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- The following information was recorded by a student team working to prepare nickel sulfate. Plan: Prepare NiSO4 by reacting NiO with 6 M H2SO4 The expected product is NiSO4·6H2O. We will filter the crystals from the reaction solution to get the product. NiO + H2SO4 --> NiSO4 + H2O molar mass of NiO: 74.69 g/molmolar mass of NiSO4: 154.75 g/mol molar mass of NiSO4·6H2O: 262.85 g/mol mass of NiO used: 7.5 gvolume of 6M H2SO4 used: 50 mL heated the solution for 30 minutes, cool and filtered the crystals mass of product: 17.4 g Two students calculated percent yield using this data. One student got 66.2% and another got 112%. Based on this information, which of the following statements are true. One or more statements are correct. Group of answer choices The percent yield of 112% was calculated using the molar mass for the hydrated product. The percent yield of 66.2% was calculated using the molar mass for the anhydrous product. Both percent yields are incorrect because…If the atmospheric burden of CO2 increases by 27.0 Gt (gigatonnes, 1Gt= 1 x 1012kg) over a given period of time, starting now, and the current atmospheric CO2 is 408.3 ppm, what will the concentration of CO2 be (in ppm) after this increase? (Assume a total atmospheric mass of 5.10 x 1021 g and an average molar mass for air of 29.0 g/mol) 411.8 ppm 408.8 ppm 410.6 ppm 417.0 ppmConstants Periodic Table Consider the following reaction: If the initial volume of the H2O2 solution is 3.2 L, what total amount of O2 (in moles) is formed in the first 20 s of reaction? Hint: Use Figure 1 to answer this problem. H2O2(aq) H20() + ½ O2(g) and the kinetics plots below to answer the questions to the right. Express your answer in moles to two significant figures. O 1.4 mol Figure 1. Plot of [H,O,] vs time O .8 mol 0.9 0.63 mol 0.8 0.7 O 0.70 mol 0.6 0.5 0.4 Submit Request Answer 0.3 0.2 0.1 Part B 20 40 60 80 time (s) concentration of H;O2 (mol L²)
- 16. The combustion of gasoline (octane) in a car engine can be represented by the following equation: 2C3H18(1) + 2502(g) a. What mass of oxygen is used up to burn a full tank of 36.00 kg of gasoline? Text --> 16CO2(g) +18H20(g) b. Why might a vehicle that is calibrated to run perfectly at sea level run poorly at higher elevations? Text Тext According to the Canadian Automobile Association, the average Canadian drives 20,000 km/yr. C. Assuming that distance, how many more kg of carbon dioxide are added to the atmosphere each year by a Toyota Tacoma (fuel economy of 12.8 L/100 km) than a Toyota Prius (4.52 L/100 km)? The density of gasoline is 0.719 kg/L.Nitric oxide reacts with hydrogen to release large amounts of chemiluminescence with the characteristics of the highly cytotoxic species. The following data were measured for the reaction of nitric oxide with hydrogen: Data number 1 2 3 2 NO(g) + 2 H₂(g) → N₂(g) + 2 H₂O(g) [NO] (M) 0.1 0.1 0.2 [H₂] (M) 0.1 0.2 0.1 Based on the data, (a) Determine the rate law for this reaction. (b) Calculate the rate constant. (c) Calculate the rate when [NO] = 0.050 M and [H₂] = 0.150 M Initial rate (M/S) 1.23 x 10-³ 2.46 x 10-³ 4.92 x 10-³The density of moist air (ideal gas mixture) at 20°C temperature and 700 mmHg pressure was found to be 1.1 g/lt. Calculate the partial pressure of water vapor in this air. Additional data: MA(H2O)18, MA (Air)29
- What is An for the gases in the following reaction: C4H100(l) + O2(g) →_CO₂(g)_H₂O(1) Type your numeric answer and submitIRS whistleblowers testify at Hou: XM $4 off on Delicious, Rejuvenating X A ALEKS-Andrew Herrera - Learn X ← → C www-awa.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-lvgXwPgmUhvlTCeeBZbufuBYTi0Hz7m7D3ZcZsVtNxxGh3NolGhgexjUoyas3VCHOBjufyala7Wgbxc... ☆ = @ 89°F Near record Fill in the information missing from this table: 4- ELECTRONIC STRUCTURE AND CHEMICAL BONDING Calculating the capacity of electron subshells subshell 3s 5s Explanation 4p 2 Some electron subshells principal quantum number n 0 0 0 Check }° с angular momentum quantum number / ▬▬ 0 0 0 Q Search FO maximum number of electrons 0 П 10 F7 F8 8 F9 X 3 en F10 *- OF ** PrtSc W 0/3 Insert © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility @dx a Delete Andrew ^ 0 olo Ar O X ⠀ 4:45 PM 7/20/2023Anna was asked to identify and explain if the equation CO2 (g) → CO2 (I) was an endothermic or exothermic reaction. However she got it wrong. What is her error and what should the answer have been? Anna's statement: The equation is an endothermic reaction because the energy is released from gaseous CO2 to the surroundings to become liquidCO2 causing the molecules to speed up. Format В I U B ... >
- As a concerned individual, this calls for an act to mitigate the problem on oceanacidification caused by anthropogenic emissions of CO2. In consideration to this perennialchallenge, we are left to answer a very important question: What can we do to help solve thisproblem? Your answer should consist at most five (5) sentences.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?10. Hydrogen peroxide, H.O2, will spontaneously disproportionate into molecular oxygen and water according to the following reaction: 2H.O. - 2H,O. + 0. 5.00 mL sample of 3.0% aqueous hydrogen peroxide is placed in a test tube and reacted according to the above reaction; the oxygen gas is collected over water at 28 °C. a) Assuming the density of the hydrogen peroxide solution is 1.00 g/mlL., what is the mass of hydrogen peroxide in the sample? b) Given the vapor pressure of water at 28 °C is 28.3 torr, what is the volume of oxygen gas isolated from the above reaction if the total pressure is 755.2 torr?