mmonia is not the only possible fertilizer. Others include urea, which can be produced by the eaction: CO (g) + 2 NH3 (g) → CO(NH, )2(s) + H2 0(g) A scientist has 72 g of dry ice to provide the carbon dioxide. If 4.50 L of ammonia at 15°C and a ressure of 1.2 atm is added, which reactant is limiting? imiting reactant: carbon dioxide Vhat mass of urea ammonia lass =

mmonia is not the only possible fertilizer. Others include urea, which can be produced by the eaction: CO (g) + 2 NH3 (g) → CO(NH, )2(s) + H2 0(g) A scientist has 72 g of dry ice to provide the carbon dioxide. If 4.50 L of ammonia at 15°C and a ressure of 1.2 atm is added, which reactant is limiting? imiting reactant: carbon dioxide Vhat mass of urea ammonia lass =

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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(a) (c) A column of water in a buret is 336 mm Hg high. How high would that column be if it were mercury instead of water? (d) In order for the pressures to be equal, density and height of a column are inversely proportional, therefore the following relationship applies: (denHg)(hHg) = (denH20)(hH20) Note: the density of mercury is 13.6 g/mL and the density of water is 1.00 g/mL. An electrolysis experiment was run for 15 minutes and 45 seconds at an average current of 189 milliamps (mA). The mass lost by the copper anode was 0.0589 grams. (b) Calculate the number of coulombs transferred. (Remember: coulomb = amps x sec) Show full calculation of the height in mercury (remember to use proper significant figures.) Calculate the moles of copper lost from the anode. Based on the moles of copper lost determined in 1c, calculate the moles of electrons transferred. Remember, the reaction at the copper anode is: Cu(s)---> Cu¹² (aq) + 2 e
What volume of carbon dioxide gas (in mL) at 835 mm Hg and 37 °C can be produced when 2.4 g of CaCO3(s) are put into an Erlenmeyer flask containing 108 mL of 0.152 M HCl(aq) ?1 CaCO3(s) + 2 HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l)
1) Calculate the volume of 1.62g of Helium gas at 25.670C and 872 mmHg. (R = 0.0821 atm.L/mol.K) 2) Given the following reaction of Ca(s) in HCl(aq): Ca(s) + 2 HCl(aq) --> CaCl2(aq) + H2(g) If 32.7g of calcium solid are placed in this reaction and at the end of the experiment, hydrogen gas is produced at 25.000C and with a pressure of 790. mmHg. Calculate the volume of hydrogen gas produced. 3) An unknown gas with a mass of 1.211g occupies a volume of 677 mL. The temperature is 230C and the air pressure is 0.987 atm. Calculate the molar mass of the gas.
A mixture of gases contains 3.16 g of 03, 7.86 g of H2, and 2.79 g of SF6. What is the partial pressure in atm of each component of this mixture if it is held in a 25.9-L vessel at 23.0 °C? Use R = 0.0821 L-atm/mol-K as the value of the gas constant. O a) P(03) = 14.3 atm, P(H2) = 0.241 atm, and P(SFs) = 49.1 atm. O b) P(03) = 41.4 atm, P(H2) = 2450 atm, and P(SF6) = 12.0 atm. O c) P(03) = 0.498 atm, P(H2) = 1.24 atm, and P(SF6) = 0.440 atm. O d) P(03) = 0.337 atm, P(H2) = 0.136 atm, and P(SF6) = 0.382 atm. O e) P(03) = 0.0618 atm, P(H2) = 3.65 atm, and P(SFs) = 0.0179 atm.
The combustion of fuel in your car engine requires oxygen gas, which is supplied as air (21% oxygen molecules) into the engine. Consider a car that is using 100% ethanol, C2H5OH, as fuel. If your engine intakes 2.71 L of air per minute at 1.00 atm and 25ºC, what is the maximum volume of ethanol (0.789 g/mL) that can be burned per minute? Hint: You can ignore the "per minute" information because both the ethanol and air are being quantified per minute. Enter the answer to three significant figures in units of mL.
Potassium permanganate, KMnO4, is produced commercially by oxidizing aqueous potassium manganate (K2MnO4) as shown in the equation below. What volume of chlorine gas is required to produce 10.0 grams of KMnO4 if the chlorine gas is at 1.00 atm and 0.00 C? 2 K2MnO4 + Cl2 --> 2 KMnO4 + 2 KCl
Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation: 2Al(s) + 2NAOH(aq) + 6H2O(1)-2NAAI(OH)4(aq) + 3H2(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 759 mm Hg. If the wet H, mol. The vapor gas formed occupies a volume of 7.78 L, the number of moles of Al reacted was pressure of water is 23.8 mm Hg at 25 °C.
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An experiment is performed to determine the volume of gas produced by the following reaction: 2HCl(aq) + Mg(s) MgCl2(aq) + H2(g) A. What is the maximum mass of Mg in g that could be reacted at 20oC temperature and 1.0atm, if the volume of the gas burette is 50mL? (Hint: Find moles of H2 using the ideal gas law; then, convert to g of Mg.) B. If the experiment were moved to a higher elevation and the pressure was decreased to 0.95 atm would the maximum amount of Mg increase or decrease? C. If 16mg of Mg were reacted, what is the volume of gas produced in this reaction? D. What is the solvent for this reaction? E. Would the HCl(aq) be considered a strong, weak, or non-electrolyte? F. Would the MgCl2(aq) be considered a strong, weak, or non-electrolyte?
When active metals such as magnesium are immersed in acid solution, hydrogen gas is evolved. Calculate the volume of H2(g) at 30.1°C and 0.85 atm that can be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride. Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) (R = 0.08206 L • atm/K • mol)
Automobile airbags are inflated by the rapid decomposition of sodium azide (NaN3). 2 NaN3(s) --> 2 Na(s) + 3 N2(g) What volume of N2 gas, at 0.973 atm and 21.3 oC, is produced by the complete decomposition of 119 g of sodium azide? V = ___ L
11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b) The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.