A sample of 0.250 mole of O, is added to the 5.10 g of O, in the container. Express the volume in liters to three significant figures. A sample of 2.35 g of O2 is removed from the 5.10 g of O2 in the container. Express the volume in liters to three significant figures. ΑΣφ V' = Submit Request Answer Part C A sample of 3.80 g of O2 is added to the 5.10 g of O2 gas in the container. Express the volume in liters to three significant figures.

A sample of 0.250 mole of O, is added to the 5.10 g of O, in the container. Express the volume in liters to three significant figures. A sample of 2.35 g of O2 is removed from the 5.10 g of O2 in the container. Express the volume in liters to three significant figures. ΑΣφ V' = Submit Request Answer Part C A sample of 3.80 g of O2 is added to the 5.10 g of O2 gas in the container. Express the volume in liters to three significant figures.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter3: Molecules, Moles, And Chemical Equations

Section: Chapter Questions

Problem 3.37PAE: 3.37 If atypical grain of sand occupies a volume of 1.3 × 10-4 cm3, what is the volume (in cm3) of 1...

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3.37 If atypical grain of sand occupies a volume of 1.3 × 10-4 cm3, what is the volume (in cm3) of 1 mole of sand (ignoring the space between grains)? What is the volume in liters?
In a clean and dry crucible with cover weighing 24.342 g some of the unknown hydrate (CuSO4.nH2O) was placed in the crucible to reach a mass of 27.557 g. The crucible was heated several times until it reached a final constant mass of 26.403 g. Use these measurements to complete your data sheet and show complete calculation for the missing values.
Given:AmmoniaDensity of Ammonia: 0.73 kg/m³Atomic Weights: H=1; C=12 ; N=14 ; O=16 ; Na=23 ; P=31; Cl=35 1. What is the density (in g/ml) of the given compound? Present your answer in decimal without rounding off your answer. 2. What is the appropriate state of matter of the given compound? 3. What is the chemical formula of the given compound? 4. What is the molecular weight of the given compound (using the given atomic weights)? 5. What is the molar volume (L/mol) of the given compound? i need help please
A beaker contains 100.0 mL of water. To it is added 10.0 mL of dilute nitric acid (HNO3). Calculate the total moles of water in the beaker after the acid is added. (Assume the density of the nitric acid is the same as that of water.) Density of water= 1.00 g/mL
1) a. Amixture contains 34.5 g of copper, 18.4 g of lead and 12.3 g of silver. State the percentage, by mass,of each type of metalin the mixture and create a variety of conversion factors using them. b. Calculate the mass, in grams, of silver in a 3.04 X 102g sample of this mixture. 2) A sample of clean air is found to contain 20.45% oxygen gas by volume. How many liters of oxygen gas are present in a 65.0 μL sample of this air? 3) A 500.0 mg pill (i.e. 500 mg/ 1 pill) contains 2.7% by mass of the active ingredient. How many g of the active ingredient would be present in 12 pills? 4) A sunscreen preparation with a density of 2.82 g/mL contains 3.55% by mass zinc oxide (ZnO). Each tube is filled with 185.0 mL of sunscreen (i.e. 185.0 mL/tube).If you are the manufacturer and you use 5.00 lb of ZnO, how many full tubes of the sunscreen would you prepare?
a) For 8.85×10−3 M LiOH, determine [OH−] and [H3O+]. Express your answers in moles per liter to two significant figures separated by a comma. b) For 1.11×10−2 M Ba(OH)2, determine [OH−] and [H3O+]. Express your answers in moles per liter to two significant figures separated by a comma. c) For 2.2×10−4 M KOH, determine [OH−] and [H3O+]. Express your answers in moles per liter to two significant figures separated by a comma. d) For 5.1×10−4 M Ca(OH)2, determine [OH−] and [H3O+]. Express your answers in moles per liter to two significant figures separated by a comma.
Given: wt NaOH = 10.0g Density of NaOH= 2.16 g/ml Wt. H2O = 200g Density of H2O= 1g/ml Calculate N
A researcher is using 7.20 x 1023 molecules of chlorine gas (Cl2) in an experiment. How many grams of chlorine is the researcher using? Remember to include units (abbreviated appropriately) and the substance in your answer. Round your answer to the nearest 0.01.
Given the following data for Mass of test tube and stearic acid = 14.17 gMass of test tube = 11.40 gFreezing point of strearic acid = 69.59o CMass of weighing paper + naphthalene =1.230 gMass of weighing paper = 0.920 gFreezing point solution = 64.00o CKf = 4.5o C/m Determine the following1. mass of stearic acid in g (2 decimal places); 2.77g2. mass of naphthalene in g (2 decimal places); 0.31g3. freezing point depression (2 decimal places); 3.93oC4. molality of solution (3 significant figures); _____5. moles of naphthalene (3 significant figures); _____6. molar mass of naphthalene, experimentally (3 significant figures); _____7. % error if theoretical molar mass of naphthalene is 128.17 g/ mole, USE ABSOLUTE VALUE (3 significant figure); _____
Methanol (CH4O) has a density of 0.791 gmLgmL and a molar mass of 32.05 gmolgmol. How many moles of methanol are in a 0.834 mL (milliliter) sample of methanol? Report your answer rounded to the proper number of significant figures.
) A 1 gallon bottle of a certain brand of bleach costs $1.49. Determine the cost to buy enough bleach to supply 100.0 grams of active ingredient (NaOCl), assuming 6.25% active ingredient by mass and a density of 1.05 g/ml.
(atk) Complete all calculations using the appropriate number of sigfigs 1) (4.184 Jg⋅∘C)(50.0 g)/(67.34 ∘C−24.56 ∘C) = ___ (J) 2) 2.385 g−1.978 g/2.385 g×100% = ___ (%) 3) e0.856(4.69 × 10−7) = ___ (M−1s−1) 4) 112.99 minutes to days

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