ment/takeCovalentActivity.do?locator3Dassignment-take [Review Topics] [References Use the References to access important values if needed for this question. According to the following reaction, how many grams of hydrogen iodide will be formed upon the complete reaction of 29.8 grams of iodine with excess hydrogen gas? hydrogen (g) + iodine (s) hydrogen iodide (g) grams hydrogen iodide Submit Answer | Retry Entire Group 9 more group attempts remaining ( Previous Next

ment/takeCovalentActivity.do?locator3Dassignment-take [Review Topics] [References Use the References to access important values if needed for this question. According to the following reaction, how many grams of hydrogen iodide will be formed upon the complete reaction of 29.8 grams of iodine with excess hydrogen gas? hydrogen (g) + iodine (s) hydrogen iodide (g) grams hydrogen iodide Submit Answer | Retry Entire Group 9 more group attempts remaining ( Previous Next

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 78AP: For each of the following balanced equations, indicate how many moles of the product could be...

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Citric acid, C6H5CH3, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger . The equation representing this reaction is C12H22O11+H2O+3O22C6H8O7+4H2O What mass of citric acid is produced from exactly 1 metric ton (1.000103kg) of sucrose if the yield is 92.30%?
Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following: (a) The number of moles and the mass of Mg required to react with 5.00 g of HCl and produce MgCl2 and H2. (b) The number of moles and the mass of oxygen formed by the decomposition of 1.252 g of silver(I) oxide. (c) The number of moles and the mass of magnesium carbonate, MgCO3, required to produce 283 g of carbon dioxide. (MgO is the other product.) (d) The number of moles and the mass of water formed by the combustion of 20.0 kg of acetylene, C2H2, in an excess of oxygen. (e) The number of moles and the mass of barium peroxide, BaO2, needed to produce 2.500 kg of barium oxide, BaO ( O2 is the other product.) (f) The number of moles and the mass of required to react with H2O to produce 9.55 g of
Write the balanced equation, then outline the steps necessary to determine the information requested in each of the following: (a) The number of moles and the mass of chlorine, Cl2, required to react with 10.0 g of sodium metal, Na, to produce sodium chloride, NaCl. (b) The number of moles and the mass of oxygen formed by the decomposition of 1.252 g of mercury(II) oxide. (c) The number of moles and the mass of sodium nitrate, NaNO3, required to produce 128 g of oxygen. ( NaNO2 is the other product.) (d) The number of moles and the mass of carbon dioxide formed by the combustion of 20.0 kg of carbon in an excess of oxygen. (e) The number of moles and the mass of copper(II) carbonate needed to produce 1.500 kg of copper(II) oxide. ( CO2 is the other product.) (f) The number of moles and the mass of formed by the reaction of 12.85 g of with an excess of Br2.
Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to determine the percent yield of a reaction that produces 12.5 g of CCl2F2 from 32.9 g of Cd4. Freon-12 has been banned and is no longer used as a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percent yield.
Titanium dioxide, TiO2 , reacts with carbon and chlorineto give gaseous TiCl4 : TiO2+2C+2Cl2TiCl4+2CO The reaction of 7.39 kg titanium dioxide with excess Cand Cl2 gives 14.24 kg titanium tetrachloride. Calculatethe theoretical yield of TiCl4 (assuming complete reaction)and its percentage yield.
For each of the following incomplete and unbalanced equations, indicate how many moles of the second reactant would be required to react completely with 0. 145 mole of the first reactant. msp;BaCl2(aq)+H2SO4(aq) msp;AgNO3(aq)+NaCl(aq) msp;Pb(NO3)2(aq)+Na2CO3(aq) msp;C3H8(g)+O2(g)
4.47 Silicon carbide is, an abrasive used in the manufacture of grinding wheels. A company is investigating whether they can be more efficient in the construction of such wheels by making their own SiC via the reaction SiO2+3CSiC+2CO (a) If this reaction consistently has a yield of 85%, what is the minimum amount of both silicon dioxide and carbon needed to produce 3400 kg of SiC for the manufacture of cutting wheels? (b) The silicon dioxide is to he obtained from sand and the carbon is derived from coal. If the available sand is 95% SiO2 by weight and the coal is 73% C by weight, what mass of coal is needed for each metric ton of sand used?
For each of the following balanced equations, indicate how many moles of the product could be produced by complete reaction of 1.00 g of the reactant indicated in boldface. Indicate clearly the mole ratio used for the conversion. msp;NH3(g)+HCl(g)NH4Cl(s) msp;CaO(s)+CO2(g)CaCO3(s) msp;4Na(s)+O2(g)2Na2O(s) msp;2P(s)+3Cl2(g)2PCl3(l)
Wnich of the following statements about chemical equations is (are) /true? 1type='a'> When balancing a chemical equation, you can never change the coefficient in front of any chemical formula. i>The coefficients in a balanced chemical equation refer to the number of grains of reactants and products. i>In a chemical equation, the reactants are on the right, and the products are on the left. i>Wnen balancing a chemical equation, you can never change the subscripts of any chemical formula. i>In chemical reactions, the matter is neither created nor destroyed, so a chemical equation must have the same number of atoms on both sides of the equation.
(b) Find the mass of barium sulphate (BaSO4) from the data given in the table. (c) Calculate the moles of barium sulphate (BaSO4) (d) Using stoichiometry for the balanced reactions, Reaction 1 and Reaction 2 from part (a), find the moles of FeS2 (e) Calculate the theoretical mass of FeS2 using your answer for moles FeS2 in part (d) (f) Calculate % mass iron pyrite FeS2 using the theoretical mass and the initial mass of mineral sample. How does your calculated % mass iron pyrite FeS2 compare to the typical 90-95% mass?
. In the gravimetric analysis of determination of loss of water molecules of hydration from a hydrated salt, identify any one possible mistake, and one proper way to fix it. b.To determine the number of moles of the water of crystallization (n) of a hydrated salt, a student took a sample of 5.94 g of a Cobalt(II)chloride hydrate. The student heated the sample over a burner until constant mass. After cooling, he found that the mass of the remaining dehydrated salt was 4.65 g.i. Determine the mass of water lost by the sample. (0.5 mark)and Determine the number of moles of anhydrous Cobalt(II)chloride and water. ii. Calculate the number of moles of water of crystallization(n). iv. Write the molecular formula for the hydrated salt. How can the student make sure that all of the water of hydration has been removed?
According to the following reaction how many grams of carbon dioxide will be formed upon the complete reaction of 25.2 grams of oxygen gas with excess carbon (graphite)?