Gas Law Studies1. Mass of zincDetermination of0.8992) Moles of zinc0.01361 mol3.) Moles of hydrogen00?←I was told to calculate thisnumber from mole of zinc.350mSo does that mean it will be 0.01361moltoo?4 Volume of water collected (mL)5) VL of water collected (Liters) 0.350 L6) Temp of water collected (°C)7) Temp of water collected (°K)8) Atmospheric pressure (mm)9) Vapor pressure of water (mm)10) Corrected pressure of hydrogen20%29°C764.0mm Hg(mm)17.5mm11) Corrected pressure of hydrogen (atm)12) Experimentally calculated value of 1913. Literature value of R14) % Error15) Suggest reasons for the % error (#14)

Calculations: 2.Moles of zinc:= mass/molar mass Mass of zinc = 0.89 g…

Answered: Gas Law Studies 1. Mass of zinc…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

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The nitrogen content of organic compounds can be determined by the Dumas method. The compound in question is first reacted by passage over hot CuO(s): CompoundCuO(s)HotN2(g)+CO2(g)+H2O(g) The product gas is then passed through a concentrated solution of KOH to remove the CO2. After passage through the KOH solution, the gas contains N2 and is saturated with water vapor. In a given experiment a 0.253-g sample of a compound produced 31.8 mL N2 saturated with water vapor at 25C and 726 torr. What is the mass percent of nitrogen in the compound? (The vapor pressure of water at 25C is 23.8 torr.)
Hydrogen gas is bubbled into a solution of barium hydroxide that has sulfur in it. The equation for the reaction that takes place is H2(g)+S(s)+2OH(aq) S2(aq)+2H2OWhat volume of 0.349 M Ba(OH)2 is required to react completely with 3.00 g of sulfur?
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In the presence of nitric acid, UO2+ undergoes a redox process. It is converted to UO22+ and nitric oxide (NO) gas is produced according to the following unbalanced equation: H+(aq)+NO3(aq)+UO2+(aq)NO(g)+UO22+(aq)+H2O(l) If 2.55 102 mL NO(g) is isolated at 29C and 1.5 atm, what amount (moles) of UO2+ was used in the reaction? (Hint: Balance the reaction by the oxidation states method.)
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A Boron and hydrogen form an extensive family of compounds, and the diagram below shows how they are related by reaction. The following table gives the weight percent of boron in each of the compounds. Derive the empirical and molecular formulas of compounds A-E.
Gold is produced electrochemically from an aqueous solution of Au(CN)2 containing an excess of CN. Gold metal and oxygen gas are produced at the electrodes. What amount (moles) of O2 will be produced during the production of 1.00 mole of gold?
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The ideal gas law relates the amount of gas present to its pressure, volume, and temperature. The ideal gas law is typically written as ??=???PV=nRT where ?P is the pressure, ?V is the volume, ?n is the number of moles of gas, ?R is the ideal gas constant, and ?T is the temperature. Rearrange the equation to solve for ?.P. ?=P= What is the pressure of 0.638 moles0.638 moles of an ideal gas at a temperature of 297.0 K297.0 K and a volume of 5.58 L?5.58 L? ?=P= atm
For divers going to great depths, the composition of the air in the tank must be modified. The ideal composition is to have approximately the same number of O2 molecules per unit volume as in surface air (to avoid oxygen poisoning), and to use helium instead of nitrogen for the remainder of the gas (to avoid nitrogen narcosis, which results from nitrogen dissolving in the bloodstream). Of the molecules in dry surface air, 78.0% are N2, 21.0% are O2, and 1.00% are Ar. (Assume that the density of seawater is 1025 kg/m3 and the temperature is 20.0°C.) Density of dry air at 20.0°C is 1.20 kg/m3. Molar mass of N2 is 14.007 g/mol, O2 is 15.999 g/mol, and Ar is 39.948 g/mol. a: How many O2 molecules per cubic meter are there in surface air at 20.0°C and 1.00 atm? b: For a diver going to a depth of 141 m, what percentage of the gas molecules in the tank should be O2?
6. If 15.00g of Mg¿(SO4)3 is reacted with 32.25mL of o.2038M of AGNO3 to produce Mg(NO3)2 and Ag.SO4, answer the following questions.
Sources Lx Give Up? Solid ammonium chloride, NH, Cl, is formed by the reaction of gaseous ammonia, NH,, and hydrogen chloride, HCI. NH, (g) + HCI(g) NH,CI(s) A 5.69 g sample of NH, gas and a 5.69 g sample of HCI gas are mixed in a 1.00 L flask at 25 °C. Identify the limiting reagent. O NH,CI O HCI O NH, How many grams of NH Cl will be formed by this reaction? mass: What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH,CI produced by the reaction. P = atm

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