Unknown elemental metal was reacted with Hydrochloric Acid. It was determined that this reaction evolved Hydrogen gas and left the metal in solution in the 2+ oxidation state. The Unknown metal was then subjected to the same test as Magnesium in the “Molar Mass of Magnesium” lab. After some adjustments to get the volume of gas collected in the right range, the following results were obtained:     Mass of Metal used = 0.3682 g   P (atmospheric) = 761.1 mm Hg

MISSED THIS? Watch KCV: Reactions in Solutions; Read Section 5.8. You can click on the Review link to access the section in your e Text. Complete and balance each of the following equations for gas-evolution reactions. Part A HNO3(aq) + Na₂SO3(aq) → Express your answer as a chemical equation. Identify all of the phases in your answer. = | ΑΣΦ A chemical reaction does not occur for this question. Submit Part B HCl(aq) + KHCO3(aq) → Express your answer as a chemical equation. Identify all of the phases in your answer. D= | ΑΣΦ Request Answer Submit Part C A chemical reaction does not occur for this question. Request Answer ? ="= | ΑΣΦ Part D HC₂H3O2 (aq) + NaHSO3(aq) → Express your answer as a chemical equation. Identify all of the phases in your answer. ? A chemical reaction does not occur for this question. Submit Request Answer ΑΣΦ ? (NH4)2SO4 (aq) + Sr(OH)2 (aq) → Express your answer as a chemical equation. Identify all of the phases in your answer. Submit Request Answer ? A chemical…

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Calculate the percentage of MnO2 in a mineral specimen  if the I2 liberated by a 0.1267-g sample in the net  reaction MnO2(s) + 4H+ + 2I- → Mn2+ + I2 + 2H2O  required 29.62 mL of 0.08041 M Na2S2O3.

6. Under suitable conditions, thiourea, CS(NH2)2, is oxidized to sulfate by solutions of potassium bromate: 3CS(NH2)2 + 4BrO3 + 3H20 → 3C0(NH2)2 + 3502 + 4Br + 6H+ A 0.0725 g sample of a material was found to consume 14.20 mL of 0.008340 M KBrO3. What was the percent purity of the thiourea (76.12 g/mol) in the sample? [ 9.33 37.52 3.126 ; 12.43 ] % 7. The tetraethyl lead, Pb(C2H5)4 in a 25.00 mL sample of gasoline was shaken with 15.00 mL of 0.02095 M I2. The reaction is Pb(C2HS)4 + I2 Pb(C2HS)3I + C2HŞI After the reaction was complete, the unused I2 was titrated with 6.09 mL of 0.03465 M NazS2O3. I2 + 2NA2S203 → 2Nal + NazS4Os Calculate the weight in milligrams of Pb(C2HS)4 (323.4 g/mol) in each milliliter of the gasoline. [ 8.100; 5.400 2.700 ; 10.80 ]mg/mL

What volume (mL) of 12 M HCl was required to react with the Mg? The data I have for you is this: Mg+2HCl-->MgCl2+H2 is the chemical equation. The mass of magnesium is 0.0273 grams and the moles is 0.001123 The moles of HCl that were consumed in the reaction was 0.002246 moles With this data, I need to know how we can get the volume (mL) of 12 M HCl was required to react with the Mg?

c. For the unbalanced redox reaction Cu + 10 ➜→ Cu²+ + 1₂ Which is oxidizing agent (oxidant)? Write the balanced redox net ionic equation when the reaction is conducted in an acidic solution.

What mass in grams of tin would be required to completely react with 1.85 L of 0.750 M HBr in Sn(s) + 4 HBr(aq) —> SnBr4(aq)+2H2(g)

All iron in 4.00 g of iron ore sample, which was dissolved in an acid solution, was converted to Fe2+ which was then titrated with 0.200 M KMNO4 solution. In this titration all iron is oxidized to Fe3+ and MnO4 to Mn2+. If 27.45 mL of KMNO4 solution is required to the end point, determine 1. How many grams of iron content is in the iron ore sample. 2. The yield percentage of iron in the sample. 3. If the iron in the sample is present as Fe2O3, what is the mass percentage of Fe2O3 in the sample.