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N2O4+ 2 N2H4= 3 N2 + 4 H2O, Determine the limiting reactant and the mass in grams of nitrogen that can be formed from 50.0g N2O4 and 45.0g N2H4. The molar masses are as follows: N2O4=92.02g/mol, N2H4=32.05g/mol.
The reaction is between furan and maleic anhydride. Using 0.19 g of furan and 0.24 g of maleic anhydride.
A mixture of 0.100 mol of CO2, 0.050 mol of H2, and 0.100 mol of H2O is placed in a 1.00 L vessel and reacts according to the reaction shown below.
A sample of gas is compressed from 13.01 L to 4.27 L using a constant external pressure of 3.63 atm. At the same time, 1,453 J of heat flows into the surroundings. What is the internal energy change for the gas
Important information about pH and Molarity, You add 5 drops of .100 M HCl to 100ml of "pure" water. Assuming that the volume of one drop is .035ml, calculate the expected pH of the resulting solution
A 0.750 g of lye is dissolved in water and titrated with 32.0 mL of 0.500 M HCl. What is the percent purity of the lye sample
A Freon leak in the air-conditioning system of a large building releases 20kg of CHF2CL per month. If the leak were allowed to continue, how many kilograms of Cl would be emitted into the atmosphere each year
What is the molarity of C6H12O6 in an aqueous solution that is prepared by dissolving a 20.95 g sample of impure C6H12O6 in water to make 1,450 mL of solution.
A plot of ln[AV] versus t (s) gives a straight line with a slope of -0.32s^-1. What is the value of the rate constant (k) for this reaction?
What is the balanced chemical equation for its reaction with nitric acid? Write the balanced chemical equation for its reaction with a potassium hydroxide.
What is the percent by mass of oxygen in a gaseous mixture whose molar composition is 0.500% CO2 and 99.500% air?
Use the systematic treatment of equilibrium to determine the pH and concentrations of species in 1.00 L of solution contatining 0.070 lysine HL 0.055 mol aspartic acid H2A and 0.0080 mol NaOH. Consider just acid base chemistry. Ignore ion pairing ..
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)--> 2Fe(s)+3Mg2+(aq+ Calculate the cell potential at 25 under each of the following conditions.
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