**Text Transcription**5. Many metals react with oxygen gas to produce the metal oxide. One of the most common reactions involves solid magnesium burning in a Fourth of July sparkler. If you have 20.2 g of solid magnesium and 34.1 g O₂, how many grams of MgO will be produced in this reaction? The reaction is given below:\[ \text{Mg(s)} + \, \text{O}_2\text{(g)} \rightarrow \, \text{MgO(s)} \]**Explanation**The problem describes a chemical reaction where magnesium (Mg) reacts with oxygen gas (O₂) to form magnesium oxide (MgO). This is a typical combustion reaction that releases energy, often seen in fireworks such as sparklers. The reaction equation is not yet balanced in the given form, so it reflects a need to balance the chemical equation for further calculations.

Answered: Image /qna-images/answer/256c32d5-1c08-4374-b46e-f7846a624a0d.jpg

P. Many metals react with oxygen gas to produce the metal oxide. One of the most common reactions involves solid magnesium burning in a Fourth of July sparkler. If you have 20.2 g of solid magnesium and 34.1 g O2, how many grams of MgO will be produced in this reaction? The reaction is given below: Mg(s) + MgO(s) – (6)2)

P. Many metals react with oxygen gas to produce the metal oxide. One of the most common reactions involves solid magnesium burning in a Fourth of July sparkler. If you have 20.2 g of solid magnesium and 34.1 g O2, how many grams of MgO will be produced in this reaction? The reaction is given below: Mg(s) + MgO(s) – (6)2)

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

If 25.0g of Nh3 and 45.0 of O2 reacts in the following reaction, what is the mass in grams of No that will be formed? 4NH3(g) +5.02(g)-4NO(g)+6H2O(g)
Balance the chemical equation for the combustion of pentane: C5H12 (g) + O2(g) → CO2 (g) + H2O (g) I need help with the amount on reactant side, element, amount on product side
Given the reaction below, if 23.5 moles ammonium carbonate is heated and it decomposes, how many moles of water form? (NH4)2CO3 (s) → 2 NH3 (g) + CO2 (g) + H2O (g)
G periodic table- Google Search OHow many moles of lithium hyd x Question 8 of 8 What is the mass in grams of CO2 that can be produced from the combustion of 2.95 moles of butane according to this equation: 2 C.Hi0(g) + 13 O:(g) → 8 CO:(g) + 10 H:O(g)
Small quantities of oxygen can be prepared in the laboratory by heating potassium chlorate, KCIO3(s) The equation for the reaction is 2KCIO3 2KCI + 3 O2 Calculate how many grams of O2(g) can be produced from heating 76.1 g KCIO3(s) g O2 mass:
Ethanol (C₂H₆O) is combusted in air according to the following reaction: C₂H₆O(l) + O₂(g) → CO₂(g) + H₂O(l) How many grams of water would be produced by the complete combustion of 6.45 moles of ethanol in the presence of excess oxygen?
Magnesium metal reacts with iron(III) sulfate to produce iron metal and magnesium sulfate, as shown in the unbalanced equation below. Mg(s) + Fe₂(SO4)3(aq) --> Fe(s) + MgSO4) How many grams of iron(III) sulfate are needed to completely react 12.0 g of magnesium? O 52.6 g O 65.8 g O 168 g O 197 g O 158 g
What is the mass in grams of magnesium chloride that can be produced from 3.47 moles of chlorine gas reacting with excess magnesium? Mg(s) + Cl₂(g) -> MgCl₂(s) What is the mass in grams of NO that can be formed from 3.68 moles of NO₂ in the reaction below? 3 NO₂ (g) + H₂O (g) -> 2 HNO3 (g) + NO (g) Answer in a clear, multiplication/division format with showing all work. Acording to the balanced reaction below, calculate the quantity of moles of NH3 gas that form when 4.20 mol of N2H4 liquid completely reacts: 3 N₂H4(1) - > 4 NH3(g) + N₂(g)
Please help with the last question, please and thank you!
Consider the following reaction: P406(s) P4(s) + 302(g) What mass of P4 will be produced from 12.0 g of po? (Molar massses: P406 = 219.9 g/mol, P4 = 123.9 g/mol) 6.768 21.3 g 0.563 g 1.77 g Consider the reaction below: BaCl2 + Na2SO4 - BaSO4 + 2 NaCl (balanced) What is the theoretical yield of barium sulfate, BaSO4, that can be produced by the reaction of 2.84 g of Na2SO4 with 5.00 g of BaCl2? molar mass of BaCl2 = 208.33 g/mol. molar mass of BaSO4 233.38 g/mol, = molar mass of Na2SO4 = 142.04 g/mol. molar mass of NaCl = 58.44 g/mol 2.38 g 4.67 g 5.60 g 1.73 g