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- 93.6g to ng and 93.6g to tons with the set up in the image possible show how to get the answer pleasehow to calculate moles of NaHCO3 and moles of CO2 from Mass of NaHCO3= 0.081g Volume of CO2=5ml show steps 10minsGiven Active Ingredient: precipitated sulfur (ointment) Raw Materials: 500 g calcium polysulphide and 1.5 kg hydrochloric acid Actual Yield: 343.4g precipitated sulfur Formulation: 250 mg per jar Dosage form: Ointment packaging:100 jars per box Synthesis and Packaging (Need answer)- Balanced Chemical Equation:- % composition by mass of each compound:- Mass to Mass Stoichiometry Calculation:- Limiting Reagent:- Excess Reagent:- Amount (g) in excess: % Yield:- Number of dosage form and packaging that can be produced from stoichiometric solution:
- A mass of KHP is measured at 0.3051g and contains ______ moles. Group of answer choicesFor the reaction C4H10 + O2 --> CO2 + H2O a) what weight of C4H10 in grams is needed for 3.01 x 10E23 particles of O2? b) how many moles of CO2 will be produced from 5.0 moles of C4H10? c) what weight in grams of H2O will be produced from 12.5 ml of C4H10? density (p)?of C4H10 = 0.506 g/mLThe manufacture of aluminium includes the production of cryolite (Na3AlF) from the following reaction 6HF (g) + 3NaAlO2 (s) - > Na3AlF6 (s) + 3H2O (l) + Al2O3 (s) How much HF (hydrogen sulfide) is required to produce 2.50kg of Na3AlF6 Provide your answer/work in dimensional analysis format
- A sample of an industrial waste water is analyzed and found to contain 16.5ppb Fe2+. How many grams of iron could be recovered from 1.81×103 kg of this waste water? Answer:_______ grams FeFor the following table fill in the missing values and calculate the theoretical yield. A + 2B à C moles 0.00242 0.00242 ?_________ MW ?_________ 98.06 164.16 g ?_________ ?__0.00002467_______ ?_________ mL 0.20 d(g/mL) 0.80I have 2 questions regarding this example in the first underlined fraction why is NO not squared ? And the second is can you explain the second underlined green line how can I get this equation can you show me the workout for it Thank you
- Stock iron(II) solution (200Ug mL-1 Fe) ferrous ammonium sulfate hexahydrate mass= 0.1437g, transfer it to a 100 ml beaker. add 15 ml approx of water and 15m1 'approx of dilute sulphuric acid (2M H2SO.). then transfer FeII to 100 ml flask makeup to the mark with water. calculate the moles of ferrous ammonium sulfate hexahydrate solution in unit ug/mL.John and Eli do a reaction with the goal to prove the law os conservation of mass. In the reaction, they place 50.00 g of acetic acid (CH3COOH) in a clean, dry ziploc bag and then add 5.00 g of baking soda (NaHCO3). The products of the reaction include sodium acetate, carbon dioxide, and water. In trial 1, Eli immediately seals the bag upon addition of the baking soda and waits until the bubbling comes to a halt. John weighs the closed bag with all contents and records mass in the table. For trial 2, John and Eli repeat the procedure but forgot to seal the bag. Their results are shown in the table below. 1. Calculate the theoretical mass of the open bag. 2. Are atoms/mass conserved in each of the reactions? 3. Provide mathematical evidence to explain your reasoning that atoms/mass are/are not conserved.How many g of ZnS is needed to react completely with 37.72 gram O2 according to this equation?2ZnS + 3O2 --> 2ZnO + 2SO2 Put answer in box in regular , non-scientific, notation with 2 places past the decimal