an ideal gas under these circumstances. The van der Waals constants for CH4 are a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.
Determine the percent yield for the reaction and also find out at which point the total pressure = 188 torr.
A sample of gas is heated. During the heating process, the volume of the gas increases 1.7 times. If the initial temperature of the gas is 80°C, what is the final temperature of the gas.
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