A mixture of 6.00 g hydrogen (H2. molecular weight 2.016 g/mol) and 35.0 g oxygen (O2, molecular weight 31.998 g/mol) is prepared in an explosion-proof container, and allowed to react forming liquid water (H2O, 18.016 g/mol). 2 H2(g) + O2(g) ---> 2 H2O(l) This explosive reaction is known to have a nearly 100% yield, so it proceeds until all limiting reagent is used up. Please select the correct amount at the end of the reaction.

2+ Natural waters often contain relatively high levels of calcium ion, Ca²+, and hydrogen carbonate ion (bicarbonate), HCO3¯, from the leaching of minerals into the water. When such water is used commercially or in the home, heating of the water leads to the formation of solid calcium carbonate, CaCO3, which forms a deposit ("scale") on the interior of boilers, pipes, and other plumbing fixtures. Ca(HCO3)2 (aq) → CaCO3 (s) + CO2(g) + H₂O(1) If a sample of well water contains 0.0016 mg of Ca(HCO3)2 per milliliter, what mass of CaCO3 scale would 1.0 mL of this water be capable of depositing? Mass= g

(4) for the reaction : 2 NaHCO3 → Na₂CO₂ + H₂O + CO₂ Find the mass of Sodium Carbmate that reacted from 1.56g of heated Sodium Hydrogen Carbonate

Assuming you started with 3.23 g of sodium bicarbonate and your actual yield of solid product is 1.20g, which reaction is more likely to be the correct one?

Arsine, AsH3, was once a product of a test used in forensic analysis. Tissues from a possible poisoning victim were treated with zinc and sulfuric acid. If arsenic was present (usually as diarsenic trioxide, As203), arsine would form: As₂03 (s) + 6 Zn(s) + 6 H₂SO4(aq) ----> 2 AsH3(g) + 6 ZnSO4(aq) + 3 H₂O(1) a) In a lab exercise, a forensic technician reacts 19.8 g of AS₂O3 with 32.7 g of Zinc in the presence of excess sulfuric acid. What mass of AsH3 will be produced? b) Use the same chemical reaction, create a question which needs to be solved by percentage yield.

Aspirin can be synthesized in the lab by combining salicylic acid (C,H,O,) and acetic anhydride (C,H,0,) to form aspirin ( C,H,O,) and acetic acid (C, H,0,). The balanced equation for this reaction is C,H,O, + C,H,O, C,H;O4 + C,H,O, A student started with 4.15 mL acetic anhydride (density 1.08 g/mL) and 1.59 g salicylic acid. The student synthesized 1.68 g of aspirin. Select the limiting reactant. acetic acid (C,H,02) aspirin (C, H,O4) acetic anhydride (C¸H,O3) salicylic acid (C,H,O;) Calculate the theoretical yield of aspirin (C,H3O4). theoretical yield: g Calculate the percent yield for aspirin (C,H,O,). percent yield:

#25y of a 23% by mass magnesium chloride (MW= 95.21 g/mole) solution is reacted with 125.0 mL da125M solution of silver nitrate (MW= 169.87g/mole) determine the mass of silver chloride (MW = 143.32 p/mole) produced

In the reaction 2NH3 + CO2 - -- > CO(NH2)2 + H2O, 8 moles of NH3 react with 8 moles of CO2, the obtained amount of CO(NH2)2 in moles will be: O 10 8. O 4 O 2

Aspirin can be synthesized in the lab by combining salicylic acid (C,H,0,) and acetic anhydride (C,H,0,) to form aspirin ( C,H,O.) and acetic acid (C,H,O,). The balanced equation for this reaction is C,H,0, + C,H,O, → C,H,0, + C,H¸0, A student started with 3.33 mL acetic anhydride (density = 1.08 g/mL) and 2.61 g salicylic acid. The student synthesized 2.53 g of aspirin. Select the limiting reactant. salicylic acid (C,H,O,) acetic anhydride (C,H,0,) aspirin (C, H,O,) acetic acid (C,H0,) Calculate the theoretical yield of aspirin (C,H, O,). theoretical yield: uloto the percent yield for aspirin (C, H, O).

Assuming you started with 3.23 g of sodium bicarbonate and your actual yield of solid product is 1.20g, which reaction is more likely to be the correct one?