Types+of+Reactions+Lab

Answer number 2-5

3. Using this data, calculate a value for Kc for the reaction, A. 2.06 x 104 B. 4.84 x 10-3 C. 0.223 D. 4.49 E. 20.2 2 NO(g) + Cl₂(g) 2. NOCI(g) Kc = 3.20 x 10-³ 2 NO2(g) 2 NO(g) + O₂(g) Kc = 15.5 4. Using the data, NOCI(g) + 1/2O2(g) NO2(g) + ½ Cl₂(g) 3 A (g) + 4 B (g) A3B4 (g) calculate a value for Kc for the reaction, 3 A (g) + 4 B -A3B4 (g) 2 AB (g) + AB2 (g) (g) Kc = 25 Kc = 3.75 2 AB (g) + AB2 (g)

9:55 ull LTE Question 4 of 15 Submit Determine the mass in grams of C4H10 that are required to completely react to produce 8.70 mol of CO2 according to the following combustion reaction: 2 C4H10(g) + 13 O2(g) → CO2(g) + 10 H20(g) STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 0.0374 2 mol C4H10 1 mol CO2 8.70 44.01 g H20 2.18 4.35 g O2 18.02 208.00 g CH10 126 13 mol H20 10 6.022 x 1023 mol O2 58.14 g CO2 Tap here or pull up for additional resources

du.co Question 10 of 22 Balance the following chemical equation (if necessary): CH(g) + O,(g) → H,O(g) + CO,(g) 04- 03. 02. O+ O2+ D3+ 04+ 1 4 7 8 9. O3 04 Os + (s) (1) (g) (aq) CO CH.0 H,O Reset • x H,O Delete MacBook Air 80 DII F3 F4 F7 F8 F9 @ $ & 2 4 5 6 8 9 W E R Y S D F G H J K C V B M * CO *3

12. Use the following equations to answer the next four questions: i. H2O(s) → H,O(1) Water ii. Na (aq) + Cl (aq) + Ag*(aq) + NO3 (aq) AgCl(s) + Na*(aq) + NO3 (aq) ii. CH3 OH(g) + O2(g) → CO2 (g) + H,O(g) -> iv. 2H,0(1) → 2H2(g) + O2(g) -> v. H* (aq) + OH (aq) H20(1) (a) Which equation describes a physical change? (b) Which equation identifies the reactants and products of a combustion reaction? (c) Which equation is not balanced? (d) Which is a net ionic equation?

If Kc = 1.52 for O 2 (g) + 2 CO (g) 2 CO 2 (g), what is the value of Ke for the reaction 4 CO2 (g) = 2 02 (g) + 4 CO (g) (with 3 significant figures)? a. 0.433 b.0.329 с. 1.32 d. 1.52 е. 3.04

9:48 LTE Question 3 of 15 Submit What quantity of moles of H2SO, are required to completely react with 7.20 mol of Al according to the balanced chemical reaction: 2 Al(s) + 3 H2SO4(aq) → Al2(SO4)3(aq) + H2(g) X STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 2.40 21.6 mol H2SO. 6.022 x 1023 342.14 mol Al 2.89 x 1024 6.50 x 1024 g Al2(SO.)3 7.20 1 mol Al;(SO.)3 2 10.8 mol H2 3 3.60 g H2 98.08 2.02 g Al 26.98 g H2SO. Tap here or pull up for additional resources

Which of the following statements is correct concerning the formula of a hydrate experiment? All hydrated salts can be converted into anhydrous salts by heating O Heating the hydrated salt too strongly at the beginning, will lead to a decrease in the calculated value of "x". 20 If the dehydration of the hydrate is incomplete, the calculated value of x" will be lower than the actual value. If the mass of hydrated salt and H20 are 0.59 g and 0.24 g, respectively, then the mass % of water of crystallization is 29 %. O If1.1g of alum is recorded instead of 1.0 g, the calculated value of "x" will be lower than the actual value.

(6) question is in the photo below

Scientifically, nitrogen and hydrogen at high temperature are converted to ammonia. When 350 grams of Hydrogen gas are added to an excess amount of Nitrogen gas, 80 grams of Ammonia are formed. Calculate the percent yield. * (10 Points) 3H2+ N2> 2NH3

Answer for the following questions. Q. 1 The progress of chemical reaction is monitored by measuring the volume of product/s from time to time during the course of the reaction. Identify the reactant/product for the following reactions whose concentration will be measured to monitor the progress of reaction. N20, 2NO, + 1/20, SO,CI, ►SO,+Cl2 CH;N= NCH3 N2 + C,H6

5. The reaction of gaseous potassium superoxide, KO, is used in life-support systems to replace CO:(g) in expired air with O:(g). The unbalanoced chemical equation for the reaction is given below. KO:(s) + CO:(g) – K:CO:(s) + O:(g) How many moles of K:CO:(s) are produced per milligram of KO2(s) consumed?

What volume (in cm3) cm3 of glacial acetic acid (100 % of acetic acid, with a density of 1.050g/cm3 ) is needed to produce 1.0 dm3 of pH 3.3 acetic acid?Ks = 1.75 x 10-5MM [CH3COOH] = 60.05 g/mol

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Font Paragraph Styles • 10.I·11 · 12. 14.I 15 · I· 16 . I 17 Rank the basic properties of the following compounds by explaining the factors that influence them:Me3N, Me2NH, MENH2, NH3 a. NH2OH, NH2NH2 b. MesN, Me2NH, MeNH2, NH3 c. MENH2, ETNH2, i-PRMH2, i-BUNH2 d. Me2NH, ET2NH, i-PR2NH, i-BU2NH

7 4. NaHSO4 (Sodium hydrogen sulfate) Number Element of atoms Na: H: S: O: Number Element of atoms Ca: P: O: X X X X Element %S = %K= X X X 5. Ca3(PO4)2 (Calcium phosphate) X X Atomic Mass X X Formula mass Atomic Mass Formula mass || || = |||||||||| = Product Product Part 2: Percent Mass Composition: The formula mass (molecular mass) and the elemental information for the compounds in Part 1. Solve for the % Mass Composition of each element in the compound. 1. K₂S (potassium sulfide).

9:39 1 ull LTE Question 16 of 24 Submit How many grams of oxygen gas are produced when 2.43 x 10-4 g of KCIO; are completely reacted according to the following chemical equation: 2 KCIO3(s) → 2 KCI(s) + 3 O2(g) STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 1 9.52 x 10-5 g KCIO3 32.00 2 mol KCIO, 1.90 x 10-4 3 mol KCI 74.55 5.95 x 10-6 mol O2 1.98 x 10-6 6.022 x 1023 g O2 2.43 x 10-4 122.55 g KCI 2.97 x 10-6 Tap here or pull up for additional resources

2:26 PM Thu Mar 3 Chapter 9 Limiting and Excess Reactants Feb 28, 2022 at 10:05 AM Name/Date Lacey Boswell 113/12 Honors Chemistry Chapter 9 Limiting and Excess Reactants Show ALL work for the following calculations: 1a. If you perform the following reaction with 35 grams of C&H10 and 45 grams of oxygen, how many grams of carbon dioxide will be formed? 2 CH10 + 17 02 → 12 CO2 + 10 H2O 55g What is the liming reagent? w much of the excess reagent is left over after the reaction is finished?

Balance this reaction by adding the missing coefficients of 2 or higher: X' X. He H,SO,+ NaOH Na, SO+ H,0

HSC 258 Major Projec X Mind Tap - Cengage Lea X d%3D55750828934189288909969212&elSBN=9781305657571&snapshotld%3D219989 The illustration to the left represents a mixture of iodine ( purple ) and fluorine ( green ) molecules. If the molecules in the above illustration react to form IF3 according to the equation I +3 F2 2 IF3 , the limiting reagent is the number of IF, molecules formed is and the number of atoms/molecules in excess is Submit Answer

3:18 Question 14 of 16 Which of the following reactions would have the most negative AS° value ? A) N₂(g) + 3 Cl₂(g) → 2 NC13(g) B) CaSO4 7 H₂O(s) → CaSO4(s) + 7 H₂O(g) C) K(s) + O₂(g) → KO₂ (s) D) NH3(g) + HBr(g) → NH,Br(s) E) 2H₂(g) + O₂(g) → 2 H₂O(g) Submit Tap here or pull up for additional resources

Chemistry

2) The following series of reactions were carried out. PbCO3(s) + 2HNO3(aq) à Pb(NO3)2(aq) + H2O(l) + CO2(g) Pb(NO3)2(aq) + 2HCl(aq) à 2HNO3(aq) + PbCl2(s) (a) If a student starts with 2.871 g of lead(II) carbonate for the first reaction and all other reagents are added in excess, what is the theoretical yield of lead(II) chloride solid? (b) If the student isolates 2.385 g of lead(II) chloride, what is the percent yield?

3.

For the reaction of nitrogen and oxygen to form nitrogen dioxide, N2(g) + 202(g) =2NO2(g) Ko = 1.5x103 If the reaction mixture is found to contain 2.0 M NO2 and 0.10 M N2 and 0.10 M O2, what is the value of Q and what does this mean? Periodic Table and Datasheet Select one: O a. Q = 2x102 and the reaction will proceed towards the reactants. %3D O b. Q= 2x102 and the reaction will proceed towards the products. O c. Q = 4x193 and the reaction will proceed towards the reactants. %3D O d. Q = 4x103 and the reaction will proceed towards the products. %3D Oxygen and ozone are allowed to come to equilibrium in the exothermic reaction

Balance the following chemical equation (ifnecessary):C6H6O(I) + O2(g) -> H20 (g) + CO2 (g)

Solve this