**Question:**How many oxygen atoms are present in 3.20 g of Al₂(SO₄)₃? Express your answer in scientific notation like this: 6.02*10^23.**Solution:**To find the number of oxygen atoms in 3.20 grams of Al₂(SO₄)₃ (aluminum sulfate), follow these steps:1. **Calculate the molar mass of Al₂(SO₄)₃:** - Atomic mass of Aluminum (Al): approximately 27.0 g/mol - Atomic mass of Sulfur (S): approximately 32.1 g/mol - Atomic mass of Oxygen (O): approximately 16.0 g/mol Therefore, the molar mass of Al₂(SO₄)₃ is: \[ 2(27.0) + 3[(32.1) + 4(16.0)] = 2(27.0) + 3(32.1 + 64.0) = 54.0 + 3(96.1) = 54.0 + 288.3 = 342.3 \text{ g/mol} \]2. **Convert grams to moles:** \[ \text{Moles of } \text{Al₂(SO₄)₃} = \frac{3.20 \text{ g}}{342.3 \text{ g/mol}} = 0.00935 \text{ moles} \]3. **Calculate the number of oxygen atoms in one mole of Al₂(SO₄)₃:** - There are 4 oxygen atoms per sulfate ion (SO₄), and there are 3 sulfate ions in each formula unit of Al₂(SO₄)₃. - Total oxygen atoms: \( 4 \times 3 = 12 \) Therefore, in 0.00935 moles of Al₂(SO₄)₃: \[ 0.00935 \text{ moles} \times 12 \text{ oxygen atoms per mole} = 0.1122 \text{ moles of oxygen atoms} \]4. **Convert moles of oxygen atoms to number of atoms:** Using Avogadro’s number \(6.

The number of moles of a substance is calculated by dividing the given mass of that substance by its…

Answered: How many oxygen atoms are present in…

How many oxygen atoms are present in 3.20 g of Al2(SO4)3? Express your answer in scientific notation like this: 6.02*10^23

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

You have 2.97 × 10^25 molecules of water. Find the volume of this in milliliters. Water has a molar mass of 18.01528 grams per mole and a density of 1 gram per milliliter. Avogadro's number is always 6.022 × 10^23 molecules per mole. Round to two decimal places.
3 Cu + 8HNO3 → 3 Cu(NO3)2 + 2 NO + 4 H₂O In the above equation, how many grams of water can be made when 7.9 moles of HNO3 are consumed? Round your answer to the nearest tenth. If you answer is a whole number like 4, report the answer as 4.0 Use the following molar masses. If you do not use these masses, the computer will mark your answer incorrect.: Molar Element Mass Hydrogen 1 Nitrogen 14 Copper 63.5 Oxygen 16
Answer the following questions regarding this chemical reaction: Cu(s) + HNO3(aq) --> Cu(NO3)2(aq) + H2O(l) + NO2(g) c. If you want to produce 100.0 g of Cu(NO3)2, how much volume of HNO3 is needed? Density of HNO3 is 1.51 g/cm3. Give your answer in mL. Use the correct number of significant figures.
Part a) Mr. Scholl likes to grow tomatoes in his backyard garden. Last year he grew a 6.27 × 10 to the power of -10 moles of tomatoes. How many tomatoes did he grow? Part b)The Waterloo Region has about 617,000 people in it. If Mr. Scholl divides his tomatoes equally among everyone in Waterloo Region, how many tomatoes will you personally receive (assuming you live in the Waterloo Region.)
Calculate the mass (in grams) of 4.54 × 1020 molecules of hydroxychloroquine, C18H26ClN3O. Report your answer to 4 decimal places.
What is the mass (in grams) of 3.2 x 1021 molecules of ibuprofen (C13H1802; molar mass 206.3 g/mol)? Only report the numeric value of your answer, not the units (grams).
A chemist adds 160.0mL of a ×6.510−5μM silver(II) oxide AgO solution to a reaction flask. Calculate the mass in micrograms of silver(II) oxide the chemist has added to the flask. Round your answer to 2 significant digits.
A student performed a similar experiment to the one you performed: They took a crucible and lid, cleaned them, heated them over a flame, and after cooling found their combined mass to be 22.538 g. The student then added a sample of zinc(II) sulfate hydrate (ZnSO4·“n”H2O) to the crucible so the combined mass of the sample, crucible, and lid was 25.896 g. They heated this sample for 10 minutes with the lid ajar, let it cool, and measured the mass of the crucible, sample, and lid to be 25.054 g. a. Based on this experiment, what is the formula for they hydrated zinc(II) sulfate compound? b. The student later looked on the reagent bottle for zinc(II) sulfate hydrate and found the actual formula was ZnSO4·7H2O. If everything had been done correctly, what value should the student have expected for the final mass of their sample, crucible, and lid after heating?
O Chemical Reactions Balancing chemical equations with interfering coefficients Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients. CH,(CH,) CH,(g) +O,(g) → CO,(g) + H,O(g) 2 X Ś
Starting with 8.39 X 1018 grams of HCIO4, how many molecules of Cl207 can you make? 12 HCIO, + P,O10 = 4 H3 PO4 + 6 Cl207 Round your answer to 2 decimal places and, if needed, enter scientific notation like this 6.02e23 (would mean 6.02 x 1023.)
The mole is a counting number that allows scientists to describe how individual molecules and atomsreact. If one mole of atoms or molecules is equal to 6.022 × 1023 atoms or molecules, how many moleculesare in a 23.45 g sample of copper (II) hydroxide, Cu(OH)2? (MM of Cu(OH)2 is 97.562 g/mol) Expressyour answer to the correct number of significant figures and you must show all work in the form ofdimensional analysis as shown in Lesson 4. You must solve the problems as they are taught in the course. 4.2 Counting particles of matter. Grams to moles of Copper Hydroxide to molecules of Copper Hydroxide.