38. ** Questions 37 through 39 use the reaction: 2 Fe (s) + 6 HCI (aq) → 2 FeCl3 (aq) + 3 H2 (g) When 98.63 ml of 1.905 M hydrochloric acid react with excess iron how many moles of hydrogen gas form? Select one: a. 0.03132 mol b. 0.5637 mol c. 0.9180 mol d. 0.09395 mol e. 0.1879 mol f. 5.508 mol g. none of these h. 2.754 mol

A student performed a similar experiment starting with a 3.2 g sample of marble chips and 75 mL of HCl solution of unknown concentration. The amount of marble chips left at the end of the reaction was 1.70 g. What is the molarity of the acid?

You react 7.35 g Al with 0.150 L of 4.5 M HCl solution according to the given reaction.  Balanced Equation: 2Al (s) + 6HCl (aq) -- > 2AlCl3 (aq) + 3H2 (g) How many grams of AlCl3  are produced? What is the molarity of the remaining HCl solution?

2. 100.0 mL of 5.0 M Cu(NO3)2 was poured into a 1 L container. a. How many mols of Cu(NO3)2 is in the container? b. 350.0 mL of water was added. What is the concentration of NO3?

What is the concentration of an HI solution if 0.5967 g of HI are dissolved in enough water to make 32.23 mL of solution? The molar mass of HI is 127.904 g/mol.     6.651 M     0.1447 M     0.1504 M     6.909 M     0.01447 M

12. Sulfuric acid can dissolve aluminum metal according to the following reaction. 2 Al(s) + 3 H₂SO4(aq) Al2(SO4)3(aq)+3 H2(g) Suppose you wanted to dissolve an aluminum block with a mass of 29.0 g and you have 1.80 L of 1.00 M sulfuric acid available. a) Determine the limiting reactant. What is the theoretical yield of aluminum sulfate? 2/3/22 b) After the reaction is complete, you weigh the aluminum sulfate and it has a mass of 145 g. What is the percent yield of aluminum sulfate?

A student dissolved 6.00 g of Co(NO3)2 in enough water to make 100. mL of stock solution. He took 4.00 mL of the stock solution and then diluted it with water to give 275. mL of a final solution. How many grams of NO3- ion are in the final solution? 0.0296 g 0.0592 g 0.0814 g 0.163 g