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Question- Hydrazine (N2H4) and dinitrogen tetroxide (N2O4) form a self-igniting mixture that has been used as a rocket propellant. The reaction products are N2 and H2O.
1. Write a balanced chemical equation for this reaction.
2. What is being oxidized, and what is being reduced?
3. Which substance serves as the reducing agent and which as the oxidizing agent?
Provide complete steps to solve the above question any help is appreciated
Calculate the amount of heat that must be absorbed by 10.0 g of ice at -20°C to convert it to liquid water at 60.0°C. Given: Specific heat (ice) = 2.1 J/g·°C Specific heat (water) = 4.18 J/g·°C ?Hfus = 6.0 kJ/mol A) 420 J B) 2,900 J C) 6,300 J D) ..
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A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature.
Question- The first step in industrial nitric acid production is the catalyzed oxidation of ammonia. Without a catalyst, a different reaction predominates
a compound has a specific rotation of -39.0. a solution of the compound 0.206 gml has an observed rotation of -7.17
Determine the standard enthalpy change of the following explosive reaction by using the apprpriate enthalpies of formation
What mass of sodium nitrite must be added to 350 mL of water to give a solution with a pH
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Give the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C8H18 with 4.00 moles of O2. 2 C8H18 + 25 O2 ? 16 CO2 + 18 H2O
Assume the first equivalence pont is around 13.30 ml,for an experiment. while carrying out the ph meter titration approximately at which volume will you
How many grams of dry NH4Cl need to be added to 1.50 L of a 0.500 M solution of ammonia, NH3,to prepare a buffer solution that has a pH of 8.79. Kb for ammonia is 1.8*10^-5.
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