<p>Hi. I have AP Chem hw due tomorrow…but I don’t understand how to do any of it!! T_T
It’s from the chapter about gases.<br>
Please help~ </p>
<li><p>An important process for the production of acrylonitrile (C3H3N) is given by the following reaction:
2C3H6(G) + 2NH3(G) + 3O2(G) → 2C3H3N(g) + 6H20(g)<br>
A 150.-L reactor is charged to the following partial pressures at 25’C:
P(C3H6)= .500MPa
P(NH3)=.800 MPa
P(O2)= 1.500 MPa
What mass of acrylonitrile can be produced from this mixture (MPa= 10^6 Pa)</p></li>
<li><p>A chemist weighed out 5.14 g of a mixture containing unknown amounts of BaO(s) and CaO(s) and placed the sample in a 1.50-L flask containng CO2(g) at 30.0’C and 750.torr. After the reaction to form BaCO3(s) and CaCO3(s) was completed, the pressure of CO2(g) remaining was 230. torr. Calculate the mass percentages of CaO(s) and BaO(s) in the mixture. </p></li>
<li><p>A mixture of chromium and zinc weighing the 0.362 g was reacted with an excess of hydrochloric acid. After all the metals in the mixture reacted, 225 mL of dry hydrogen gas was collected at 27’C and 750. torr. Determin the mass percent Zn in the metal sample. [Zince reacts with hydrochloric acid to produce zinc chlorid and hydrogen gas; chromium reacts with hydrochloric acid to produce chromium (III) chloride and hydrogen gas.]</p></li>
<li><p>Consider a sample of hydrocarbon (a compound consisting of only carbon and hydrogen) at 0.959 atm and 298 K. Upon combusting the netire sample in oxygen, you collect a mixture of gaseous carbon dioxide and water vapor at 1.51 atm and 375 K. This mixture has a density of 1.391 g/L and occupies a volume four times as large as that of the pure hydrocarbon. Determine the molecular formula of hte hydrocarbon. </p></li>
<li><p>You have an equimolar mixture of the gasses SO2 and O2, along with some He, in a container fitted with a pison. The denisty of this mixture at STP is 1.924 g/L. Assume ideal behavior and constant temperature and pressure.<br>
What is the mole fraction of He in the original mixure?
The SO2 and O2 react to completion to form SO3. What is the denisity of the gas mixture after the reaction is complete? </p></li>
<li><p>A steel cylinder contains 5.00 mol of graphite (pure carbon) and 5.00 mol of O2. The mixture is ignited and all the graphite reacts. Combustion produces a mixture of CO gas and CO2 gas. After the cylinder has cooled to its original temperature, it is found that the pressure of hte cylinder has increased by 17.0%. Calculate the mole fractions of CO, CO2, and O2 in the final gaseous mixture. </p></li>
<li><p>You have sealed, flexible balloon filled with argon gas. The atmospheric pressure is 1.00 atm and the temperature is 25’C. The air has a mole fraction of nitrogen of .790, the rest being oxygen.<br>
a. Explain why the balloon would float when heated. Make sure to discuss which factors change and which remain constant, and why this matters. Be complete.<br>
b. Above what temperature would you heat the balloon so that it would float? </p></li>
<li><p>You have a helium balloon at 1.00 atm and 25’C. You want to mnake a hot-air balloon with the same volume and same lift as the helium balloon. Assume air is 79% nitrogen, 21% oxygen by volume. THe “lift” of a balloon is given by the difference between the mass of air displaced by the balloon and the mass of gas inside balloon.<br>
a. Will the temperature in the hot-air ballloon have to be higher or lower than 25’C? Explain.<br>
b. Calculate the temperature of the air required for the hot-air balloon to provide the same lift as the helium balloon at 1.00 atm and 25’C. Assume atmostpheric conditions are 1.00 atm and 25’C. </p></li>
<li><p>We sate that the ideal gas law tends to hold best at low pressures and high temperatures. Show how the van der Waals equation simplifies to the ideal gas law under these conditions. </p></li>
<li><p>Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia gas (NH3). You have nitrogen and hydrogen gases in a 15.0-L container fitted with a movable piston (the piston allows the container volume to change so as to keep the pressure constant inside the container). Initially the partial pressure of each reactant gas is 1.00 atm. Assume the temperature is constant and that the reaction goes to completion.<br>
a. Calculate the partial pressure of ammonia in the container after the reaction has reached completion.<br>
b. Calculate the volume of the container after the reaction has reached completion.</p></li>
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