3. A balanced chemical reaction and corresponding reaction map are shown below. Where do the numbers written above and below the arrow between "Milliliters of H2" and "Moles of H2 (g)" come from? * 1 Mg (s) + 2 HCI (aq) → 1 H2 (g) + 1 MgClh (aq) Milliliters of H2 Grams of Mg 2 mol HCI 1 mol H2 Moles of Moles of Moles of Mos Mg (s) 1 mol Mg HCI (aq) 2 mol HCI H: (g) O a. They come from how many moles are in a milliliter of gas. O b. They are atomic numbers from the periodic table. O c. They are the molar mass of H2. d. They correspond to coefficients in the balanced equation. 0.000045 mol H2 I milliliter 1 mol Mg 24.31 g Mg

Suppose a 250. mL flask is filled with 0.20 mol of H₂S, 1.1 mol of CS2 and 1.2 mol of H₂. This reaction becomes possible: CH₂(g) + 2H₂S (g) = CS₂(g) + 4H₂(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of CH4. You can leave out the M symbol for molarity. initial change equilibrium CH4 X H₂S 0 CS2 0 H₂ 0 X S

If a solution containing 123.67 g of silver nitrate is allowed to react completely with a solution containing 11.85 g of lithium hydroxide, how many grams of solid precipitate will be formed?   How many grams of the reactant in excess will remain after the reaction?   Assuming complete precipitation, how many moles of each ion remain in solution? If an ion is no longer in solution, enter a zero (0) for the number of moles.   Li+:   OH-:   Ag+:   NO3-:

Suppose a 500. mL flask is filled with 0.40 mol of CH4, 0.30 mol of H₂S and 0.10 mol of CS2. This reaction becomes possible: CH(g)+2H,S(g) CS2(g)+4H2(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of CS2. You can leave out the M symbol for molarity. initial change equilibrium CS₂ H₂ CH₁ H,S છું" 0 n 0 D X 0 ㅁㅁ X 5

Suppose a 250. mL flask is filled with 0.80 mol of CH4, 1.6 mol of H2S and 1.0 mol of H₂. This reaction becomes possible: CH4(g)+2H2S(g) CS2(g) +4H2(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of CS2. You can leave out the M symbol for molarity. initial change equilibrium CH H,S CS2 H₂ U X Fraction

For each of the following precipitation reactions, calculate how many grams of the first reactant are necessary to completely react with 18.0 gg of the second reactant. Na2CO3(aq)+CuCl2(aq)→CuCO3(s)+2NaCl(aq) to g

A sample of 0.75 g of hydrogen gas was obtained by reacting 32.5 g hydrochloric acid with 18.0 g magnesium. Mg(s) + 2 HCI (aq) --> MgCl₂ (aq) + H₂(g) What is the percent yield for this reaction? 100% 83% 41% 50%

What is the mass of solute in each of the following solutions? Express your answers with the appropriate units. A. 3.00 L of 2.00 M NaOH m= B. 3.00 L of 0.200 M LiHCO3 m= C. 25.0 mL of 0.500 M CuCl2 m=

What is the mass of solute, in grams, in 100. mL of a -3 1.179 × 10-³ M solution of Na3PO4? Mass of solute = g 3- What are the molar concentrations of the Na+ and PO4³- ions? Molar concentration Na+ 3- Molar concentration PO4³ = = M M

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