Write a balanced equation that describes each of the following chemical reaction. 1. Acetylene gas, C2H2, burns in air forming gaseous carbon dioxide and, CO2, and water. Answer: 2C2H2 + 502 → 4CO2 + 2H20 (double displacement/Combustion reaction) 2. Acid rain, a solution of sulfurous acid, H&PO4(aq), forms when sulfur dioxide reacts, SO2, reacts with water. 3. Water vapor reacts with sodium metal to produce gaseous hydrogen, H2, and solid sodium hydroxide, NaOH. 4. Gaseous water and hot carbon react to form gaseous hydrogen, H2, gaseous carbon dioxide. 5. Ca3(PO4)2 + H3PO4 → Ca(H2PO.)2 6. Ag + H2S + O2 Ag2S + H2O nglish (United States) O Accessibility Good to go

Write a balanced equation that describes each of the following chemical reaction. 1. Acetylene gas, C2H2, burns in air forming gaseous carbon dioxide and, CO2, and water. Answer: 2C2H2 + 502 → 4CO2 + 2H20 (double displacement/Combustion reaction) 2. Acid rain, a solution of sulfurous acid, H&PO4(aq), forms when sulfur dioxide reacts, SO2, reacts with water. 3. Water vapor reacts with sodium metal to produce gaseous hydrogen, H2, and solid sodium hydroxide, NaOH. 4. Gaseous water and hot carbon react to form gaseous hydrogen, H2, gaseous carbon dioxide. 5. Ca3(PO4)2 + H3PO4 → Ca(H2PO.)2 6. Ag + H2S + O2 Ag2S + H2O nglish (United States) O Accessibility Good to go

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter8: Gases

Section: Chapter Questions

Problem 155CP: Methane (CH4) gas flows into a combustion chamber at a rate of 200. L/min at 1.50 atm and ambient...

See similar textbooks

Similar questions

Methane (CH4) gas flows into a combustion chamber at a rate of 200. L/min at 1.50 atm and ambient temperature. Air is added to the chamber at 1.00 atm and the same temperature, and the gases are ignited. a. To ensure complete combustion of CH4 to CO2(g) and H2O(g), three times as much oxygen as is necessary is reacted. Assuming air is 21 mole percent O2 and 79 mole percent N2, calculate the flow rate of air necessary to deliver the required amount of oxygen. b. Under the conditions in part a, combustion of methane was not complete as a mixture of CO2(g) and CO(g) was produced. It was determined that 95.0% of the carbon in the exhaust gas was present in CO2. The remainder was present as carbon in CO. Calculate the composition of the exhaust gas in terms of mole fraction of CO, CO2, O2, N2, and H2O. Assume CH4 is completely reacted and N2 is unreacted.
Consider the reaction between 50.0 mL liquid methanol, CH3OH (density = 0.850 g/mL), and 22.8 L O2 at 27C and a pressure of 2.00 atm. The products of the reaction are CO2(g) and H2O(g). Calculate the number of moles of H2O formed if the reaction goes to completion.
One of the many remarkable enzymes in the human bodyis carbonic anhydrase, which catalyzes the interconversionof carbon dioxide and water with bicarbonate ionand protons. If it were not for this enzyme, the body couldnot rid itself rapidly enough of the CO2 accumulated bycell metabolism. The enzyme catalyzes the dehydration(release to air) of up to 107 CO2 molecules per second.Which components of this description correspond to theterms enzyme, substrate, and turnover number?
1)Please express the normal salt (NaCl) concentration in body fluid into molarity (mM).2) Commercial fuming Sulphuric acid (Oleum-H2S2O6) is 99.9%. solution. Please convert it into molarity.3) Find out the Volume (dm3) of product (gas) at RTP when 0.58 M, 150 mL NaOH (aq.) reacts with 350 mL, 0.25 NH4Cl.4) The above reaction has the product Ammonia, which when dissolved in 650 mL ethanol makes an alkaline ethanolic solution. Find its molarity (M) 5) Calculate the adult dose as per the BW of the baby. (Child dose-50 mg and the BW of the baby is 48 lb (British pound) (1lb=0.453 Kg)
Combustible vapor-air mixtures are flammable over a limitedrange of concentrations. The minimum volume % of vapor thatgives a combustible mixture is called the lower flammable limit(LFL). Generally, the LFL is about half the stoichiometric mix-ture, the concentration required for complete combustion of thevapor in air. (a) If oxygen is 20.9 vol % of air, estimate the LFL forn-hexane, C₆H₁₄. (b) What volume (in mL) of n-hexane (d=0.660 g/cm³) is required to produce a flammable mixture of hexane in 1.000 m³of air at STP?
Ideal Gas Law: Temperature, Volume & Pressure Given: Temperature of H2O = 200C Pressure = 0.95 atm Initial Air Volume = 50mL Final Air Volume = 95mL Volume of O2 collected = 95mL - 50mL = 45mL Total Reaction time = 17mins Balanced equation for hydrogen peroxide decomposition: 2H2O2 ------ 2H2 + O2 Using the Ideal Gas Law (PV = nRT), calculate the grams of O2 produced in the reaction above(decomposition of hydrogen peroxide). (Hint: solve for n, and then convert moles of O2 to grams. Watch your units; you may need to convert some of your data into different units.)
A political candidate fighting for a smoke-free environment conducts an experiment in a room containing 1400 cubic feet of air that is initially free of carbon monoxide. Beginning at time t=0, cigarette smoke containing 4% carbon monoxide is introduced into the room at the rate of 0.1 cubic foot perminute, and the well-circulated mixture is allowed to leave the room at the same rate. If carbon monoxide levels in the air reach 0.012%, it is harmful to the human body. Find the time at which this unhealthy level is reached.
In 2014, the World Anti-Doping Agency announced that Xenon gas would be added to the list of banned substances for athletes. Apparently since 2004, Russian athletes had been inhaling xenon while training, with the physiological effect being to boost the capacity of blood to carry oxygen needs for aerobically demanding sports. If an athlete inhaled an average of 1.75 x 10-4 moles of Xe per breath while sleeping, with an average rate of 13.0 breaths per minute for 8.50 hours how many total GRAMS of Xe(g) were inhaled while sleeping? please show all calculations
In Beirut, Lebanon, a storage warehouse with 2750 tonnes of ammonium nitrate exploded damaging the city and killing at least 78 people in August 2020. Pure ammonium nitrate does not explode easily and can be handled safely. It decomposes at 230oC producing nitrous oxide gas (N2O) and water vapor. Give a balanced equation for the decomposition reaction. Above 260oC, if confined and when contaminated, ammonium nitrate will explode forming toxic gases such as NO2, responsible for the ‘orange brown fireball’ that occurred in the explosion. The following equation represents one of the reactions contributing to the explosion: 4NH4NO3(s) → 3N2(g) + 2NO2(g) + 8H2O(g) + 405.6 KJ/mol picture Identify the reaction diagram that shows the reaction above. Make sure to explain why you chose A or B using the concepts of energy of reactants and products.
Here is the overall reaction in an automobile airbag:20NaN3 (s) + 6SiO2 (s) + 4KNO3 (s) -----> 32N2 (g) + 5Na4SiO4 (s) + K4SiO4 (s) Calculate how many grams of sodium azide (NaN3) are needed to inflate a 30.0 × 30.0 × 20.0 cm bag to a pressure of 1.20 atm at a temperature of 20.0°C?
UCI Chemistry researchers, Prof. F. Sherwood Rowland and Dr. Mario Molina werefirst to discovered in 1973 that chlorofluorocarbons (CFCs) were depleting the Earth’sozone layer when released into the atmosphere. Once they reach the stratosphere, Clis released from the CFCs molecules by interaction with UV light. Free Cl atoms areable to react with ozone in a catalytic cycle that converts O3into the more stable O2.It is estimated that a single Cl atom is able to react with∼100000 O3molecules.Although CFCs production was banned in 1996, there are still a substantial numberof motor vehicle air conditioners (MVACs) that use CFC-12 (CF2Cl2) as refrigerant.The average CFC-12 emission rate from operating MVACs has been estimated tobe 59.5 mg per hour per vehicle (Zhang et al.Environ. Sci. Technol. Lett.2017).How much chlorine, in kg, is added to the atmosphere in a year due to 100 millionMVACs using CFC-12 as refrigerant?
Butane C4H10 is burned with 16% excess air. An analysis of the combustion gases revealed that all hydrogen in the fuel burns to H20 but only 88.9% of the burns to CO2 with the remaining C forming Co. What is the volumetric fraction in % of the of CO2 in the products?