Answered: H2O + CO2 ---> C2H12O6 + O2 How many…

H2O + CO2 ---> C2H12O6 + O2 How many moles of CO2 are needed to make 0.065 mol oxygen? Be sure your answer has a correct unit symbol if applicable, and round to correct number of significant digits.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter5: Gases

Section: Chapter Questions

Problem 25QAP: Cyclopropane mixed in the proper ratio with oxygen can be used as an anesthetic. At 755 mm Hg and...

See similar textbooks

Related questions

Q: sample of the unknown compound was placed in a weighed drying pan and heated to give the data below.…

A: Given that the experimental data: Mass of the drying pan m1= 1.445 g Mass of drying pan and…

Q: Ammonium perchlorate NH4ClO4 is the solid rocket fuel used by the U.S. Space Shuttle. It reacts…

A: Mole is the amount of the substance that contains the same number of particles or atoms or…

Q: What is the coefficient in front of the O2 when the equation below is balanced (using only whole…

A: Balanced equation :- A chemical equation is said to be balanced if the number of atoms of different…

Q: In the air we breathe at 74.0 ∘F∘F and 1.09 atmatm pressure, how many molecules does a typical cubic…

Q: Chemistry (1= T15HW Question 5 Homework Unanswered O Determine the percent by mass of both magnesium…

Q: Be sure to answer all parts Hew many moles of cobalt (Ce) stoms are there la 2.00 x 10 (200 hillion)…

A: Given, Number of Co atom = 2.00×10^9 Avogadro's no. = NA= 6.023×10^23

Q: The bitter-tasting compound quinine is a component of tonic water and is used as a protection…

Q: How many carbon atoms are present in 0.200 mol of C2H4? Please express the answer in scientific…

A: We know that 1 mol Carbon atom = 6.022×1023 atoms of carbon

Q: 2. a. What is the mass of one mole of caffeine (C8H10N4O2)? Show your work. Box your final answer.…

A: We know, molar mass of : C = 12.01 g/mol , H = 1.007 g/mol , N = 14.007 g/mol , O = 16.00 g/mol The…

Q: How many formula units are in 6.6 grams of Si? Si=28.09

A: The given information is as follows: The mass of Si = 6.6 grams The atomic mass of Si = 28.09 g/mol…

Q: What is the empirical formula for C10H2005 ?

A: Empirical formula of a compound = Formula of a compound written with the smallest integer subscript.…

Q: The bitter-tasting compound quinine is a component of tonic water and is used as a protection…

A: Data given: Mass of the sample = 0.487 g Mass of carbon dioxide produced = 1.321 g Mass of water…

Q: Calculate the number of moles in each of the following Part B 0.231 g of C Express your answer with…

A: Given that, Part-B: 0.231 g Carbon (C) We have to calculate the number of moles of carbon (C).…

Q: How many moles of Al atoms are present in 5.96 · 1018 Al(ClO3)3●6H2O formula units? Express your…

Q: Assume that the ratio of moles of Cl to moles of Cu are 2.7. If we can represent the formula by…

Q: Inbox ← → C www. Apps Aktiv Chemistry X OneLogin + X app.101edu.co Time's Up! An unknown compound is…

Q: Hexane, C6H14, is known to have a density of 0.655 g/mL at room temperature. How many moles would…

Q: 12- I. 96 grams of O2 gas II. 44.8 liters of Oz gas in NK III. 9,1023 O molecules Which of the…

Q: 5. Empirical formula for C4Hsl4N2 Is. a) CH2IN b) C2H42N c) C2H2LN2 d) none of all

A: Empirical formula is the simplest whole number ratio of atoms present in a compound. Where as the…

Q: Hilfur oxide is 50.0% by mass sulfur. This empirical formula could be For the toolbar, press ALT+F10…

A: Given: Weight % of sulphur in sulphur dioxide = 50 % Empirical formula is the chemical formula…

Q: A pure sample of an organic molecule has the formula CxHyOz. If x = 10, y = 22, and z = 2. Calculate…

A: • The formula of a pure sample of an organic molecule is CxHyOz •Since, the value of x = 10, y…

Q: Find the percent, by weight, of each component.

Q: Calculate the number of nitrogen atoms in a 100.0 g sample of hydrazine (N,H). Be sure your answer…

A: 1 mol of a molecule contains Avogadro number of molecules. Avogadro number = 6.022×1023

Q: Calculate the number of nitrogen atoms in a 90.0 g sample of hydrazine (N,H,). Be sure your answer…

A: The number of moles is calculated using following equation: number of moles=given mass molar mass…

Q: Calculate the number of phosphorus atoms in a 130.0 g sample of diphosphorus pentoxide (P,05). Be…

A: Diphosphorus pentoxide (P2O5) is an oxide of phosphorous that has 2 atoms of phosphorous and 5 atoms…

Q: Match each of the following with its correct answer The empirical formula of a compound is CH. If…

Q: Combustion of a compound of formula CyH,O, yields 6.25g H20 and 20.4g CO2 when 16.7g of O2 is used.…

A: Given data : Mass of CO2= 20.4 g Mass of H2O = 6.25 g Mass of O2 used = 16.7 g

Q: 12. The mass in grams of 10.0 million molecules of sulphur dioxide is: SO2 Answers: a)1.06…

A: 1 mole = 6.022×1023 ( Avogadro's number ) Molar mass : The mass of one mole of molecules of a…

Q: How do you calculate the number of moles in each sample? Express answer with appropriate units…

A: The relation between mole and mass of any substance is given as - Mole = mass /molar mass

Q: Pre-Lab Questions "Counting by weighing" is used in other applications besides chemistry. A hardware…

A: Given, Hardware sells nails in package of 500. Office supply store sells 100 paper clips.

Q: High fructose corn syrup (HFCS) is a sweetener that was designed in the 1970s, which takes corn…

A: Given, Amount of HFCS used = 67.5 g Percentage of fructose molecules =55.1 % Percentage of glucose…

Q: Calculate the moles of anhydrous (dry) KAl(SO4)2 that were present in the sample. Show all work to…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: Given the following equation: N2 + 3H2 --> 2NH3, write the following molar ratio for N2 to NH3 O a)…

A: The balanced Chemical equation given in the question is - N2 + 3H2 -----> 2NH3 Here, in the…

Q: The following data were obtained when a hydrate was heated 31.781 g crucible+ sample 30.501 g empty…

A: The mass of sample is calculated as,

Q: Calculate the number of vanadium atoms in a 80.0 g sample of vanadium(V) oxide (V,O5). Be sure your…

A: here we are required to find the number of vanadium atoms in 80g sample of Vanadium oxide using…

Q: 4. Determine the number of molecules of compounds or atoms for the following. 15.8 mol H20 9.51 x10…

A: Mole concept: The number of molecules or atoms present in the one mole of the substance is equal to…

Q: CS2 Express your answer in moles. ? mole Submit Previous Answers Request Answer X Incorrect; Try…

A: To calculate the number of moles in 5.00 g of each of the following: CS2 Ca3N2

Q: What mass of chlorine gas is produced by the reaction of 7.5g of ammonium perchlorate?

A: Given :- mass of NH4ClO4 = 7.5 g To calculate :- mass of Cl2 (in grams)

Q: • Sodium metal reacts with hydrogen to form sodium hydride (NaH) 2Na + H2---- 2 NaH If 10 grams of…

A: Given reaction --- 2Na + H2 ----> 2NaH mass of Na =10 g, mass of H2= 8 g moles of NaH = ?…

Q: 4. What is the percentage of water in the hydrate? mass of water in sample X 100 44.8% H,0 % water =…

A: The mass of water in a sample is 0.729 g. The mass of hydrate sample is 1.628 g.

Q: Determine the percentage by mass of each element in the following compounds. (Round your answers to…

A: Mass percent of an element:

Q: O STOICHIOMETRY Using the Avogadro Number An oxygen atom has a mass of 2.66 x 10 - 23 g and a glass…

A: We are given mass of one atom and we have to calculate mass of one mole and hence calculate how many…

Q: Calculate the moles of C2H6 in 3.76x1023 molecules of C2 H6. Express your answer using three…

A: Interpretation- To determine the number of moles of C2H6 in 3.76× 1023 molecules of C2H6 -…

Q: Calculate the moles of anhydrous (dry) KAl(SO4)2 that were present in the sample. Show all work to…

A: Since you have posted a question with multiple sub-parts, we will solve the first three subparts for…

Q: Aluminum hydroxide is used as a deodorant and sometimes an antacid (something that prevents acid…

Q: Aluminum has a density of 2.70 g/cm^3. How many moles of aluminum are in a 13.2 cm^3 block of the…

A: Given, Density of Aluminium = 2.70 g/cm3 Volume = 13.2 cm3

Q: For items 1 and 2: 4NH3 + 302 6H2O + 2N2 1. What is the mole ratio of NH3 to H2O? 2. What is the…

Q: Calculate the moles of ammonium phosphate produced by the reaction of 1.9mol of phosphoric acid.…

A: Given values - Mole of H3PO4 = 1.9 mole

Q: A pure sample of an organic molecule has the formula CxHyOz. If x = 11, y = 13, and z = 2. Calculate…

A: The molecular formula of the given compound is CxHyOzthat is C11H13O2.

Q: The following represents an empirical formula. a. C6H12O6 b. C3H6O3 c. CH2O d. C2H2 e. S2O4

Question

H₂O + CO₂ ---> C₂H₁₂O₆ + O₂

How many moles of CO₂ are needed to make 0.065 mol oxygen?

Be sure your answer has a correct unit symbol if applicable, and round to correct number of significant digits.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react gas X with gas Y to make the products, you get the following data (all at the same pressure and temperature): 1 volume gas X + 2 volumes gas Y 2 volumes compound I 2 volumes gas X + 1 volume gas Y 2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.
You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react gas X with gas Y to make the products, you get the following data (all at the same pressure and temperature): 1. volume gas X + 2 volumes gas Y2 volumes compound I 2. volumes gas X + 1 volume gas Y2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.
How many moles are there in 572.6 g of Na 2 SO 4 ? Answer to 2 decimal places and give the unit .
In the air we breathe at 74.0 ∘F∘F and 1.09 atmatm pressure, how many molecules does a typical cubic centimeter contain, assuming that the air is all N2N2. N= ---------- molecules
What is the mass of 2.41 moles of AgN*O_{3} ? Write your answer to 2 decimal places and include the unit.
Calculate the number of nitrogen atoms in a 150.0g sample of hydrazine N2H4. Be sure your answer has a unit symbol if necessary, and round it to 4significant digits.
Calculate the mass percentage composition of aluminum in the compound AL(NO3)3. Please report the answer with three significant digits.
The empirical formula for C6H12 is-
6.35 x10 to the 22nd power molecules of H2SO4 then how many grams of H
Vitamin C has a formula of C6H8O6, calculate the number of vitamin molecules present in a 0.250g of pure vitamin C
You wish to prepare 213 grams of 17.4% (w/w) NaI. Assume that the density of water is 1.00 g/mL. You will need grams of sodium iodide and mL of water.
General formula of a polymer is-(CH2CHCHCN)n-, where n is typically greater than 10,000. Then take a sample of this polymer weighs 755.9 g and contains 3.112 x 1020 molecules of -(CH2CHCHCN)n-, so calculate n?