Nexi An aluminum can is cut into small pieces. A 0.62-g sample of the aluminum chips is used to prepare potassium alum according to the procedure described in this experiment. Calculate the theoretical yield (in grams) of potassium alum that could be obtained in the reaction using the correct number of significant figures. The molar mass of potas- sium alum is 474.39 g/mol. slurtnol ori ael momops airli ni basizoidnyemul muizeaio 02-

Use 1 decimal point for all atomic masses. 12.3 g of NCl3(g) are reacted with 0.605 g of H2(g) by the following reaction   NCl3(g) + 3H2(g) --> NH3(g) + 3HCl(g) What is the limiting reagent? NCl3(g) H2(g)     Based on the limiting reagent, what should the yield of NH3(g) be?

Write the balanced chemical equation for the following chemical reactions. Include the correct formulas for all reactants and products and balance with coefficients. Identify the type of reaction in the right column. bbs yd anal Balanced Equation 11. Iron and oxygen react to form iron (III) oxide. OCH Fet 302 12. 2 Fe203 Ag No 3 t. MgCl2 → Mg (NO 3 ) ₂ + Ag Cl 100 H 2 + onjа ин erit anionels (a)tubara en ho (e)slümot dit gnishw bubong salt goinlinereb di bis 87 Holdsset to says arls noised to sayI temessige eldung A equations for the either the read odstrabi 18229090 Type of Reaction Silver nitrate and magnesium chloride react to form magnesium nitrate and silver chloride. Double displacement reaction 13. Aluminum reacts with copper (II) sulfate to form aluminum sulfate and copper solid. OCH H The Redox reaction 01019 ion 02 H OVBA noitsup3 beonsle8 upe ghiwollet od: 919lamo zinaibittooo ritiw noitsupe +Del Calld OSH TOVEN TO 350°F BAKING SMEROM BOX AND d only for orders at…

3 CuO(s) + 2 Al(s) → 3 Cu(s) + Al2O3(s) 25.0 g of copper(II) oxide are combined with 25.0 g of Al , and the mixture is heated strongly to react. molar masses (g/mol):  CuO - 79.55    Al - 26.98    Cu - 63.55   If 18.2 g of Cu metal is recovered from the reaction, what is the percent yield of the reaction?  Do not include the percent sign (%) on your submitted answer.

For the following reaction, 37.3 grams of sulfuric acid are allowed to react with 42.5 grams of zinc hydroxide. sulfuric acid (aq) + zinc hydroxide(s) → zinc sulfate (aq) + water (1) What is the maximum amount of zinc sulfate that can be formed? Mass= What is the formula for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? Mass= g.

Use 1 decimal point for all atomic masses. 82.1 g of Ni3C(s) are reacted with 1.80 g of H2(g) by the following reaction   Ni3C(s) + 2H2(g) --> 3Ni(s) + CH4(g) What is the limiting reagent? H2(g)Ni3C(s)     Based on the limiting reagent, what should the yield of Ni be?   g

Consider the following chemical reaction HCl (aq)  + HgNO3 (aq) à Hg2Cl2 (s) + HNO3 (aq) If 20.0 grams of HCl is mixed with 30.0 grams of HgNO3     Determine the excess reactant   The amount of the solid precipitate that was recovered equals to .................. grams , if the percentage yield from this reaction was determined to be 78.4%. Write the net ionic equation for the chemical reaction   Determine the type of this chemical reaction

Consider the balanced chemical equation when 18.3 g Al is reacted with 113 g I₂ to form AlI₃(g). a. Calculate the theoretical yield in grams AlI₃ from the complete reaction of 18.3 grams Al according to the following balanced chemical equation: 2 Al(s) + 3 I₂(s) → 2 AlI₃(s) b. Calculate the theoretical yield in grams AlI₃ from the complete reaction of 113 grams I₂ according to the following balanced chemical equation: 2 Al(s) + 3 I₂(s) → 2 AlI₃(s) c. Which of the following substances is the limiting reactant? 2 Al(s) + 3 I₂(g) → 2 AlI₃(g) d. What is the mass in grams of the excess Al remaining after the partial reaction of 18.3 g Al with 113 g I₂? 2 Al(s) + 3 I₂(g) → 2 AlI₃(g)

For the following reaction 36.4 grams of sulfuric acid are allowed to react with 40.1 grams of zinc hydroxide. What is the maximum amount of zinc  sulfate that can be formed? What is the formula for the limiting reagent? What amount of the excess reagent remains after the reaction is complete?

For the reaction of sodium sulfide with iron(III) chloride below (as an unbalanced reaction - that's how I will almost always give you reactions.  ALWAYS check to see if a reaction is balanced before you use it.  You balanced it in the last question; make sure you have that right before you start calculating!), you have 319.5 kg of sodium sulfide and 502.3 kg of iron(III) chloride available. What mass (in kilograms) of sodium sulfide do you NEED if you're going to reduce  all of the iron(III) chloride you have?   Na2S(s)  +   FeCl3(s)    →   Fe2S3(s)   +  NaCl(s)