(a)
Interpretation:
The number of kilograms of
Concept Introduction:
Thermodynamic stability and kinetic stability works hand in hand.
(b)
Interpretation:
The number of kilograms of
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
The number of kilograms of
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
The number of kilograms of
Concept Introduction:
Refer to part (a).
(e)
Interpretation:
The number of kilograms of
Concept Introduction:
Refer to part (a).
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OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)
- Propane, C3H8, is a hydrocarbon that is commonly used as a fuel. (a) Write a balanced equation for the complete combustion of propane gas. (b) Calculate the volume of air at 25 C and 1.00 atmosphere that is needed to completely combust 25.0 grams of propane. Assume that air is 21.0 percent O2 by volume. (Hint: we will see how to do this calculation in a later chapter on gasesfor now use the information that 1.00 L of air at 25 C and 1.00 atm contains 0.275 g of 2 per liter.) (c) The heat of combustion of propane is 2,219.2 kJ/mol. Calculate the heat of formation, Hf of propane given that Hf of H2O(l)=285.8 kJ/mol and Hf of CO2(g)=393.5 kJ/mol. (d) Assuming that all of the heat released in burning 25.0 grams of propane is transferred to 4.00 kilograms of water, calculate the increase in temperature of the water.arrow_forward19. The chemical equation for photosynthesis is _CO2 (g) + _H₂O (1)→ __C6H1206 (s) + (C6H12O6 is glucose, the simplest sugar) a. Balance the chemical equation above by filling in the blanks. b. According to onetreeplanted.org, the average tree (across all climates and sizes) removes 10 kg of carbon dioxide from the atmosphere every year. Based on this, what mass of glucose is produced annually by the average tree? O2 (g) c. Teak is a common species of tropical tree. The graph below shows the amount of CO₂ absorbed by teak forests in tons of CO₂ per hectare of forest per year, according to the climate region where the forests are found (dry = low rainfall, humid=high rainfall). Looking at your photosynthesis equation again, what does this data suggest about which reactant is the limiting reactant for teak trees? Explain. C Teak Carbon sequestration rate (tons CO₂ ha -1yr -1) 10 10 20 Tropical humid Tropical dry Aboveground biomass, 0-20 years Belowground biomass, 0 -20 yearsarrow_forward4. Methanol, CH;OH, can be produced by the following reaction: CO + 2He → CH;OH a) Hydrogen at STP flows into a reactor at a rate of 16.0 L/min. Carbon monoxide at STP flows into the reactor at a rate of 25.0 L/min. If 5.30 g of methanol is actually produced per minute, how much methanol may be produced theoretically? b) What is the proportion of actual to the theoretical yield, expressed as a percentage?arrow_forward
- The atmosphere slowly oxidizes hydrocarbons in a number of steps that eventually convert the hydrocarbon into carbon dioxide and water. The overall reaction of a number of such steps for methane gas is:CH4(g) + 5 O2(g) + 5 NO(g) ------> CO2(g) + H2O(g) + 5 NO2(g) + 2 OH(g) Suppose that an atmospheric chemist combines 155 mL of methane at STP, 885 mL of oxygen at STP, and 55.5 mL of NO at STP in a 2.0-L flask. The flask stands for several weeks at 275 K. If the reaction reaches 90.0% of completion (90.0% of the limiting reactant is consumed), what is the partial pressure of each of the reactants and products in the flask at 275 K? What is the total pressure in the flask?arrow_forwardYou are heating potassium perchlorate and collecting the oxygen gas from the decomposition over water. Write the equation here! 2 KClO3(s) ----------> 2KCl (s) + 3O2 (g) 2. Mass of sample: 0.398 g Ambient pressure: 752.3 mmHg Volume of gas: 81.4 mL Room temperature: 18.9 degrees Celsius 3. Using the mass of your KClO4 sample, and the balanced equation, calculate the theoretical yield of O2 gas in grams. 4. With vapor pressure of water versus temperature, find the vapor pressure of water at your temperature: Vapor pressure of water at given temperature:arrow_forwardChemistry written by hand.arrow_forward
- If gasoline produces only carbon dioxide and water when it burns completely, why is automobile exhaust a source of air pollution? List the pollutants formed and briefly describe their impact.arrow_forwardBalance this unbalanced equation by entering only whole numbers into the blank. If the molar coefficient is 1, enter "1" (do not leave it blank: CaHg + O2 → CO2 + H20arrow_forwardThe reaction between SO3 (g) and CO2 (g) is based on the chemical equation below. 2 SO3 (g) + CO2 (g) = CS2 (g) + 4 O2 (g) At 500 oC, we mix 0.20 mol SO3 (g) 0.25 mol CO2 (g) and 1.20 mol O2 (g) (without CS2 (g)) initially in a 1-L bottle. After the reaction reaches equilibrium, the amount of SO3 (g) becomes 0.12 mol. Determine the value of the equilibrium constant of the above reaction (with 2 significant figures).arrow_forward
- Previous Page 6 of 16 Next O References Use the References to access important values if need According to the following reaction, how many grams of oxygen gas are required for the complete reaction of 25.2 grams of ammonia? ammonia (g) + oxygen (g) nitrogen monoxide (g) + water (g) grams oxygen gas Cengage Learning | Cengage Technical Supportarrow_forwardAn industrial factory makes an effort to reduce the amount of nitrogen dioxide (NO2) emissions it releases into the atmosphere on a weekly basis. Which statement de- scribes the most likely reason for this effort by the industrial factory? A The factory wants to decrease the amount of tropospheric ozone 3) that is formed when nitrogen dioxide N2) emissions react with sulfur dioxide 02). B. The factory wants to decrease the amount of stratospheric ozone 3/ that is (NO) formed when nitrogen dioxide emissions mix with fog. The factory wants to decrease the amount of gray smog that is formed when nitro- gen dioxide N2) emissions mix with fog. The factory wants to decrease the amount of photochemical smog that is formed when nitrogen dioxide 2) emissions react with VOCS and mix with fog.arrow_forwardDetonation of nitroglycerin proceeds as follows:4 C3H5N3O9(l)------>12 CO2(g) + 6 N2(g) + O2(g) + 10 H2O(g)(a) If a sample containing 2.00 mL of nitroglycerin (density =1.592 g/mL) is detonated, how many moles of gas are produced?(b) If each mole of gas occupies 55 L under the conditionsof the explosion, how many liters of gas are produced?(c) How many grams of N2 are produced in the detonation?arrow_forward
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