Question

Must write equation with format and choices given. Not just final answer. Fill in with options given. May add factors.

How many liters of a 0.209 M KI solution is needed to completely react with 2.43 g of Cu(NO)2 according to the balanced chemical reaction: 2 Cu(NO3)2(aq)+4Kl(aq)-2 Cul(aq) I2(s) + KNO3(aq) 4 х STARTING AMOUNT RESET ADO FACTOR ANSWER 0.00542 166 187.57 4 0.124 2.43 2 0.209 6.022 x 1023 0.0620 0.0310 1 mol Cu(NO3)2 mL Cu(NO3)2 L Cu(NO3)2 L KI M KI g KI mL KI mol K g Cu(NOs)2

Answer 1

Answer Given that, Mass of cu CNO3)₂ = 2.43 g . finstly we calculate the no. of moles of Cu CNO3)₂ Given mass no of moles of Eu CNO3)2 = Molar mass 2.438 ,-/-0013 mote 187.56 g mol-1 Given reaction 2 Cu (NO3), caq) + 4 kI canj 2CuI caq) + 4 Knq (ay) it means 2 mole of Cu(NO3), react with 4 male of KI So moles of KI = 2 x moles of Cu(NO₃)₂ = 2x 0.013 mole = 0.026 mol Now we calculate the man y volume of kI Molarity = no al moles Volume = - Volume in no of moles 0.026 mote molarity 0.209 mole El volume = 0.124L