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A substance has a molar mass of 60 g/mol with 40.0 percent carbon, 6.7 percent hydrogen, and 53.3 percent oxygen. What is its empirical formula?
Every measurement has a measurement uncertainty. Discuss how precise and accurate measurement can be achieved in spite of the inherent measurement uncertainty.
Complete the following equations in molecular form. The reactant coefficients are correct. Indicate precipitation, redox, or acid – base. Write the equations in NET ionic form (no spectator s). Balance charges and use the correct suffixes.
At a particular temperature, K = 3.75 for the following reaction. SO2(g) + NO2(g) SO3(g) + NO(g)
A steel tank with a volume of 9.583 L contains N2 gas under a pressure of 4.972 atm at 31.8 °C. Calculate the number of moles of N2 in the tank.
if you burn 1.5 mol C3H8 according to the following reaction C3H8 +5O2 = 3CO2 + 4H2O how many grams of carbon dioxide are produced.
A 0.894-g sample of gas occupies 125 mL at 60. cm of Hg and 25C. What is the molar mass of the gas.
Ethanol is a common laboratory solvent and has a density of 0.789 g/mL. What is the mass, in grams, of 143 mL of ethanol.
Draw the accepted mechanism for each reaction and illustrate how each stereoisomer is formed in the reaction.
Determine what is the percent yield of the reaction If 15.0 grams of Nitrogen and 2.00 grams Hydrogen react to produce 1.38 grams of Ammonia?
Constant external pressure of3.00 atm, followed by2) against a constant external pressure of 2.00 atm. Calculate q and w. (101.33 J = 1 L atm)
A 1.43-L flask is filled with propane gas (C3H8), at 1.00 atm and -23.0°C. What is the mass of the propane in the flask?
A 2.30 L sample of O2(g) was collected over a liquid at a total pressure of 785 torr and 25°C. When the O2(g) was dried (vapor of that liquid removed), the gas had a volume of 1.86 L at 25°C and 785 torr.
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