1/ For the following reaction, which, if any product, is a precipitate? Enter a name Ba(NO 3)2 + NaC2H3O2 →? Group of answer choices no reaction sodium nitrate barium acetate 2/ For the following reaction, which, if any product, is a precipitate? CaCl2 + Na2CO3? Group of answer choices calcium carbonate no reaction sodium chloride 3/ For the following reaction, which product, if any, is a precipitate? Pb(C2H3O2)2 + Nal? Group of answer choices no reaction sodium acetate lead(II) iodide

Given the following reaction: 2 Al + 2 KOH + 4 H2SO4 + 22 H20 --> 3 H2 + 2KAI(SO2 12H20 If you start with 8.0 mL of 8.9M sulfuric acid, what is the theoretical yield of alum?

i need help on this question

Balance the following reaction. If a reactant or product is not present, put a zero (0) in the blank. H+(aq) + H2O(l) + ClO-13(aq) + e-1 <--> Cl-1(g) + H+(aq) + H2O(l)

Q#6: The following balanced equation will be useful to answer the two questions that follow. MM's are given below each molecule or salt. 2 KMNO4 + 5 K2C204 + 16 HCI 2 MnCl2 + 12 KCI + 10 CO2 + 8 H20 158.04 166.22 36.46 125.84 74.55 44.01 18.0 part A) How many grams of potassium chloride will be produced from the reaction of 25.00 mL of a 0.123 M solution of potassium permanganate? part B) The only gas in the above equation is CO2 (MM = 44.01 g/mol). If 45.3 g of %3D potassium permanganate are completely reacted in a 4.0 L container at 345 K, what is the resulting pressure?

The balanced equation below shows a simple way of manufacturing hydrogen gas in lab (you've done thisl). For your convenience, the molar mass of each substance is shown below their formulas (in purple). Use this information to make the requested calculation: 2 Al(s) + 6 HCI(aq) -> 2 AICI3(aq) + 3 H2(g) 26.982 36.461 133.341 2.016 What volume of hydrogen gas, in mL, would be produced by the reaction of 922 mg of hydrochloric acid with excess aluminum metal?

In the laboratory, you are given the task of separating Ba2+ and Co2+ ions in an aqueous solution. For each reagent listed below, indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES   HCl  Na2S  K2CO3

esc K INTRODUCTION # CALLUJ SI J JIM VULPUTUS. Step 1 Choose match Step 2 Choose match Step 3 Choose match Step 4 Choose match Na2CO3(aq) +CaCl₂ (aq) → 2 NaCl(aq) + CaCO3(s) Calculate the volume (in mL) of 0.200 M CaCl₂ needed to produce 2.00 g of CaCO3(s) There is an excess of Na₂CO3. Molar mass of calcium carbonate = 100.09 g/mol ? Volume of calcium chloride = 100.0 mL 55°F Mostly cloudy @ #/Q/W A LABORATORY SIMULATION 2 S Z X # 3 E $ 4 f5 R METHODS % F DE C Q Search 5 f6 T RESET - G 4+ J (²+ MY NOTES ALAB DATA V B & Y f8 7 H N fg 8 C ly 3 f10 SHOW LABELS DII 9 12 [ NEW

Determine the amount of excess reagent (in grams) left over after 0.1229 g NaOH reacts with 0.2786 g Al. Assume that there is plenty of water to react with both the NaOH and Al, and don't consider it for the excess or limiting reagent. 2 NaOH (aq) + 2 Al (s) + 6 H2O (l) →→4 (aq) + 3 H2 (g)

For each reaction in the table below, write the chemical formulae of any reactants that will be oxidized in the second column of the table. Write the chemical formulae of any reactants that will be reduced in the third column. reaction Cr(s) + O₂(g) Ni (s) + 1₂ (s) S. (s) + 16Cu(s)→ CrO₂ (s) Nil₂ (s) 8Cu₂S (s) reactants oxidized □ reactants reduced 0 0 X 00 Ś