Question

5. What mass of calcium chloride must be dissolved in water to renare 200 mL of a solution with concentration of 0.50 M? 6. What is the coefficient for oxygen when this equation is balanced? HS(g) + 20 (8) SO(g) + H2O(l) (B)3 (C)4 (D) 5 7. Ammonia is prepared by the Haber Process. N2 +3 H2< =>2 NHỊ If 2.0 mol of N, and 3.0 mol of Hare combined together, what is the percent of yield if 1.5 mol of Nis is obtained? 8. What would be the volume of oxygen gas produced at 25 °C and 1.0 atm from the electrolysis of 2.0 kg of water? 2H20 (1) ► 2H2(g) + O2(g)
5, 7, and 8 please!

Answer 1

5.

molarity = 0.5M

volume of solution = 200ml = 0.2L

no of moles of CaCl2 = molarity *volume in L

                                = 0.5*0.2   = 0.1moles

mass of CaCl2 = no of moles* gram molar mass

                       = 0.1*111

                        = 11.1g >>>answer

6.2H2S(g) + 3O2(g) -----------> 2SO2(g) + 2H2O(l)

B) 3

7.

N2 + 3H2 -----------> 2NH3

1 mole of N2 react with 3 moles of H2

2 moles of N2 react with = 3*2/1 = 6 moles of H2 is required

H2 is limiting reactant

3 moles of H2 react with exess of N2 to gives 2 moles of NH3

perccent yield   = actual yield *100/theoretical yield

                         = 1.5*100/2   = 75%

8. no of moles of H2O   = W/G.M.Wt

                                   = 2000/18   = 111.11moles

2H2O(l) ------------> 2H2(g) + O2

2 moles of H2O electrolysis to gives 1 mole of O2

111.11moles of H2O electrolysis to gives = 1*111.11/2   = 55.555moles of O2

n = 55.555moles

P = 1atm

T = 25+273 = 298K

PV = nRT

V   = nRT/P

      = 55.555*0.0821*298/1 = 1359L of O2 >>>>answer