Given 4.68L CO2 and the following unbalanced equation, complete a-h. ___CaCO3 (s) + ___HCl (aq) → ___CO2 (g) + ___H2O (l) + ___CaCl2 (s) a) Balance the equation density of CO2 = 1.96 g/L      (1.96g CO2/ 1L CO2) b) __?__ g CO2 produced (this is the theoretical yield of g CO2) c) __?__ mol CO2 produced (this is the theoretical yield of mol CO2)

If excess chlorine gas reacts with a solution containing 20.0grams of potassium bromide, how many liters of bromine gas can be produced?   Please show me how this question is solved

Dteremine the limiting reaganet (SHOW THE calculations for determinig the limiting reagent ) and calculate the theoretical mass of PbI2 by using limiting reagent. show your calculations.  Balanced Equation: Pb(NO3)2 (aq) + 2KCL(aq) ---> 2KNO3(aq) + PbI2(s) No of moles of Pb(NO3)2 = 0.003 No of moles of KI = 0.007

6 of 12 Questions Assignment Score: L Give Up? O Hint Check Answer 32.1% Resources Question 6 of 12 > O 4 Question 100% 1 of o Attempts Correct Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation 5 Question 0% 3 of o Attempts In Progress MnO, (s) + 4 HCI(aq) MnCl, (aq) + 2 H,O(1) + Cl, (g) 6 Question 0% How much MnO, (s) should be added to excess HCl(aq) to obtain 105 mL of CI, (g) at 25 °C and 715 Torr? O of o Attempts (Hint: It's another stoichiometry problem. See hints for previous problems. You will get n which is moles of chlorine gas first, 7 Question then use stoichiometry to get moles of the reactant that you need, then grams of that reactant.) 0% O of ∞ Attempts 8 Question 0% O of o Attempts g MnO, mass: 9 Question O of o Attempts 0% 10 Question 0% O of o Attempts 11 Question 0% 0 of o Attempts 12 Question 0% O of o Attempts