In the red are my answers can u please help me Moto X3M Winter-..Run 3 - Play it now. E 4.3 Questions - Goo..404-Page could n...change the size of iFrame to whatever dimensions you prefer.Concept BuildersAbout the ConceptBuildersVersion 2Identify the reaction type for reactions #1, #2, and #3.Pricing For SchoolsDirections forVersion 2Measurement andபாரட#1:O21g)→ CO2(9)H2O (g)HydrocarbonRelationships andGraphsKinematicsElementCompoundB.#2:->ElementCompoundCompoundCompoundB.# 3:->SCompoundCompoundD.+.Newton's LavwsVectors andProjectilesForces in 2-DimensionSTap below to toggle through answer options andto identity the reaction type for each of the three reactions.Momentum andCollisionsWork and EnergyThe type ofreaction forReaction #1The type ofreaction forReaction #2is ..The type ofreaction forReaction #3isCircular and SatelliteMotionRotation and Balanceis ..s ..Static ElectricityElectric CircuitsSynthesisSingle ReplacementDouble ReplacementWaves and SoundLight and ColorReflection andRefractionCheck Answer

There are different types of reactions depending on heat, direction etc. Reaction 1 = combustion…

entify the reaction type for reactions #1, #2, and #3. 1: O219) -> CO2(9) + + H2O Hydrocarbon 2: Element Compound B Element C Compor D 3: Compound A Compound -> Compound + C Compo D Tap below to toggle through answer options and to identify the reaction type for each of the three reactions. The type of reaction for The type of reaction for The type c reaction fc Reaction #1 Reaction #2 Reaction is is is

entify the reaction type for reactions #1, #2, and #3. 1: O219) -> CO2(9) + + H2O Hydrocarbon 2: Element Compound B Element C Compor D 3: Compound A Compound -> Compound + C Compo D Tap below to toggle through answer options and to identify the reaction type for each of the three reactions. The type of reaction for The type of reaction for The type c reaction fc Reaction #1 Reaction #2 Reaction is is is

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.6PAE

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Some sulfuric acid is spilled on a lab bench. You can neutralizethe acid by sprinkling sodium bicarbonate on it and thenmopping up the resulting solution. The sodium bicarbonatereacts with sulfuric acid according to:2 NaHCO3(s) + H2SO4(aq)----->Na2SO4(aq) + 2 H2O(l)+ 2 CO2(g)Sodium bicarbonate is added until the fizzing due to the formationof CO2(g) stops. If 27 mL of 6.0 M H2SO4 was spilled,what is the minimum mass of NaHCO3 that must be addedto the spill to neutralize the acid?
The simplifying assumption (a.k.a. the 100 rule) Nitrogen oxides from exhaust gases are a serious pollution problem. One such reaction is given here: N2(g) + O2(g) ⇌ 2 NO(g) At the temperature of the exhaust gases from a particular engine the value if K is 4.2 x 10-8. A chemist puts 0.085 mol of nitrogen and 0.038 mol of oxygen in a rigid 1.50 dm3 cylinder. What is the concentration of nitrogen monoxide gas in the mixture at equilibrium?
__K2S(aq) + __H3PO4(aq) ® __K3PO4(aq) + __H2S(g) In a reaction mixture of 14.2 mL of 0.42 M K2S and 6.0 mL of 0.85 M H3PO4: 1. The theoretical yield of H2S from this reaction mixture, in mL at STP is _______ mLSTP 2. If 120 mL at STP of H2S was isolated, the percent reaction yield is ______
In the interface between sediment and water around a deep lake bottom, dissolved oxygen (DO) is usually low. Under such a condition, iron and sulfur typically exist in their reduction forms (i.e. Fe2+ and S2-). Fe2+ and S2- can readily react with each other to produce ferrous sulfide (FeS), which is a black solid substance and finally settles down into the sediments at the lake bottom. The solubility product constant (i.e. equilibrium constant) of FeS is 8 x 10-9. At a chemical equilibrium state, what is the concentration of S2- in the water nearby the sediments if Fe2+ concentration in water is 10 - 4 M.
For a 22.16 mg sample of MgC2O4•H2O (Mwt = 130.35 g/mol) shows two steps:a loss of 3.06 mg from 100–250 oC and a loss of 12.24 mg from 350–550oC. For each step, identify the volatilization product and the solidresidue that remains. In second step, two volatile products are formed.(Mwt C = 12 g/mol; O = 16 g/mol; H = 1 g/mol)
A 50.00 mL volume of 0.0600M K2CrO4 is mixed with 50.00 mL 0.0800 M AgNO3. Calculate the concentration of Ag+, CrO42-, K+, and NO3- at equilibrium. The solubility product of Ag2CrO4(s) is 1.20 x 10-12. Please show work
When 22.0 mL of a 8.84×10-4 M potassium carbonate solution is combined with 25.0 mL of a 6.48×10-4 M iron(II) bromide solution does a precipitate form? fill in the blank 1 (yes or no) For these conditions the Reaction Quotient, Q, is equal to . ( Please type answer note write by hend )
1. Instructor Date Section Station The solubility of magnesium hydroxide (Mg(OH)2) is approximately 3.70 x10−5 M at room temperature. Write the aqueous dissolution ionic reaction for magnesium hydroxide. Include state symbols. Calculate the solubility product constant (Ksp) for magnesium hydroxide at room temperature. Refer back to the General Formula for “K” presented in the “Equilibrium Lab Manual” . 2. 3. c. How many grams of magnesium hydroxide are present in 1.0 L of a saturated solution at room temperature? An Excel plot of ln K vs. �??1� a slope value of −2980 K and an intercept of −10.6. Show all work using Dimensional Analysis to calculate ∆H° in kJ/mol and ∆S° in J⋅K−1⋅mol−1. Hint: Write out the equation for this line in terms of K, T, ∆H° and ∆S° to start with. By setting ∆G = 0 in Eqn. 5, use the Lit values above to solve for “T” below. (Hint: “T” is the only unknown left in that equation now.)
The molarity of a solution is 0.15 M in NaI (aq) at 298.15 K. A large excess of HgI2 (s) to the solution. What is the solubility (in grams) of HgI2 (s) at saturation? HgI2 (s)<------->Hg2+ (aq) + 2I- (aq) Ksp= 2.7 × 10^-29HgI2 (s) + 2I- <------> [HgI4]2- (aq) Kf= 0.75 M
MnSO4•H2O is soluble in water at 25°C, with a solubility of 70.0 g per 1000 g of solution. A saturated solution of MnSO4•H2O has a density of 1.02 g mL-1. When MnSO4•H2O dissolves in water, it absorbs roughly 3.05 kJ/mol of energy. MnSO4•H2O = 169.03 g/mol; H2O = 18.02 g/mol; MW: MnSO4•H2O = 169.03 g/mol. Which of the following is TRUE about a 0.32 M solution of MnSO4•H2O in water? a. A 0.32 M solution contains 70.0 g MnSO4•H2O b. A 0.32 M solution of MnSO4•H2O is unsaturated c. A 0.32 M solution of MnSO4•H2O is supersaturated d. A 0.32 M solution of MnSO4•H2O is saturated
MnSO4•H2O is soluble in water at 25°C, with a solubility of 70.0 g per 1000 g of solution. A saturated solution of MnSO4•H2O has a density of 1.02 g mL-1. When MnSO4•H2O dissolves in water, it absorbs roughly 3.05 kJ/mol of energy. MnSO4•H2O = 169.03 g/mol; H2O = 18.02 g/mol; MW: MnSO4•H2O = 169.03 g/mol. What is the mole fraction of MnSO4•H2O in its saturated solution?
TOPIC: GRAVIMETRY SHOW THE SOLUTION The mercury in a 0.7152-g sample was precipitated with an excess of paraperiodic acid, H5IO6, according to the following reactions:5 Hg+2 + 2 H5IO6 ---> Hg5(IO6)2(s) + 10 H+The precipitate was filtered, washed free of precipitating agent, dried and found to weigh 0.3408-g. Calculate the percentage of Hg2Cl2 in the sample. Molar Masses: Hg5(IO6)2 = 1448.75 Hg2Cl2 = 472.09 Answer: 38.82% Hg2Cl2 An iron ore was analyzed by dissolving a 1.1324-g sample in concentrated HCl. The resulting solution was diluted with water, and the iron (III) was precipitated as the hydrous oxide Fe2O3·xH20 by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.5394 g of pure Fe2O3. Calculate (a) % Fe, and (b) % Fe3O4 in the sampleMolar Masses: Fe2O3 = 159.69 Fe = 55.847 Fe3O4 = 231.54 Answer: 33.32% Fe and 46.04% Fe3O4