---### Decomposition of Mercury (II) Oxide**Problem Statement:**When 15.00 g of mercury (II) oxide decomposes, how many moles of oxygen gas are produced?**Chemical Equation:**\[\_ \text{HgO} \rightarrow \_ \text{Hg} + \_ \text{O}_2\]**Approach to Solve:**1. **Balance the Chemical Equation:** - The balanced equation is as follows: \[2 \text{HgO} \rightarrow 2 \text{Hg} + \text{O}_2\]2. **Calculate the Moles of \(\text{HgO}\):** - First, determine the molar mass of \(\text{HgO}\): \[ \text{HgO} = (200.59 \text{ g/mol}) + (16.00 \text{ g/mol}) = 216.59 \text{ g/mol} \] - Next, calculate the number of moles of \(\text{HgO}\) in 15.00 g: \[ \text{moles of HgO} = \frac{15.00 \text{ g}}{216.59 \text{ g/mol}} \approx 0.0692 \text{ moles} \]3. **Determine the Moles of O\(_2\) Produced:** - According to the balanced equation, 2 moles of \(\text{HgO}\) produce 1 mole of \(\text{O}_2\). - Therefore, the moles of \(\text{O}_2\) produced from 0.0692 moles of \(\text{HgO}\) can be calculated as: \[ \text{moles of O}_2 = \frac{0.0692 \text{ moles} \times 1 \text{ mole O}_2}{2 \text{ moles HgO}} \approx 0.0346 \text{ moles O}_2 \]**Answer:**When 15.00 g of mercury (II) oxide decomposes, approximately 0.0346 moles of oxygen gas are produced.---### Explanation of Diagrams and Graphs:There are no visual graphs or diagrams provided in the given image. The problem is focused on

Given : When 15.00 g of mercury (ll) oxide decomposes, how many moles of oxygen gas are produced?…

Answered: When 15.00 g of mercury (I) oxide…

Science

Chemistry

When 15.00 g of mercury (I) oxide decomposes, how many moles of oxygen gas are produced? _HgO _Hg +02

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

In the unbalanced chemical equation shown above for the combustion of ethanol, what least common multiple whole number coefficient should go in front of the hydrocarbon (C2H5OH) to balance the equation? See image below
I’m having trouble trying to find the answer to this question
What is the easiest process to get to the result?
2NaClO, --> 2NaCI + 30, Reactants combine into a large one Reactant breaks apart into smaller molecules A pure element swaps places with an element in a compound elements from two different compounds switch place a hydrocarbon reacts with oxygen to form carbon dioxide and water
Please don't provide handwritten solution....
Consider the reaction of copper(II) oxide with aluminum metal to produce copper metal and aluminum oxide: 3 CuO(s) + 2 AlI(s) → 3 Cu(s) + Al2O3(s) If 7.99x1023 atoms Al react with an excess of CuO, what mass of Cu(s) is produced? Assume the reaction goes to 100% completion. Enter your response in decimal notation to three significant figures. Answer: Enter Value g.
ookmarks Profiles Tab Window Help G molar r ste X Learnir O Checko R Search M Ryerso E Ryerso Jassignments/389/tasks/103 The Haber-Bosch process involves the combination of nitrogen and hydrogen at high temperatures in the presence of a catalyst to produce ammonia. It is currently the main industrial source of ammonia. N2 (g) + 3 H2 (g) 2 NH3 (g) Assuming that a reaction vessel originally contains 0.400 moles of N, and 0.900 moles of H2 , answer each of the following questions: a) How many moles of NH3 could be produced from these quantities of N, and H2 ? mol NH3 0.600 b) After the reaction is complete, how many moles of N2 would remain? mol N2 0.100 c) After the reaction is complete, how many moles of H2 would remain? moles H2 0.8
Find the Mass to Mass Stoichiometry Calculutation using this formula: CaS5 + HCl → S + CaCl2 + H2S whereas here are the other given: Raw Materials: 500 g calcium polysulphide and 1.5 kg hydrochloric acid Actual Yield: 343.4g precipitated sulfur
If 200 kJ of heat are supplied, how many grams of NO can be produced? N2(g) + O2(g)→ 2 NO(g) AH = 180.6 kJ/mol O 66.5 g 54.2 g O 30.1 g O 2.21 g
Methanol has tremendous potential to be used as an alternate fuel. Carbon monoxide gas reacted with hydrogen gas can be used to produce methanol.A student reacted 51.9 g of H2(g) with excess CO(g) to produce methanol.If his percent yield was 47.7%, calculate the mass (in g) of CH3OH(l) that he collected in the experiment.Hint: Write a balanced chemical reaction equation.Record only your final answer with the correct number of significant digits and the proper units.
91. A common demonstration in chemistry courses involves adding a tiny speck of manganese(IV) oxide to a concentrated hydro- gen peroxide (H₂O₂) solution. Hydrogen peroxide decomposes quite spectacularly under these conditions to produce oxygen gas and steam (water vapor). Manganese(IV) oxide is a catalyst for the decomposition of hydrogen peroxide and is not consumed in the reaction. Write the balanced equation for the decomposition reaction of hydrogen peroxide. 92. Iron oxide ores, commonly a mixture of FeO and Fe,O,, are given the general formula Fe,O,. They yield elemental iron when heated to a very high temperature with either carbon monoxide or elemen- tal hydrogen. Balance the following equations for these processes: Fe,O(s) + H₂(g) →→→ Fe 0.(s) + CO(e) Fe(s) + H₂O(e) Fe(s) + CO)
The drawing below shows a mixture of molecules: key carbon Onitrogen 238 oxygen chlorine Suppose the following chemical reaction can take place in this mixture: CH₂(g) +4 S(s)→→ CS₂(9)+2 H₂S(9) 0 Of which reactant are there the most initial moles? Enter its chemical formula: 0 Of which reactant are there the least initial moles? Enter its chemical formula: 0 Which reactant is the limiting reactant? Enter its chemical formula: O hydrogen O sulfur