A researcher needed some N-methylbenzamide but only had sodium benzoate available. What reaction conditions could they use to convert their sodium benzoate to the desired product? 00 1.) SOCI₂, pyridine; 2.) CH3NH₂ 1.) H₂O, HCI; 2.) CH3NH2 1.) CH3NH₂; 2.) H₂O, HCI 1.) H₂ CrO4; 2.) NH3 NHCH3

A researcher needed some N-methylbenzamide but only had sodium benzoate available. What reaction conditions could they use to convert their sodium benzoate to the desired product? 00 1.) SOCI₂, pyridine; 2.) CH3NH₂ 1.) H₂O, HCI; 2.) CH3NH2 1.) CH3NH₂; 2.) H₂O, HCI 1.) H₂ CrO4; 2.) NH3 NHCH3

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

What is the sum of coefficients from the following reaction (both products and reactants)? X.3H2O + Heat ---> X can be any element.
The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(II) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. 2. Suppose 53.0mL of dioxygen gas are produced by this reaction, at a temperature of 50.0°C and pressure of exactly 1atm. Calculate the mass of mercury(II) oxide that must have reacted. Be sure your answer has the correct number of significant digits.
4. A solution is prepared by taking a clean and dry 50.00 mL volumetric flask. Some sucrose (Mm 342.2 g/mol) is added to the flask with the following mass measurements recorded: mass of empty volumetric flask: 142.88 g mass of weighing dish + sucrose: 29.83 g mass of weighing dish after adding sucrose to volumetric flask: 24.62 g Some water is added to the flask, the solution stirred until all the sucrose is dissolved. Then water is added carefully to the mark on the flask. The filled flask is then weighed again. mass of filled volumetric flask: 187.30 g What is the mole fraction of water? Answer to 3 decimal places.
H8.
What is the sum of coefficients from the following reaction (both products and reactants)? X.3H2O + Heat ---> X can be any element.
Convert the following measurement. - 6 7.7 x 10 kg g mol · dL mol · L
For the reaction 2A(g) s B(g) K. = 69 For the reaction A(g) = ½ B(g) Kc = For the reaction ½ B(g) A(g) Kc = Report each answer to two significant figures. Do NOT use scientific notation.
Which of the following chemical reactions is (are) classified as a decomposition reaction? A. 2NACIO3(s) 2NACI(s) + 302(g) > B. KCI(aq) + AgNO3(aq) →KNO3(aq) +AgCl(s) C. Fe(s) + CuS04(aq) FeSO4(aq) + Cu(s) D. 2NaHCO3(s) NazCO3(s) + CO2(g) + H2O(g) E. 2Fe(s) + 3C12(g) →2 FeCl3(s) A none of these B.
The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(II) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. x10 2. Suppose 75.0 mL of dioxygen gas are produced by this reaction, at a temperature of 80.0 °C and pressure of exactly 1 atm. Calculate the mass of mercury(II) oxide that must have reacted. Be sure your answer has the correct number of significant digits.
6. Write the expression for Kc for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous. a. CH4 (g) + H2S (g) → CS2(g) + H2 (g) HF + F¯ (aq) b. (aq) ⇒ H* (aq) c. Ti (s) + Cl2 (g) → TiCl4 (1) d. HCI (aq) + O2 (g) → H₂O (1) + 2 Cl2 (g)
||| O CHEMICAL REACTIONS Balancing chemical equations with interfering coefficients Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients. CH,CH, (g) + O,(g) → CO,(g) + H,O(g) X Ś
(3) A container holding NO2 and CO gas will lose NO2 gas via the reaction NO2 (g) + CO (g) → NO (g) + CO2 (g) A chemist measures the [NO2] over time and finds that plotting 1/[NO2 ] versus time yields a straight line with a slope of 3.56×10-2 M-1·s-1. If the container originally held 1.00 M NO2, what is the concentration of NO2 after 1.50 hour [NO2]1.5 hrs = ___________ How long will it take the [NO2] to drop to 20% of its initial concentration of 1.00 M? T20% = __________