Homework 4 - Weeks 8 & 9 - Formulas and States8/18 tasks attempCitric acid (CeH;O7), named for its natural occurrence in citrus fruits, is produced in large quantitiesindustrially. This is often achieved through large-scale fermentation of sucrose and/or glucose. The reactioninvolving sucrose is summarized below:C12 H22O11 +3 O22 C6H3O7 +3 H2OHow many grams of citric acid would be produced from 900.0 kg of sucrose assuming a percent yield of87.10 % ?MassHelpful tip: To enter a number in scientific notation, enter 1.0E5 or 1.0e5, for 1.0 x 105 where the E# (or e#) denotes 10SAVE RESPONSE9.101118Book ProSearch or tyne URI

% yield = ( actual mass/ theoretical mass )×100

8/18 tasks attemp Citric acid (Ce H,O-) , named for its natural occurrence in citrus fruits, is produced in large quantities industrially. This is often achieved through large-scale fermentation of sucrose and/or glucose. The reaction involving sucrose is summarized below: C12 H22O1+302 2 C,HgO7 +3 H20 How many grams of citric acid would be produced from 900.0 kg of sucrose assuming a percent yield of 87.10 % ? Mass Helpful tip: To enter a number in scientific notation, enter 1.0E5 or 1.0e5, for 1.0 x 105 where the E# (or e#) denotes 10 SAVE RESPONSE

8/18 tasks attemp Citric acid (Ce H,O-) , named for its natural occurrence in citrus fruits, is produced in large quantities industrially. This is often achieved through large-scale fermentation of sucrose and/or glucose. The reaction involving sucrose is summarized below: C12 H22O1+302 2 C,HgO7 +3 H20 How many grams of citric acid would be produced from 900.0 kg of sucrose assuming a percent yield of 87.10 % ? Mass Helpful tip: To enter a number in scientific notation, enter 1.0E5 or 1.0e5, for 1.0 x 105 where the E# (or e#) denotes 10 SAVE RESPONSE

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

Consider the combustion reaction of a hydrocarbon compound here: C2H4(g) + 302(g): 2 CO2(g) + 2 H20(g) ----> When 5.00 mol of C2H4 and 12.0 mol of O2 are added to the reactor, How many moles of CO2 can be produced by the reaction? O 4.00 mol of CO2 O 10.0 mol of CO2 O 5.00 mol of CO2 O 8.00 mol of CO2
Dimethyl ether, a useful organic solvent, is prepared in two steps. In the first step, carbon dioxide and hydrogen react to form methanol and water: CO₂(g) + 3 H₂(g) CH₂OH(1) + H₂O(1) In the second step, methanol reacts to form dimethyl ether and water: 2 CH₂OH(1)→ CH₂OCH3(g) + H₂O(1) Calculate the net change in enthalpy for the formation of one mole of dimethyl ether from carbon dioxide and hydrogen from these reactions. Round your answer to the nearest kJ. เม kJ AH=-131. kJ Ś ΔΗ= 8. kJ
If 200 kJ of heat are supplied, how many grams of NO can be produced? N2(g) + O2(g)→ 2 NO(g) AH = 180.6 kJ/mol O 66.5 g 54.2 g O 30.1 g O 2.21 g
Ethanol, C,H,O, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to burn more efficiently in combustion engines. The heat of combustion of ethanol is 326.7 kcal/mol. The heat of combustion of 2-methylheptane, C3H18, is 1.306×10³ kcal/mol. How much energy is released during the complete combustion of 482 grams of 2-methylheptane ? kcal Assuming the same efficiency, would 482 grams of ethanol provide more, less, or the same amount of energy as 482 grams of 2- methylheptane v more less the same amount
Given the reaction: 2C,H, + 70, → 4C0, + 6H,0 What is the total number of moles of CO, produced by the complete combustion of 5.0 moles of C,H,? 2.0mol 1.0mol 5.0mol O 10.mol
Consider the reaction 3X + 2Y → 5C + 4D How many moles of C can be synthesized from 37.0 moles of Y and excess X?
Asprin can be made in a laboratory by reacting acetic anhydride (C4H6O3) with salicylic acid (C7H6O3) to form asprin (C9H8O4) and acetic acid (C2H4O2). The balanced equation is: C4H6O3 + C7H6O3 ------> C9H8O4 + C2H4O2 In a laboratory synthesis, a student begins with 5.00 mL of acetic anhydride (density = 1.08 g/mL) and 2.08g of salicylic acid. Once the reaction is complete, the student collects 2.06g of asprin. Determine the percent yield for the reaction.
01 04 in the balanced equation for the complete combustion of heptane, the coefficient for carbon dioxide is: Cu + O = CO + HO W
The following unbalanced equation illustrates the overall reaction by which the body utilizes glucose to produce energy: C6H12O6(s) + O2(g) → CO2(g) + H2O(l) What is the conversion factor that allows for the calculation of moles of carbon dioxide based on moles of glucose?
esc Phosphoric acid, which is commonly used as rust inhibitor, food additive and etching agent for dental and orthopedic use, can be synthesized using a two-step thermal process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P₁(1)+50₂(g) 2 P₂O(g) In the second step, diphosphorus pentoxide and water react to form phosphoric acid: P₂O(g) + 3 H₂O(1)-2 H₂PO₂(0) 4 Write the net chemical equation for the production of phosphoric acid from phosphorus, oxygen and water. Be sure your equation is balanced. 0 Continue 56°F Clear F1 J F2 @ 2 F3 # 3 Q Search F4 $ 4 F5 % 5 F6 6 0-0 X F7 & 00 7 Ś F8 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibi M OO DELL F9 prt sc F10 home F11 end 12 F12 0 Submit Assignment J olo 18 Ar insert
2. If 550 mL of water changes temperature from 25.0°C to 28.0°C during the complete combustion of propane, determine the mass of propane that is combusted using the information in this question? C3H8(g) + 502(g) · 3CO2(g) + 4H₂O(g) + 2050 kJ