a. For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.225 mol of the first reactant. Cl₂ (9) + KI(aq) → I2 (8) + KCl(aq) mol KI b. For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.405 mol of the first reactant. Co(s) + P4 (8)→ Co3 P2 (8) mol P4 c. For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.415 mol of the first reactant. Zn(s) + HNO3(aq) → Zn(NO3)2 (aq) + H₂(g) mol HNO3 d. For the following unbalanced equation, indicate how many moles of the second reactant would be required to react with exactly 0.180 mol of the first reactant. C5 H12 (1) + O2(g) → CO2 (g) + H₂O(g) mol 02

For the following reaction, 0.557 moles of potassium hydroxide are mixed with 0.224 moles of phosphoric acid. potassium hydroxide(aq)+phosphoric acid(aq)= potassium phosphate(aq)+water(l)   What is the formula for the limiting reagent? What is the maximum amount of potassium phosphate that can be produced?

1. Balance the reaction equations below. a) HCl(aq) + _Mg(OH)2(s) – Н-0() + MgCl2(aq) b) _HNO3(aq) + Na,S(aq) → _H,S(g) + NANO3(aq) 2. What is the moles HCI-to-moles MgCl2 ratio in reaction (a)?

3. What mass of NaCl can be produced from 0.55 mol Cl2 in the following reaction? 2 Naa + Cle) → 2 NaCle) d. 88 g a. 0.55 g b. 1.1 g с. 64 g С.

Suppose  0.0350 g Mg0.0350 g Mg is reacted with 10.00 mL of 6 M HCl10.00 mL of 6 M HCl to produce aqueous magnesium chloride and hydrogen gas.      Mg(s)+2HCl(aq)→MgCl2(aq)+H2(g)Mg(s)+2HCl(aq)→MgCl2(aq)+H2(g) What is the limiting reactant in this reaction?

A sample of 8.51 g of solid calcium hydroxide is added to 35.0 mL of 0.480 M aqueous hydrochloric acid. Write the balanced chemical equation for the reaction. Physical states are optional. chemical equation: What is the limiting reactant? hydrochloric acid calcium hydroxide How many grams of salt are formed after the reaction is complete? mass of salt: How many grams of the excess reactant remain after the reaction is complete? excess reactant remaining: g

Consider the unbalanced chemical  reaction equation :  Na2SO4 (aq) + BaCl2 (aq) ---> BaSO4 (s) + NaCl (aq)  Balance the reaction and how many millimeters of a 0.250 M BaCl2 solution are needed to react with 0.0325 L of a 0.160 M Na2SO4 solution?

Use the References to access important values if needed for this question. Enter the coefficients directly from the balanced chemical equation. Do not reduce to lowest terms. For example: If 3 moles H, react with 3 moles 0,, enter "3" for each, not "1". According to the following reaction: 3Cl, (g) + 3H20 (1) → 5HCI (aq) + HClo3 (aq) What would you multiply "moles of chlorine" by to convert to the units "moles of chloric acid (HCIO3)" ? (number) (unit) moles Cl2 = moles HCIO3 (number) (unit)

Sodium bicarbonate reacts with hydrochloric acid in a gas-forming reaction to produce aqueous sodium chloride, water, and carbon dioxide gas NaHCO3(s) + HCl(aq)→NaCl(aq) + H2O(l) + CO2(g) Determine the mass of CO2 gas produced when 8.89 g of NaHCO3 is added to a solution that contains 5.15 g of HCl.

15. If 23.0 mL of a 1.00 M Ba(NO3)2 solution was reacted with 55.0 mL of a 0.700 M solution of K3PO4 to produce the solid Ba3(PO4)2 by the balanced chemical equation 3 Ba(NO3)2 (aq) + 2 K3PO4(aq) – Ba3(PO4)2(s) + 6 KNO3(aq) a. What is the limiting reagent? AS b. How many grams of Ba3(PO4)2 will be produced? elomibt.ESE -3HA