**How to Calculate the Production of Oxygen Gas in a Chemical Reaction**In this section, we will explore a stoichiometry problem involving a chemical reaction. The goal is to determine how many grams of oxygen gas (O₂) are produced when 2.43 × 10⁻⁴ grams of potassium chlorate (KClO₃) are fully reacted.### Chemical EquationThe balanced chemical equation for the decomposition of potassium chlorate is:\[ 2 \text{KClO}_3 (s) \rightarrow 2 \text{KCl} (s) + 3 \text{O}_2 (g) \]### Problem Overview- **Given:** 2.43 × 10⁻⁴ grams of KClO₃- **Find:** Grams of O₂ produced### Calculation SetupThe interface provides boxes for entering the starting amount and various stoichiometric factors. Below are detailed steps to follow:1. Enter the starting amount of KClO₃ (2.43 × 10⁻⁴ g) in the "STARTING AMOUNT" box.2. Use the stoichiometric coefficients from the balanced equation to set up conversion factors that link moles of KClO₃ to moles of O₂.3. The molar masses needed for the conversion are: - KClO₃ = 122.55 g/mol - O₂ = 32.00 g/mol### Input Controls- **ADD FACTOR:** Add conversion factors such as the molar mass or mole ratio.- **ANSWER:** Calculate or reset to input new values.- **RESET:** Clear all input fields.### Key Concepts- **Stoichiometry:** Using mole ratios for converting between reactants and products.- **Molar Mass:** Molecular weight necessary for translating between grams and moles.By following these steps, you can accurately calculate how much oxygen is produced from a given amount of KClO₃ in this chemical reaction.

Stoichiometry involves the calculation of concentration of solutions in the given conditions of…

Answered: How many grams of oxygen gas are…

How many grams of oxygen gas are produced when 2.43 x 10-g of KCIO: are completely reacted according to the following chemical equation: 2 KCIO:(s) – 2 KC(s) + 3 o:(g)

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

A sample of 108.2 g of Calcium oxide was obtained by heating 258 g of calcium carbonate. What is the percent yield for this reaction? CaCO3(s) ⟶ CaO(s) + CO2(s)
An intermediate step in the industrial production of nitric acid, HNO3, involves the reaction of ammonia, NH3, with oxygen gas, O2, to form nitrogen monoxide, NO, and water, H2O. 4 NH3 (g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) Molar masses (g mol-1) NH3 = 17.03 O2 = 32.00 NO = 30.01 H2O = 18.02 (a) Assuming excess O2, how many grams of nitrogen monoxide, NO, (i.e., the theoretical yield of NO) can be formed by the reaction of 46.00 g of ammonia, NH3 b. Assuming excess NH3, what is the theoretical yield of NO if we start with 73.00 grams of O2? c.If we start with 8.0 moles of NH3 and 8.0 moles of O2, how many moles of NO will we produce? d. If we have 36.00 g of NH3 and 72.00 g of O2, what is the theoretical yield of NO
For the reaction shown, calculate how many moles of each product form when the given amount of each reactant completely reacts. Assume that there is more than enough of the other reactant. C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) 1. 0.0558 molO2, v=?molCO2 2. 0.0558 molO2, v= ?molH2O
Given the equation: 4 NH3 + 7 O2 ----> 4 NO2 + 6 H2O (a) How many moles of NH3 must react if 24.8 moles of water are produced? (b) Determine the number of moles of H2O that would be formed from the combustion of86.0 grams of NH3.
For the following reaction, 5.82 grams of water are mixed with excess chlorine gas. The reaction yields 14.0 grams of hydrochloric acid. chlorine (g) + water (1) →→→hydrochloric acid (aq) + chloric acid (HCIO3) (aq) What is the theoretical yield of hydrochloric acid ? What is the percent yield of hydrochloric acid ? grams %
In the combustion of pentanol according to the equation: 2C5H11OH + 15 O2 → 10CO2 + 12H2O How many molesof CO2 are produced if 2.28 mole of H2O are produced
In one experiment, 12.0 g of PCl5 was slowly added to 15.0 g of H2O according to the following balanced chemical equation: Pcl5(s)+4H2O(l) ---> H3PO4 (aq) + 5HCl (g) The molar masses for each compounds in the equation are as follows; PCl5: 208.224 g/mol H2O: 18.015 g/mol H3PO4: 97.994 g/mol HCl; 36.45 g/mol What is the limiting reagent in this scenario? Your answer should be an explanation! You're not solving anything. Note! Make an accurate claim: The limiting reagent in this scenario is _____. Provide additional details and use subject specific language. Cite evidence from what's given to you in the problem that supports your answer, hint: look at that equation!. Lastly! Fully connect the evidence to the claim/your answer to the question. Include subject specific language in your reasoning. The two images attached are examples of how your response SHOULD look.
According to the following reaction, how many moles of potassium sulfate will be formed upon the complete reaction of 24.0 grams of potassium hydrogen sulfate with excess potassium hydroxide?potassium hydrogen sulfate (aq) + potassium hydroxide (aq) potassium sulfate (aq) + water (l)? moles potassium sulfate
According to the following reaction, how many grams of ammonia will be formed upon the complete reaction of 23.1 grams of hydrogen gas with excess nitrogen gas?nitrogen (g) + hydrogen (g) ammonia (g)
According to the balanced reaction below, calculate the quantity of moles of NH, gas that form when 4.20 mol of N,H, liquid completely reacts: 3 N,H,(1) → 4 NH,(g) + N,(g)
For each of the following balanced chemical equations, calculate how many grams of the products listed would be produced by complete reaction of 0.480 mol of the first reactant. (a) CaCO3(s) + HCl(aq) → CaCl2(aq) + CO2(g) + H2O(l) CaCl2 g CO2 g (b) Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s) ZnSO4 g Cu g (c) N2H4(l) + O2(g) → N2(g) + 2 H2O(g) N2 g H2O g (d) NH4Cl(aq) + NaOH(aq) → NH3(g) + NaCl(aq) + H2O(l) NH3 g NaCl g
For the following reaction, 0.497 moles of sulfur are mixed with 0.217 moles of carbon monoxide. What is the formula for the limiting reagent? What is the maximum amount of sulfur dioxide that can be produced? sulfur(s) + carbon monoxide(g) -> sulfur dioxide(g) + carbon(s)