Given the following reaction. 2Na2S + __Na2CO3 + __SO2(g) __Na2S2O3 + CO2(g) DH =-1025kJ A. Balance the above equation by filling in the missing coefficients. B. Provide the name of Na2CO3. C. How many grams of CO2(g) would be produced if 12.5g SO2(g) reacted with 10.0g Na2S. Assume Na2CO3 is in excess.

Given the following reaction. 2Na2S + Na2CO3 + SO2(g) __Na2S2O3 + CO2(g) DH =-1025kJ A. Balance the above equation by filling in the missing coefficients. B. Provide the name of Na2CO3. C. How many grams of CO2(g) would be produced if 12.5g SO2(g) reacted with 10.0g Na2S. Assume Na2CO3 is in excess.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter5: Gases

Section: Chapter Questions

Problem 25QAP: Cyclopropane mixed in the proper ratio with oxygen can be used as an anesthetic. At 755 mm Hg and...

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Cyclopropane mixed in the proper ratio with oxygen can be used as an anesthetic. At 755 mm Hg and 25C, it has a density of 1.71 g/L. (a) What is the molar mass of cyclopropane? (b) Cyclopropane is made up of 85.7% C and 14.3% H. What is the molecular formula of cyclopropane?
A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
In the reaction: As2O3 + H2O + I2 = As2O5 + HI, 300 g of As2O3 is added to 400 g of I2 and 50 g of H2O. a) Find the limiting and excess reactants.b) What are the % excess reactants?c) If 160g of As2O5 is formed, what is the degree of completion?d) Illustrate the Law of Conservation of Mass for the reaction.
Methane is produced in the human gut during digestion. As it passes through the digestive tract, it collects at thelower end and is emitted as flatulence. About 10% of a fart is composed of methane.__CH4 + __O2 → __ CO2 + __H2Oa) The average human fart contains 0.00643g of methane gas. Ifyou were to light said fart (and you SHOULD NOT), what mass ofoxygen would combust along with it?b) People, on average, pass 0.75L of gas per day. This is about0.0536g of methane per 24 hour period (remember, only ~10% ismethane). What mass of water could be generated by one personigniting their “methane emission”? c) How many water molecules is this? (SHOW ALL WORK IN TRAIN TRACKS)
The manufacture of aluminum includes the production of cryolite (Na3AlF6) from the following reaction: 6〖HF〗_((g))+3〖NaAlO〗_(2(s))→ 〖Na〗_3 〖AlF〗_(6(s))+3H_2 O_((l))+ 〖Al〗_2 O_(3(s)) How much HF (hydrogen sulfide) is required to produce 2.50kg of Na3AlF6? How many cm3 of HF(g) are needed to produce 26.0g of Na3AlF6? The density of HF (g) at 25is 1.15g/L.
Soda ash (sodium carbonate) is widely used in the manufacture of glass. Prior to the environmental movement much of it was produced by the following reaction. CaCO3 + 2 NaCl → Na2CO3 + CaCl2 Unfortunately, the byproduct calcium chloride is of little use and was dumped into rivers, creating a pollution problem. As a result of the environmental movement, all of these plants closed. Assume that 125g of calcium carbonate (100.09 g/mol) and 125 g of sodium chloride (58.44 g/mol) are allowed to react. Determine how many grams of useful sodium carbonate (105.99 g/mol) will be produced. How many grams of useless calcium chloride (110.98 g/mol) will be produced? You should also determine how many grams of excess reactants are left (indicate which one is the limiting reactant)
Sulfuric acid, H2SO4, can be formed from the chemical reaction 2SO2+O2+H2O--->2H2SO4. Suppose 400g of SO2; 175g of O2, and 125 g H2O are mixed and the reaction proceeds until one of the reactants is used up. How many grams of H2SO4 is produced?A. 612gB. 620gC. 622gD. 630g
14. If 124g of Al reacts with 601g of Fe2O3 as per the following reaction2Al + Fe2O3 → Al2O3 + 2FeCalculate the mass of Al2O3 formed. Indicate which is the limiting reactant.
Part A. How many moles of O2, are needed to react with 1.40 mol of C2H2? Part B. How many moles of CO2 are produced When 0.135 mol of O2 reacts? Express your answer to three significant figures and include the appropriate units.
If 0.300 mol of liquid H2O reacts stoichiometrically according to the balanced equation, how many grams of solid Al2S3 are required? Al2S3(s) + 6H2O(l) → 2Al(OH)3(s) + 3H2S(g) Molar Mass (g/mol) H2O 18.015 Al2S3 150.16 Density (g/mL) H2O 0.9982 Molar Volume (L) 22.4 at STP Gas Constant(L.atm.mol-1.K-1) 0.0821
If 0.460 mol of liquid CS2 and 0.500 mol of gaseous O2 are reacted stoichiometrically according to the balanced equation, how many moles of gaseous CO2are produced? CS2(l) + 3O2(g) → CO2(g) + 2SO2(g) Molar Mass (g/mol) CS2 76.143 O2 31.998 CO2 44.009 Density (g/mL) CS2 1.26 Molar Volume (L) 22.4 at STP Gas Constant(L.atm.mol-1.K-1) 0.0821
Calcium carbonate decomposes to form carbon dioxide and calcium oxide. CaCO3 --> CO2 + CaO. How many liters of carbon dioxide can 200g of CaCO3 generate?

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