Pentaerythritol tetranitrate (abbreviated PETN, chemical formula C5H8N4O12) is an explosive material with a structure that is very similar to nitroglycerin. It is one of the components of plastic explosives such as Semtex. The explosion of PETN can be represented by: C5H8N4O12(s)→2CO(g)+4H2O(g)+3CO2(g)+2N2(g) A plastic explosive charge is formed into a cylinder about 30 cm long and about 2 cm in diameter. It weighs about 246 grams and is 58.5% PETN by mass. What is the total number of moles of gas produced when this plastic explosive charge explodes?  mol gas Sulfuric acid (H2SO4) reacts with sodium bicarbonate (NaHCO3) to produce sodium sulfate, carbon dioxide and water. If 1.45 L of 4.50 M H2SO4 is spilled and 1.00 kg NaHCO3 (MM=84.01 g/mol) is available to clean up the spill, is there enough sodium bicarbonate to neutralize the spilled sulfuric acid? No, and there is about 10% less NaHCO3than needed. Yes, and there is about 10% more NaHCO3than needed. No, and there is about 20% less NaHCO3than needed. Yes, and there is precisely enough NaHCO3. Yes, and there is about 20% more NaHCO3than needed.

7.312 g of dry ice (solid carbon dioxide) is placed in a sealed 2.000 L bag in a room where the pressure is 0.9140 atm. The carbon dioxide sublimes into a gas, and the bag expands to 12.116 L. If the enthalpy of sublimation for CO, is 25.9 kJ/mol, what is the total energy change of the system in kilojoules?

The total volume of hydrogen gas needed to fill the Hindenburg was 2.0 x 108 L at 1.0 atm and 25°C. Given that  ΔH°f for H2O(I) is -286 kJ/mol, how much heat was evolved when the Hindenburg exploded, assuming all of the hydrogen reacted to form water?

When heated calcium carbonate decomposes according to the equation below. CaCO3(s) → CO2(g) + CaO (s) In a study of the decomposition of calcium carbonate, a student added a 25.0 g sample of powdered CaCO3(s) into a rigid 2.0 L container. The student sealed the container, pumped out all the gases, then heated the container in an oven at 1100 K. As the container was heated, the total pressure of the CO2in the container was measured over time. The data are plotted in the graph below.   The student repeated the experiment but this time the student used a 50 g sample of powdered CaCO3(s). In this experiment, the final pressure in the container was 1.04 atm, which is the same final pressure as in the first experiment. f. The student claimed the final pressure in the container and each experiment became constant because all of the CaCO3 had decomposed. Based on the data in the experiments do you agree with this claim? Explain.

Based on the nature of reactants and products, which of the following processes would you expect to be exothermic? (You can select more than one). 2SO3 → 2S +30₂ N₂ + 3H₂ → 2NH₂ CO₂ → C+0₂ 2 NO ₂ → N₂O4 2

Please answer question 9 part A

A student dissolves 14.0 g of ammonium nitrate (NH4NO3) in 200. g of water in a well-insulated open cup. He then observes the temperature of the water fall from 22.0 °C to 16.6 °C over the course of 5.5 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH4NO₂ (s) NH(aq) + NO3(aq) - You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy AHxn per mole…

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The pressure of a gas is measured as 60. torr. Represent this pressure in atmospheres. (1 atm = 760 torr) Show work.

1a) Ea is 14.0 kJ/mol, for the uncatalyzed reaction: O3(g) + NO(g)-->  NO2(g) + O2(g) Slow NO2(g) + O(g)-->  NO(g) + O2(g) Fast   (uncatalyzed reaction) Overall reaction: O3(g) + O(g)-->  2O2(g) Ea for the same reaction, when catalyzed as above, is 11.9 kJ/mol.At -37°C, what is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction?(Assume the frequency factor A is the same for each reaction.)  1b) One of the concerns about the use of freons is that they will migrate to the upper atmosphere, where chlorine atoms can be generated by the reaction CCl2F2 --> CF2Cl + Cl (photolysis of Freon-12) Chlorine atoms can also act as a catalyst for the destruction of ozone.The activation energy for the reaction Cl + O3 --> ClO + O2 is 2.1 kJ/mol. Cl is regenerated by the fast reaction ClO + O --> O2 + Cl If the frequency factors are the same and both catalysts are in equal concentration, how many times faster,…