Urea, CO(NH2)2 (molar mass: 60.06 g/mol), is commercially manufactured from liquid ammonia (molar mass: 17.031 g/mol) and carbon dioxide (molar mass: 44.01 g/mol) at 180-210 °C. The reaction is given below: cO2 (9) + 2 NH3 (g) → CO(NH,)2 (s) + H20m What mass of liquid ammonia is required to produce 120.0 kg of urea if the percent yield for the reaction is 64.80%? Select one: O a. 52.51 kg NH3 O b. 46.28 kg NH3 O c. 23.14 kg NH3 O d. 105.0 kg NH3

Urea, CO(NH2)2 (molar mass: 60.06 g/mol), is commercially manufactured from liquid ammonia (molar mass: 17.031 g/mol) and carbon dioxide (molar mass: 44.01 g/mol) at 180-210 °C. The reaction is given below: cO2 (9) + 2 NH3 (g) → CO(NH,)2 (s) + H20m What mass of liquid ammonia is required to produce 120.0 kg of urea if the percent yield for the reaction is 64.80%? Select one: O a. 52.51 kg NH3 O b. 46.28 kg NH3 O c. 23.14 kg NH3 O d. 105.0 kg NH3

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...

See similar textbooks

Similar questions

While ethanol (CH₂CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 25 L tank with 12. mol of ethylene gas and 2.7 mol of water vapor. When the mixture has come to equilibri he determines that it contains 10.3 mol of ethylene gas and 1.0 mol of water vapor. The engineer then adds another 0.68 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. mol de wall x10 X 553 S Ws 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibili CH151_152_lab....docx ook Pro A W Chapter 13- Che....doc +
While ethanol CH3CH2OH is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene CH2CH2 with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 75L tank with 16.mol of ethylene gas and 27.mol of water vapor. When the mixture has come to equilibrium she determines that it contains 9.6mol of ethylene gas and 20.6mol of water vapor. The engineer then adds another 9.0mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits.
Imagine that a chemist puts 0.828 mol each of HNO3 and SO2 in a 1.00-L container at a constant temperature of 341 °C. This reaction occurs: 2 HNO3(g) + SO2(g) ⇄ H2SO4(g) + 2 NO2(g) When equilibrium is reached, 0.389 mol of H2SO4 is in the container. Find the value of Keq for the reaction.
Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample of gas from the system is collected into a 5.00 L flask at 1200 K. The flask is found to contain 2.81 g of CH, 1.25 g of CO, 15.1 g of cO, and 25.3 g of H, What is the value of Kc for this reaction? CH.(g) + CO,(9) = 2 CO(g) + 2 H,(g)
The value of KC for the thermal decomposition of hydrogen sulfide, shown below, is 2.2 × 10-4 at 1400 K. A sample of gas in which [H2S] = 5.96 M is heated to 1400 K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H2S]? Assume no H2 or S2 was present in the original sample.
Consider the following reaction where K. = 5.10×10-6 at 548 K. NHẠCI(s)ENH3(g) + HCl(g) A reaction mixture was found to contain 5.15x10² moles of NHCI(s), 1.56×103 moles of NH3(g), and 2.26x103 moles of HCI(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc, equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.
Nitrogen dioxide decomposes according to the reaction 2 NO2 (g) ⇌ 2 NO (g) + O2 (g) Where Kp = 4.48 x 10 ^ -13 at a certain temperature. If 0.40 atm of NO is added to a container and allowed to come to equilibrium, what are the equilibrium partial pressures of NO (g) and O2 (g)? P NO = atm NO P O2 = atm O2 Use correct significant figures.
Consider the following reaction where Kc = 1.20×10-2 at 500 K:PCl5 (g) PCl3 (g) + Cl2 (g)A reaction mixture was found to contain 0.115 moles of PCl5 (g), 4.47×10-2 moles of PCl3 (g), and 4.16×10-2 moles of Cl2 (g), in a 1.00 liter container.Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium PCl5(g) must be consumed . 2. In order to reach equilibrium Kc must increase . 3. In order to reach equilibrium PCl3 must be consumed . 4. Qc is less than Kc. 5. The reaction is at equilibrium. No further reaction will occur.
Consider the following reaction where Kc = 1.29×10-2 at 600 K.COCl2(g) CO(g) + Cl2(g)A reaction mixture was found to contain 0.120 moles of COCl2(g), 4.54×10-2 moles of CO(g), and 4.37×10-2 moles of Cl2(g), in a 1.00 liter container.Is the reaction at equilibrium?If not, what direction must it run in order to reach equilibrium?The reaction quotient, Qc, equals .The reactionfill in the blank 2A. must run in the forward direction to reach equilibrium.B. must run in the reverse direction to reach equilibrium.C. is at equilibrium.
A student ran the following reaction in the laboratory at 479 K: PCI3(g) + Cl₂(g) =PC15(g) When she introduced PCI3(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of PCI3 was 2.13 atm and the initial partial pressure of Cl₂ was 1.34 atm, she found that the equilibrium partial pressure of PCI5 was 1.12 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp Submit Answer Retry Entire Group 8 more group attempts remaining
As you are walking across your laboratory, you notice a 5.25 L flask containing a gaseous mixture of 0.0205 mole NO2 (9) and 0.750 mol N2O4 (q) at 25°C. 4 (g) Is this mixture at equilibrium? If not, will the reaction proceed towards forming more products, or more reactants? N2O4 4 (9) → 2NO2 (9) Ko = 4.61 x 103 at 25°C
Consider the following reaction: CO (g) + 2 H₂ (9) CH3OH (g) A reaction mixture in a 5.21 - L flask at a certain temperature initially contains 27.4 g CO and 2.36 g H₂. At equilibrium, the flask contains 8.65 g CH3OH. Calculate the equilibrium constant (K) for the reaction at this temperature. Kc = Submit ΠΑΠ ΑΣΦ 4 Request Answer ?