A student was given an unknown chloride of copper. He was asked to determine the formula of the chloride. He mixed the chloride with 2.125 g Zn. When the reaction was completed, the copper that was formed from the reaction was transferred (following a series of steps to detach the copper solid from the Zn solid and washing off zinc chloride from it) to a previously weighed out evaporating dish. Fill in the blanks in answering the question. Mass of Zinc chloride = 4.293 g Mass of evaporating dish = 10.320 g Mass of evaporating dish + copper (after drying) = 14.320 g Mass of copper = 4.00g Mol of copper in original chloride? 0.063 mol Mol of zinc chloride ? 0.315 mol Mol of Cl in the chloride? 0.0315/0.063 I Mol CI/Cu? 1/2 For Blank 4 Chemical Formula of the copper chloride? CUC12 Systematic name of the copper chloride cupric chloride

A student was given an unknown chloride of copper. He was asked to determine the formula of the chloride. He mixed the chloride with 2.125 g Zn. When the reaction was completed, the copper that was formed from the reaction was transferred (following a series of steps to detach the copper solid from the Zn solid and washing off zinc chloride from it) to a previously weighed out evaporating dish. Fill in the blanks in answering the question. Mass of Zinc chloride = 4.293 g Mass of evaporating dish = 10.320 g Mass of evaporating dish + copper (after drying) = 14.320 g Mass of copper = 4.00g Mol of copper in original chloride? 0.063 mol Mol of zinc chloride ? 0.315 mol Mol of Cl in the chloride? 0.0315/0.063 I Mol CI/Cu? 1/2 For Blank 4 Chemical Formula of the copper chloride? CUC12 Systematic name of the copper chloride cupric chloride

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

. Consider a 3.52-g sample of CaCO3 (99.87% pure) in a flask and a 100.0 mL sample of vinegar (5% acidity) in a graduated cylinder. The combined mass of both reagents and containers is 255.98 g. After swirling the reaction mixture for about twenty minutes, the combined mass of the reaction mixture and containers is found to be 254.46 g. What is the percent yield of carbon dioxide in this experiment?
In several sequential reactions a chemist uses carbon, CaO, HCl and H₂O for C₆H₄Cl₂ (147.09 g mol⁻¹). Assuming the efficiency of the reaction is 68% and some C₆H₄Cl₂ and 3 moles of CO are formed from the initial total carbon, how many grams of C₆H₄Cl₂ are obtained from 500 g of carbon?
The density of sodium chloride is 2.164 g cm-³. What is the molar concentration of NaCl in a 14.5 cm³ sample of pure NaCl? molar concentration = i M What is the molar concentration of NaCl in a 25.9 g sample of pure NaCl? molar concentration = M
In one reaction, 41.2 g of Cu(NO3)2 is produced. What amount (in mol) of CuCl2 was consumed? What mass (in grams) of AgCl is produced? mol CuCl2 consumed g AgCl produced
You are given a mixture of CuCO3 and CuO. You place the mixture in a crucible and heat it to decompose the CuCO3 into CO2 gas and CuO. You made sure that the CuCO3 had completely decomposed by constantly heating it, cooling it, and weighing it until the mass remains the same. Using the data below from the experiment, calculate the % CuCO3 in the original sample. Mass of empty crucible: 22.19 g Mass of crucible + sample before heating: 23.193 g Mass of crucible + sample at constant mass: 22.851 g PLease show and create one solution map: i made this solution map, is it correct? 1.561g CO2 x (1mol CO2/44.01g CO2) x (1mol CrCO3/1mol CO2) x (112.01g CrCO3/1mol CrCO3)= 3.973g CrCO3 than, (3.973/25.422) x 100% = 15.63% 2.) A 12.622 g sample of a compound that contains sulfur is analyzed by precipitating all the sulfur as BaSO4. If 11.957 g of BaSO4 are obtained in the analysis, what is the percentage of sulfur in the original compound? (Need help with this one too)
What is the amount of excess reactant left over at the end of the reaction. Use the first image as an example.
Classify each chemical reaction.
Aqueous solutions barium chloride and potassium sulfate are combined. 1) Predict the products and write the balanced equation showing the states of each substance. 2) The barium chloride solution has a volume of 100.0 mL and contains 10.00 grams of barium chloride. The molarity of the potassium sulfate solution is 0.574 moles/liter and has a volume of 100.0 mL. Determine the limiting reactant and the mass of each product in grams. 3) Determine how many grams of excess reactant remain. 4) Calculate the molarity of just the potassium ions after the reaction has finished.
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
[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.
1. Mg (s) + HNO3 (aq) → Mg(NO3)2 (aq) + H2 (g) ,this reaction is considered to be a: * Synthesis Combustion Single replacement Double replacement
Consider the general chemical equation 3A+B→2C. Part A. If 1.45 g of A reacts with 1.75 g of B, what is the mass of C? Express your answer with the appropriate units. Part B. If 4.70 g of A reacts to produce 8.95 g of C, what is the mass of B? Express your answer with the appropriate units.