5. Part AThe forensic technician at a crime scene has just prepared a luminol stock solution by adding 20.0 g of luminol intoa total volume of 75.0 mL of H,0.What is the molarity of the stock solution of luminol?Express your answer with the appropriate units.• View Available Hint(s)?HAmolarity of luminol solution =1.505mSubmitPrevious AnswersX Incorrect; Try Again; 5 attempts remaining Before investigating the scene, the technician must dilute the luminol solution to a concentration of 5.00x10-2 MThe diluted solution is then placed in a spray bottle for application on the desired surfaces.How many moles of luminol are present in 2.00L of the diluted spray?Exprêss your answer with the appropriate units.• View Available Hint(s)HA?12 10 2moles of luminol =molSubmitPrevious AnswersX Incorrect; Try Again; 9 attempts remaining

Answered: Image /qna-images/answer/3e82097e-010c-4452-ba46-f87a2eb1d793.jpg

Part A The forensic technician at a crime scene has just prepared a luminol stock solution by adding 20.0 g of luminol into a total volume of 75.0 mL of H20. What is the molarity of the stock solution of luminol? Express your answer with the appropriate units. > View Available Hint(s) HA molarity of luminol solution = 1.505 m

Part A The forensic technician at a crime scene has just prepared a luminol stock solution by adding 20.0 g of luminol into a total volume of 75.0 mL of H20. What is the molarity of the stock solution of luminol? Express your answer with the appropriate units. > View Available Hint(s) HA molarity of luminol solution = 1.505 m

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

(5.5, 5.7 & 5.8) Classify the following reaction. Ba(NO3)2(aq) + K₂SO4(aq) --> O acid-base reaction O gas-forming reaction O decomposition reaction O precipitation reaction
8.8
6. 7 8. 9. 10 11 12 13 14 A chemist prepares a solution of potassium iodide (KI) by measuring out 3.0 × 10“ umol of potassium iodide into a 350. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in umol/L of the chemist's potassium iodide solution. Round your answer to 2 significant digits. alo Ar μ mol x10 Submit Assignment Continue 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center | Accessibility Show All IMG-4472.jpg IMG-4471.jpg IMG-4467.jpg IMG-4464.jpg IMG-4474.jpg MacBook Air DII F12 80 F9 F10 F11 F7 F8 F5 F6 F3 F4 F2 %23 $ 4 5 6 7 8 9 3 P 4.
If an automobile travels 225 mi with a gas mileage of 20.5mi / gal,how many kilograms of CO{2} are produced? As- sume that the gasoline is composed of octane, C8H18(l) whose density is 0.69g / mL (b) Repeat the calculation for a truck that has a gas mileage of 5mi /gal
49.62 kcal into joules
CS2 6.61 Phosphoric acid, H,PO4, can be prepared by the reac- tion of phosphorus(V) oxide, P4O10, with water. P,O10(s) +H,O(1) → H,PO.(ag); AH = -96.2 kl What is AH for the reaction involving 1 mol of P4O10- %3D P,O 10(s) + 6H,O(I) 4H;PO,(aq)
1:39 1 Send a chat Enter your answer in the provided box. Hydrogen fluoride is used in the manufacture of Freons (which destroy ozone in the stratosphere) and in the production of aluminum metal. It is prepared by the reaction CaF2 + H2SO4 → CASO4 + 2HF In one process, 5.75 kg of CaF, is treated with an excess of H,SO, and yields 2.45 kg of HF. Calculate the percent yield of HF. % yield
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(11) 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(11) oxide (HgO) into liquid mercury and gaseous dioxygen. 2. Suppose 39.0 mL of dioxygen gas are produced by this reaction, at a temperature of 50.0 °C and pressure of exactly 1 atm, Calculate the mass of mercury(11) oxide that must have reacted. Round your answer to 3 significant digits. 0. 0-0 X
(2) 8. Write the balanced equation for the neutralization reaction between HI and Ba(OH)2 in aqueous solution. Include phases (physical states) in your equation. Use the arrow, not "=".
10) The number 0Aunpcired dectrans opected kr the Compler icn: ColoH)is: +
1. LIAI Hy, THE 9. 2.