A chemist is doing a study on the utilization of sugars during sleep. According to the reaction below, when lactose (a sugar) oxidizes, it produces carbon dioxide and water. C12H22011(s) + 12 O2(g) 12 CO2(g) + 11 H2O) --> How many grams of lactose (C12H22011) are used when 0.2215 L of CO2 are produced at STP?

A chemist is doing a study on the utilization of sugars during sleep. According to the reaction below, when lactose (a sugar) oxidizes, it produces carbon dioxide and water. C12H22011(s) + 12 O2(g) 12 CO2(g) + 11 H2O) --> How many grams of lactose (C12H22011) are used when 0.2215 L of CO2 are produced at STP?

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

Enter your answer in the provided box. Sodium peroxide (Na,O2) is used to remove carbon dioxide from (and add oxygen to) the air supply in spacecrafts. It works by reacting with CO, in the air to produce sodium carbonate (Na,CO3) and 0,. 2 Na202(s) + 2 CO29) → 2 Na,CO3(s) + O2(g) What volume (in liters) of CO, can be consumed at STP by 735 g Na,02?
A gas is composed of 30.4%N and 69.6%O. Its density is 11.1 g/L at -20°C and 2.50 atm. What are the empirical and molecular formulas of the gas?
Based on the following equation, how many liters of NH3 can be produced from 15 liters of H2 at constant temperature and pressure? (use appropriate units in any conversions) N2(g) + 3H2(g) ⟶ 2NH3(g)
Nitrogen forms a surprising number of compounds with oxygen. A number of these, often given the collective symbol NOx (for "nitrogen + x oxygens") are serious contributors to air pollution. They can often be interconverted, sometimes by reaction with oxygen or ozone (O3) in the air. An atmospheric scientist decides to study the reaction between nitrogen trioxide and oxygen that produces nitrogen dioxide and ozone. He fills a stainless steel reaction chamber with 7.9atm of nitrogen trioxide gas and 1.7atm of oxygen gas and raises the temperature considerably. At equilibrium he measures the mole fraction of nitrogen dioxide to be 0.14. Calculate the pressure equilibrium constant Kp for the equilibrium between nitrogen trioxide, oxygen, nitrogen dioxide and ozone at the final temperature of the mixture. Round your answer to 2 significant digits.
Calculate the volumes of ammonia and oxygen required to produce 28 moles of nitrogen dioxide. 4NH3(g)+7O2(g)→4NO2(g)+6H2O(l)
1. Solve the following problem: a. A cooler has a 1.95kg internal steel liner. It holds 12.6L of water at 17.5°C. A 0.49kg block of ice at -5°C is placed inside. Find the equilibrium Temperature. (Ignore the steel liner, assume perfect insulation)
80.26 g LiO, is reacted with 13.00 L of CO, at STP, according to the chemical reaction shown below. Determine the percent yield if 28.00 g of Li,CO3 is produced. 4 LIO2(s) + 2 CO2(g) → 2 Li,CO3(s) + 3 O2(g) Enter your answer as a percent without units. For example, if your answer is 5.2%, enter "5.2"
The explosive, PETN, pentaerythritol tetranitrate, is one of the most powerful explosives known. It reacts with the following balanced equation: C(CH2ONO2)4(s) → 2C0(g) + 4H20(g) + 3CO2(g) + 2N2(g) 1> If 0.0250 mol of PETN reacts to fill a 30.0 L sphere at a temperature of 25 °C, what is the partial pressure of each gas and the total pressure in the flask? Pco= i atm PH20= i atm Pco2- atm PN2 atm Ptotal- atm
The following five questions refer to the same balanced chemical equation below: Sn + 4HNO3 --> Sn(NO3)4 +2H2 If you have 150. g of HNO3 and 100. g of tin, how many moles of hydrogen can you make? If you have 3.6 X 1023 atoms of tin, how many liters of hydrogen gas can you make at 1.0 atm and 25 Celsius? If you have 6.7 L of 1.5M of HNO3 solution, it will react with how many milliliters of tin (d= 5.77 g/mL)? If you made 27.7 g of hydrogen, how many grams of stannic nitrate did you also make? If you start with 2.0 mol of HNO3 and you produce 146 g of stannic nitrate, what is your percent yield?
Help me please
An experiment is performed to determine the volume of gas produced by the following reaction: 2HCl(aq) + Mg(s) MgCl2(aq) + H2(g) C. If 16mg of Mg were reacted, what is the volume of gas produced in this reaction?
1) Hexane combusts according to the following balanced equation: 2 C6H14(C) + 19 O2(g) 12 CO2(g) + 14 H2O(g) a) How many grams of H2O are produced if 10.0 L of hexane is burned at SATP? b) What is the percent yield of the reaction if 78.9 g CO2 are collected? c) What is the percent yield of the reaction if 59.9 L CO2 are collected at SATP?