The formula to use for calculations of dilutions is 1. VC =V½C2 2. V¡C2 = V½C1 %3D %3D C1 %3D O 1 O 2 4

A number of reactions can be used to generate common gases on a laboratory scale. For example, nitrogen can be produced from sodium metal and potassium nitrate as indicated by the balanced equation: 10 Na (s)+ 2KNO3(s)= K2o(S)+5Na2O(s)+N2(g) A common laboratory-scale reaction can also generate oxygen gas by heating potassium chlorate, as indicated by the balanced equation: 2KClO3(s)= 2KCl(s)+3O2(g) What mass of potassium nitrate is needed to generate 161.0 L of gas, composed of 101.0 L of N2 and 60.0 L of O2at 0.920 atm and 285  K, using these two reactions? ? g KNO3

if you mix 15.3 mL of 0.320 M solution of K2CrO4 with 55.7 mL of a 0.320 M solution of AgNO3, what mass in grams (g) of Ag2CrO4(s) (MM=331.732 g/mol) is formed? Give your answer with three digits to the right of the decimal point. No marks for the unit.   2AgNO3(aq)+ K2CrO4(aq) → Ag2CrO4(s)+ 2KNO3 (aq)

A student sets up the following equation to solve a problem in solution stoichiometry. (The ? stands for a number the student is going to calculate.) Enter the units of the student's answer. (0.19 L) 1 mL 10-³ 146.86 g mol 1.04 mL = ☐ x10 ロ･ロ X I 00

Let us explore a reaction with a limiting reactant. Here, zinc metal is added to a flask containing aqueous HCl, and H2 gas is a product.   The three flasks each contain 0.300 mol of HCl. Zinc is added to each flask in the following quantities: 4.90 g, 9.81 g, 19.6 g.  When the reactants are combined, the  inflates the balloon attached to the flask. The results are as follows: Flask 1: Balloon inflates completely, but some  remains when inflation ceases. Flask 2: Balloon inflates completely. No Zn remains. Flask 3: Balloon does not inflate completely. No Zn remains.   What mass of Zn was added to each flask? Mass = ? g (flask 1) Mass = ? g (flask 2) Mass = ? g (flask 3)

The reaction below takes place in water at room tempeture. Balance the reaction and write the correct state of matter for the substance.  CaCI_2(aq) + (NH_4)_3PO_4 -> Ca_3(PO_4)_2 + NH_4CI

For the following reaction, 5.82 grams of water are mixed with excess chlorine gas. The reaction yields 14.0 grams of hydrochloric acid. chlorine (g) + water (1) →→→hydrochloric acid (aq) + chloric acid (HCIO3) (aq) What is the theoretical yield of hydrochloric acid ? What is the percent yield of hydrochloric acid ? grams %

Aluminum oxide (used as an adsorbent or a catalyst for organic reactions) forms when aluminum reacts with oxygen. 4Al(s) + 3O2(g) → 2Al2O3(s) A mixture of 101.15 g of aluminum (ℳ= 26.98 g/mol) and 117.65 g of oxygen (ℳ = 32.00 g/mol) is allowed to react.   What is the limiting reactant? What is the excess reactant? What mass of aluminum oxide (ℳ = 101.96 g/mol) can be formed?  Note: Round off your answer to two decimal places

[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant.   b) Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 64.7 grams Al according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) c) Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 201 grams Fe₂O₃ according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) d) Which of the following substances is the limiting reactant? e) What is the mass in grams of the excess Fe₂O₃ remaining after the partial reaction of 201 g Fe₂O₃ with 64.7 g Al? Give your answer to three significant figures.

[References] Use the References to access important values if needed for this question. For the following reaction, 27.8 grams of sodium chloride are allowed to react with 66.9 grams of silver nitrate. sodium chloride ( aq ) + silver nitrate ( aq) → silver chloride ( s) + sodium nitrate ( aq ) What is the maximum amount of silver chloride that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams Visited Submit Answer Try Another Version 1 item attempt remaining Show Hint