A reaction for the reduction of copper is shown 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 are given 3.000 tonnes (3.000x103 kg) of copper oxide.  You check and find that you have 404.9 kg of ammonia gas available to you. What mass (in kilograms) of copper(II) oxide can react with this much ammonia?     CuO(s)  +  NH3(g)  →  Cu(s)  +  H2O(g)  +  N2(g)

A 0.9 g sample of a mixture of KCl and MgCl2 is treated with excess AgNO3(aq). If 2.37 grams of AgCl(s) are obtained, then what is the percentage by mass of KCl in the original mixture? Your answer must be accurate to two significant digits. Keep several extra digits in your calculations and round off only at the end. Do not include the percent sign (%) as part of your answer.   Molar masses (in g mol−1): KCl, 74.55 MgCl2, 95.21 AgCl, 143.35

A student working in a lab, needed to add 1.599 g acetone and 3.2 g of benzaldehyde to a Reaction flask. If the student does not have access to a weighing balance, how would they measure out the reactants ? Provide the name of the equipment/glassware and the final amount that was added to the reaction vial.

Balance the following reaction in basic solution then enter the coefficients of the balanced reaction into the blank spaces. Remember to include "understood" coefficients of 1! 9. Type your answer here Ag20(s) + Type your answer here Al(s) + Type your answer here OH (aq) + H20(1) → Type your answer here Type your answer here Ag(s) + Type your answer here H2A!O3 (aq)

For the following unbalanced chemical equation, suppose that exactly 2.00 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of H2O is expected (assuming that the limiting reactant is completely consumed). H2 (g) + MnO2 (s) → Mn0(s) + H2 O(1) Limiting reactant: Mass of H20 = For each of the following unbalanced chemical equations, suppose that exactly 1.90 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of ICI is expected (assuming that the limiting reactant is completely consumed). I2 (s) + Cl2 (9) → ICI(9) Limiting reactant: Mass of ICl =

Balance this reaction.  If a coefficient is one, enter "1" explicitly.   N2+H2 → NH3

Balance the following equations using lowest whole number coefficients. A number 1 must be placed where applicable.Example:H2O(l) →  H2(g) + O2(g)is correctly balanced as2 H2O(l) →  2 H2(g) + 1 O2(g)You will record only the coefficients as your answer.Your answer should be221

33. You can -Text A 62.5 mL sample of a 0.118 M potassium sulfate solution is mixed with 37.0 mL of a 0.128 M lead(II) acetate solution and the following precipitation reaction occurs: The solid PbSO, is collected, dried, and found to have a mass of 1.00 g - Determine the limiting reactant, the theoretical yield, and the percent yield. ▸ Part A Part B Determine the theoretical yield. mass of PbSO, K₂SO, (aq) +Pb(C₂H₂O₂) (aq) +2KC₂H₂O₂ (aq) + PbSO,(s) ΗΘΕΙ ΑΣΦ Submit Previous Answers Bequest Answer nin * Incorrect; Try Again; 5 attempts remaining ? K

Qa 02.

A chemist goes into the lab and performs an experiment in which a mixture of 8.47 grams of Zn and 6.03 g of sulfur are reacted. Before starting the experiment they perform the following calculations to predict the maximum (theoretical) yield of zinc sulfide that could be produced. First, write a balanced equation: Zn + 2 S → ZnS2 Second, check to see which reagent is limiting: 1 mole Zn 1 mole ZnS, 1 mole Zn 129.4 g ZnS, 1 mole ZnS, 8.47 g Zn × = 16.8 g ZnS, %3D 65.4 g Zn 1 mole ZnS, 129.4 g ZnS, 1 mole ZnS, 1 mole S 6.03 g S × = 12.2 g ZnS, 32.0 g S 2 moles S Since 6.03 g S produces the least amount of ZnS2, the S is limiting! They obtain an actual yield of 8.25 grams of zinc sulfide. Calculate their percent yield to one decimal place.