Exactly 4.0 g of hydrogen gas combines with 32 g of oxygen gas according to the following reaction. 2H2 + O2 2H20 a. How many hydrogen molecules are required to completely react with 41 oxygen molecules? molecules b. If you conducted the reaction, and it produced 8.6 mol H20, how many moles of both O2 and H2 did you start with? mol O2 mol H2 c. If you started with 53.0 g O2, how many grams of H2 did you start with to have a complete reaction? d. How many grams of O2 and H2 were reacted to produce 42.6 g H20? g O2 g H2

Exactly 4.0 g of hydrogen gas combines with 32 g of oxygen gas according to the following reaction. 2H2 + O2 2H20 a. How many hydrogen molecules are required to completely react with 41 oxygen molecules? molecules b. If you conducted the reaction, and it produced 8.6 mol H20, how many moles of both O2 and H2 did you start with? mol O2 mol H2 c. If you started with 53.0 g O2, how many grams of H2 did you start with to have a complete reaction? d. How many grams of O2 and H2 were reacted to produce 42.6 g H20? g O2 g H2

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

Combustion of octane (regular gasoline): 2 C3H18 + 25 O2 → 16 CO2 + 18 H20 How many grams of CO2 are produced from burning 2.0 x 103 grams of octane. What is the first step you would take? A B Take grams of octane and divide by the molar mass of octane to get moles of octane Convert moles of octane to moles of carbon dioxide using the molar ratio Take grams of carbon dioxide and multiply by the molar mass of carbon dioxide to get moles of carbon dioxide D Take grams of octane and divide by molar mass of carbon dioxide.
12 and 13
Consider the following reaction: C3H8 + 5 02→ 3 CO2 + 4 H20 How many grams of water vapor can be produced if you begin with 70.24 g of C3H8 and 56.02 g of 02? g of H20 What is the limiting reactant: O 02 O C3H8
P4O10 + H2O → H3PO4 If 1.002mol of P4O10 is added, how much H2PO4, in grams and mol, will be produced?
Please fill in empty boxes with correct answers. Thank you very much
If 2.80 moles of H2 and 1.55 moles of O2 react how many moles of H20 can be produced in the reaction below? 2 H2(g) + O2(g) → 2 H2O(g) | mol 1 4 6. C 7 8 9. +/- х 100 LO
The following data was collected when a reaction was performed experimentally in the laboratory. Reaction Data Reactants Products Al(NO3)3 Naci NaNO3 AICI3 Starting Amount in Reaction 4 moles 9 moles ? ? Determine the maximum amount of NaNO3 that was produced during the experiment. Explain how you determined this amount.
According to the following reaction, how many moles of carbon dioxide will be formed upon the complete reaction of 0.521 moles carbon monoxidewith excess water? mol carbon dioxide
According to the following reaction, how many moles of hydrogen gas will be formed upon the complete reaction of 0.711 moles water?water (l) hydrogen (g) + oxygen (g)
SS a. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.255 mol of the first reactant were to react completely. CO₂(g) + 4H₂(g) → CH4 (g) + 2H₂O (1) mol CH₂ mol H₂O b. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.790 mol of the first reactant were to react completely. BaCl₂ (aq) + 2AgNO3(aq) → 2AgCl(s) + Ba(NO3)2 (aq) mol AgCl mol Ba(NO3)2 c. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.815 mol of the first reactant were to react completely. C3H8 (9)+502(g) → 4H₂O(1) + 3CO2(g) mol H₂O mol CO2 Submit Answer Retry Entire Group Show Hint 9 more group attempts remaining 19 Previous Next
Determine the total mass of the product that could be formed from the balanced reaction shown below if one starts with 4.20 g Al (26.98 g/mol) and 17.40 g iodine, I₂ (MW 253.80 g/mol). 2Al + 3I₂ → 2AlI₃ Set up the table below that represents 100% yield with the given reaction conditions..
5. Given the equation: Al4C3 + 12 H₂O 4 Al(OH)3 + 3 CH4 a. How many grams of water are needed to react with 100.0 moles of Al4C3? b. How many moles of Al4C3 were reacted when 3.55 x 1035 formula units of aluminum hydroxide were produced? c. How many grams of aluminum hydroxide were produced when 673. mg of CH4 were formed?