lhe energy used to power one of the Apollo lunar missions was supplied by the following overall reaction: 2N2H4 + (CH3)2N2H2 + 3N204.-> 6N2 + 2C02 +81-120. For the phase of the mission when the lunar module ascended from the surface of the moon, a total of 1200. kg N2H4 was avail-able to react with 1000. kg (CH3)2N2H2 and 4500. kg N204. a. For this portion of the flight, which of the allocated components was used up first? b. How much water, in kilograms, was put into the lunar atmosphere through this reaction?

Explanation is in the file

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answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.

frequency, z, and the collision density, z, in carbon dioxide (co2), r 180 pm at 30 °c and 120 kpa