**Educational Website Text**---### Determining Mass from MolesIn this exercise, you will calculate the mass of various chemical compounds given their mole quantity. Use the molar mass of each compound to determine the answer.#### Questions:a. **What mass is represented by 0.0146 mol of \( \text{C}_3\text{H}_7\text{OH} \) (2-propanol, rubbing alcohol)?** - **Mass =** _____ gb. **What mass is represented by 0.0146 mol of \( \text{C}_{11}\text{H}_{16}\text{O}_2 \) (an antioxidant in foods, also known as BHA or butylated hydroxyanisole)?** - **Mass =** _____ gc. **What mass is represented by 0.0146 mol of \( \text{C}_9\text{H}_8\text{O}_4 \) (aspirin)?** - **Mass =** _____ gd. **What mass is represented by 0.0146 mol of \( (\text{CH}_3)_2\text{CO} \) (acetone, an important industrial solvent)?** - **Mass =** _____ g---#### Instructions:Complete the calculations and input your answers in the provided fields. Each question requires you to apply the formula mass = moles × molar mass. You have 8 attempts remaining for the group of questions. Click **Submit Answer** once you have filled all answers.---**Note:** Make sure to refer to the periodic table for accurate molar mass values.**Website Interface:**- **Submit Answer**- **Retry Entire Group**- **8 more group attempts remaining****End of Text**---

a). Given: The moles of C3H7OH = 0.0146 mol. The molar mass of C3H7OH = 60.09 g/mol.

a. What mass is represented by 0.0146 mol of C3H7OH (2-propanol, rubbing alcohol)? Mass %3D b. What mass is represented by 0.0146 mol of C11H16O2 (an antioxidant in foods, also known as BHA or butylated hydroxyanisole)? Mass = c. What mass is represented by 0.0146 mol of C9H3O4 (aspirin)? Mass d. What mass is represented by 0.0146 mol of (CH3)2CO (acetone, an important industrial solvent)? Mass g I more groun attempts remaining

a. What mass is represented by 0.0146 mol of C3H7OH (2-propanol, rubbing alcohol)? Mass %3D b. What mass is represented by 0.0146 mol of C11H16O2 (an antioxidant in foods, also known as BHA or butylated hydroxyanisole)? Mass = c. What mass is represented by 0.0146 mol of C9H3O4 (aspirin)? Mass d. What mass is represented by 0.0146 mol of (CH3)2CO (acetone, an important industrial solvent)? Mass g I more groun attempts remaining

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

Please help with question 3 a-c
6. A compound contains C, H, and I. Burning 18.42 g of this compound produced 0.42 g H20. Treatment of 13.27 g of the compound with excess AGNO, produced 23.75 g of Agl. What is its empirical formula?
part 1 of 9 Balance the cquation NH3 + O2 + N2 + H2O Given 1.25 mol of the reactant NH3, deter- mine the corresponding amount of O2. Answer in units of mol. part 2 of 9 Find the corresponding amount of N2. Answer in units of mol. part 3 of 9 Find the corresponding amount of H2O. Answer in units of mol. part 4 of 9 Given 4.17 mol of the product N2, find the corresponding amount of NH3. Answer in units of mol. part 5 of 9 Find the corresponding amount of O2. Answer in units of mol. part 6 of 9 Find the corresponding amount of H2O. Answer in units of mol. part 7 of 9 Given 4.19 mol of the reactant O2, find the corresponding amount of NH3. Answer in units of mol. part 8 of 9 Find the corresponding amount of N2. Answer in units of mol. part 9 of 9 Find the corresponding amount of H2O. Answer in units of mol.
Calculate the molar mass of the following substances. Molar Mass = C b. Mg3(PO4)2 Molar Mass = c. Na₂HPO4 Molar Mass P g/mol g/mol g/mol
2.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 160. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 3.30 g water 0.90 g Use this information to find the molecular formula of X.
Please don't provide hand written solution
4)_ _Snoz +_H; >. Sn + H20 3.912 g of Sn0, form how many grams Sn?
What is the elements, atomic mass, number of atoms, subtotal and composition? 1. Compound: C8H10N4O2 2. Compound: CuSO4 * 5 H2O
3. What is the reaction that corresponds to AH; for chloric acid, HC1O3(aq)? a. ClO, (aq) + H*(aq) b. HCIO3(aq) + H2O(1) c. H(g) + Cl(g) + 3 0(g) d. ½ H2(g) + ½ Cl2(g) + ¾O2(g) e. H2(aq) + Cl2(aq) +3 O2(aq) → 2 HCIO3(aq) 0-257 HCIO<(aq) mi dod ClO, (aq) + H30*(aq) HCIO3(aq)tiwollot ordt lo e0o doifW HCIO3(aq) 4. A 0.218 g sample of ethanol (molar mass: 46.07 g/mol) is burned in a constant-volume calorimeter (i.e. bomb calorimeter). If the temperature of the calorimeter rises from 25.13°C to 28.86°C, determine the heat capacity of the calorimeter. The enthalpy of combustion of ethanol is -1235 kJ mol-l. giue lolain ofT giua loubin orts uslh oatstogaet fead torigid s ovsd b. 3.33 J/Kh tud gina blog adi asdi gono ord eon dhoeria lliw gide loxoin odi giua blog arl Nor ovom dioeda a. 1.57 kJ/K c. 7.00 J/K d. 21.1 J/K of he e. 21.8 kJ/K agaibnuomua ors motaya s of bonotanst ei vgon9 5. The amount of heat energy released when zinc metal reacts with hydrochloric acid: Zn(s) + HCl(aq) →…
An impure sample of table salt (NaCl) that was dissolved in water and treated with silver nitrate to form silver chloride. If the initial sample had a mass of 1.741 g and the final mass of the AgCl was found to be 4.084 g, what is the mass percent of NaCl in the impure sample?
Which element has the largest mass % in alcohol CH3CH₂OH? (Hint: calculate the "mass" of each atom, C, H, O, in the compound) All three elements are the same! H O
3. An organic compound was found to contain 54.5% C, 9.2% H, and 36.3% O. a. What is the empirical formula of the compound? b. If the molar mass of the compound is 88.1 g/mol. What is the molecular formula? Note. Refer to your periodic table for the atomuc mass/mass number in whole number. For the final answer, in case of decimals, round off into two decimal places.