When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the product is carbon dioxide. C(s) + O₂ (g) CO₂ (g) However, when the amount of oxygen present during the burning of the carbon is restricted, carbon monoxide is more likely to result. 20 (s) + O₂(g) →→→2CO (g) Calculate the mass of product for each reaction when a 5.00 g sample of pure carbon is burned. Which reaction produces more product?

When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the product is carbon dioxide. C(s) + O₂ (g) CO₂ (g) However, when the amount of oxygen present during the burning of the carbon is restricted, carbon monoxide is more likely to result. 20 (s) + O₂(g) →→→2CO (g) Calculate the mass of product for each reaction when a 5.00 g sample of pure carbon is burned. Which reaction produces more product?

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

This question has two parts and requires two answers. Consider the reaction 4 Fe + 3 02→ 2 Fe203 a) What is the theoretical yield, in grams, of iron(III) oxide if 20.0 g of iron are mixed with 10.5 grams of oxygen gas? b) What is the limiting reactant?
When 1.547 g of sodium hydrogen carbonate (baking soda) is heated, it decomposes to 0.561 g of sodium carbonate. 2NaHCO3 (s) → Na2CO3(s) + H2O(g) + CO2(g) Use the balanced chemical equation and other given information to determine the percent yield of sodium carbonate. Molar Mass of sodium hydrogen carbonate = 84.01 g/mol Molar Mass of sodium carbonate = 105.99 g/mol
The following reaction shows the products when sulfuric acid and aluminum hydroxide react.2Al(OH)3 + 3H2SO4 → Al2(SO4)3 + 6H2OThe table shows the calculated amounts of reactants and products when the reaction was conducted in a laboratory. Initial Mass and Yield Sulfuric Acid Aluminum Hydroxide Initial Amount of Reactant 40 g 15 g Theoretical Yield of Water from Reactant 14.69 g 10.38 g What is the approximate amount of the leftover reactant? 11.73 g of sulfuric acid 10.33 g of sulfuric acid 11.12 g of aluminum hydroxide or 13.67 g of aluminum hydroxide
4 NH3(g) + 5 O2(g) -----------> 4 NO(g) + 6 H2O(g)What mass of nitric oxide can be formed from a mixture of 50.0 grams of ammonia and 50.0 grams of oxygen gas?
How many molecules of carbon monoxide (CO) are needed to react with excess iron (III) oxide (Fe₂O 2 3) to produce 11.6 g of iron (Fe)? Fe₂O₂ +3CO→2Fe + 3CO A 11.6 molecules CO FR [] U D 6.02 x 10 molecules of CO 1.88 x 10² molecules of CO 2.0 molecules CO
For the following reaction, 0.370 grams of hydrogen gas are allowed to react with 52.0 grams of iodine. hydrogen (g) + iodine (s) →→→→→→ hydrogen iodide (g) What is the maximum amount of hydrogen iodide that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams grams
Chapter 4 Limiting reactants
When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: CH4 (g) + CCI4 (g) →→→ CH₂Cl₂ (g)
39.06 g C6H6) + (120.00 g O2) ------------> (132.03 g CO2) + (x g H2O) Assuming that both reactants are completely used up, calculate the numerical value of x. Place your answer in the box
For the following reaction, give the balanced equation for the reaction. Consider the following unbalanced equation: NH3(g) → N2(g) + H2(g) How many moles of N2 will be produced by the decomposition of 3.08 moles of ammonia? What information do we need to find how many moles of N2 will be produced?
Consider the following unbalanced chemical reaction: Al (s) + HCI (g) → AICI3 (g) + H2 (g) 1. Balance the chemical equation 2. How many moles of aluminum metal are needed to produce 3.33 moles of aluminum chloride? 3. Calculate the mass of aluminum metal (g) needed to produce 3.33 moles of aluminum chloride.
Which formula can be used to calculate the percent yield? (Theoretical yield + actual yield) x 100 O (Actual yield + theoretical yield) x 100 (Amount of reactants + amount of products) x 100 O (Amount of products + amount of reactants) × 100