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. g. After 20 minutes some CO2, was injected into the container and initially raising the pressure to 1.5 atm. Would the final pressure inside the container be less than, greater than, or equal to 1.04 atm? Explain.

A NASA spacecraft measures the rate R of at which atmospheric pressure on Mars decreases with altitude. The result at a certain altitude is: - 1 R=0.0296 kPa·km -4 Convert r to j·cm ala 4 J•cm x10 18 Ar

The decomposition of NI3 to form N2 and I2 releases −290.0 kJ of energy. The reaction can be represented as 2NI3(s)→N2(g)+3I2(g), ΔHrxn=−290.0 kJ   Find the change in enthaply when 11.0 g of NI3 decomposes.

Ethylene (C2H4) plays an important role in the ripening of certain fruits and vegetables. It is sometimes supplemented under controlled conditions at produce—processing facilities but is also produced naturally by many fruit-bearing plants.  Although the actual process by which plants produce ethylene is a complex one, imagine that it is produced by the simple breakdown of glucose according to the equation: C6H12O6 (s)  à 3 C2H4 (g) + 3 O2 (g)   Given S°= 212.1 J/molK, DG°= -910.56 kJ/mol and DH°= -1274.5 kJ/mol for C6H12O6 (s).   a.) Determine the sign of DS° for the reaction. b.) Calculate DS° for the reaction. c.) Using the tabulated DG° values in the appendix, calculate DG° for the reaction. d.) Above what temperature (in °C) is the reaction spontaneous? Hint: you will first have to calculate DH° using tabulated values.

When potassium chloride reacts with oxygen under the right conditions, potassium chlorate is formed: 2 KCl +3 02 → 2 KC103 39 kJ/mol 78 kJ/mol O O-78 kJ/mol -39 kJ/mol G

#15

On a 14.6 oz bag of candy, the manufacturer states that a single 2.00 oz serving is equivalent to 200. kJ. How many Calories are in the bag of candy?

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A student makes the following statement: The energy required to break the bonds in the reactants is less than the energy released in the formation of the bonds of the products. Do you agree or disagree with this statement?

A student dissolves 13.8 g of ammonium chloride (NH4Cl) in 250. g of water in a well-insulated open cup. She then observes the temperature of the water from 21.0 °C to 17.3 °C over the course of 6.3 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH₂Cl(s) → NH(aq) + Cl¯ (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 t 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 AH per mole of NH Cl.…