Copper(II) sulfate has been used extensively as a fungicide (kills fungus) and herbicide (kills plants). Copper(I1) sulfate can be prepared in the laboralory by feaction of copper CuO(e) + H,80,(ag)CuSO,(ag) + H,O(1) If2.03 g of copper(II) oxide is treated with 5.00 g of pure sulfuric acid, which reactant would limit the quantity of copper(II) sulfate that could be produced? Limiting reactant: Submit Answer Try Another Version 1 item attempt remaining

Copper(II) sulfate has been used extensively as a fungicide (kills fungus) and herbicide (kills plants). Copper(I1) sulfate can be prepared in the laboralory by feaction of copper CuO(e) + H,80,(ag)CuSO,(ag) + H,O(1) If2.03 g of copper(II) oxide is treated with 5.00 g of pure sulfuric acid, which reactant would limit the quantity of copper(II) sulfate that could be produced? Limiting reactant: Submit Answer Try Another Version 1 item attempt remaining

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...

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Many mining operations produce tailings that can be oxidized to form acids, including sulfuric acid. One chemical that reacts in this way is chalcopyrite, CuFeS2, whose net oxidation can be described by the following equation. 4 CUFES2(s) + 17 О2(9) + 10 Н:0() — 4 Fe (ОН), (s) + 4 CUSO4 (ад) + 4 H;SO4(aд) In a laboratory experiment to study weathering, a mining engineer put a 1.63 kg sample of CuFeS2 (s) near an empty 40 L container. Simulated weathering experiments were conducted and the runoff was collected, leading to 35.5 L of solution. A 25.00 mL aliquot of this solution was analyzed with 0.0100 M NaOH(ag). The titration required 31.3 mL of base. (а) What was the concentration (in M) of sulfuric acid? M (b) Assuming the only acid in the container comes from the reacted chalcopyrite, what mass (in g) of the chalcopyrite has reacted? (c) What percentage of the chalcopyrite reacted in this experiment? %
2. In the laboratory, O2(g) can be obtained from the following thermal decomposition reaction of potassium chlorate (KCIO3) with the aid of catalyst: A, MnO2 (catalyst) 2KC1O;(s) > 2KCI(s) + 302(g) To determine the composition of the mixture of KCIO3 and potassium chloride (KCI), 0.612 g KCIO3/KCl mixture is taken into a test tube and heated in the presence of sufficient catalyst, MnO2. The total mass of the test tube after heating decreased by 0.096 g. According to this result, what is the percentage of the KCIO3 in the mixture? (K: 39.0 g/mol, Cl: 35.5 g/mol, O: 16.0 g/mol)
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In the reaction CrCl3 (aq) + 3 AgNO3 (aq) --> Cr(NO3)3 (aq) + 3 AgCI (s) 4.4 moles of CrClą are reacted with 1 moles of AgNO3. Determine the theoretical yield in mols of the product, silver chloride.
B) Sodium hydroxide (NAOH) reacts with sulfuric acid (H2SO.) to form sodium sul- fate (Na2SO4) and water (H2O). The chemical equation is NAOH + H2SO4 Na SO, + H20.
Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N2(3) + 3H,(g) 2 NH, (g) In the second step, ammonia and oxygen react to form nitric acid (HNO,) and water: NH, (g) + 20,(g) - HNO, (g) + H,0 (g) Suppose the yield of the first step is 79.% and the yield of the second step is 70.%. Calculate the mass of nitrogen required to make 6.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
Lead ions can be precipitated from solution with KCI according to the following reaction: Pb (aq) + 2 KCI(aq) PbCl2 (s) + 2 K" (aq) When 28.7 g KCI is added to a solution containing 25.8 g Pb, a PbCla precipitate forms. The precipitate is filtered and dried and found to have a mass of 29.6 g
The mineral iron pyrite (FeS2), typically, has a mass percentage of what is known as fool’s gold of 90-95%. The actual percentage in a sample can be determined using gravimetric analysis. To find the % mass of FeS2 the sulphur in FeS2 is firstly converted to sulphate (SO42-). These sulphate ions (SO42-) is mixed with an excess of barium chloride (BaCl2) to form barium sulphate (BaSO4), according to the following reaction: Ba2+(aq) + SO42- (aq) à BaSO4 (s) When the reaction has gone to completion, the BaSO4 precipitate is collected in a filter paper and carefully washed. The filter paper and its contents are then transferred to a crucible. The crucible and its contents are heated until constant mass is achieved. The data for the analysis of a mineral sample is shown in the table below: Initial Mass of mineral sample 17.5 g Mass of crucible and filter paper 144.60 g Mass of crucible, filter paper and dry BaSO4 196.89 g Molar mass…
Which of the following correctly expressed the balanced equation for the following word equation:
A 5.0-g sample of greenish-yellow Cl₂ gas is added to a 10.0-g sample of gray potassium metal to form a white solid in a sealed container.poitor 2007 bixosq (a) Write a balanced equation for the combination reaction that should occur. H for 25. nailw (b) Identify the limiting reactant. (c) Predict the appearance of the substances left in the reaction container once the reaction is complete. (d) Calculate the mass of product that should form. 10 (e) What mass of excess reactant should be mixed with sis to for the product after the reaction is complete? 6.113 6 E