Experiment 10: How much CO2? Introduction The goal of this lab was to determine the amount of grams of sodium bicarbonate (NaHCO3) required to produce enough CO2 gas to completely fill the lab and also how many Alka-Seltzer tablets that would equate to. This was done by collecting CO2 gas by inverting a buret and submerging it under water in order to calculate the volume of CO2 released from a fragment of Alka-Seltzer tablet. The main component of Alka-Seltzer is sodium bicarbonate‚ used to neutralize
Premium Chemistry Temperature Water
CALORIMETRY Abstract: During the experiment‚ the group were able to perform the following objectives; to compute the heat capacity of a Styrofoam-cup calorimeter‚ and also to compute the heat of neutralization of 1.0 M hydrochloric acid and 1.0 M sodium hydroxide‚ the heat of dilution of concentrated sulfuric acid‚ and the heat of solution of solid ammonium chloride The sixth experiment was named "Calorimetry" wherein it is the measurement of how much heat is gained or released by a system
Premium Energy Enthalpy Hydrochloric acid
60+9.53)/3 = 9.66mL Sample Calculations: (9.85+9.60+9.53)/3 = 9.66mL The average volume of NaOH used. Calculations: 1. Moles NaOH = M x V = (0.1M) (0.00966L) = 0.000966 moles 2. Moles HCl = moles NaOH 0.000966 moles -> 9.66x10-4 3. NaOH + HCl = NaCl + H2O Moles NaOH = M x V = (0.1M)(0.00966L) = 0.000966 moles Moles HCl = moles NaOH [HCl] = moles/volumes = (0.000966)/ (0.0096L) [HCl] = 0.1M Follow-up Questions: 1. It will have no effect because the phenolphthalein
Free PH Hydrochloric acid Acid
Experiment 9 Aim A. To investigate the existence of hydrogen bonds between ethanol molecules. B. To measure the strength of hydrogen bond formed between ethanol molecules C. To investigate the formation of hydrogen bonds between molecules of ethyl ethanoate and trichloromethane. D. To measure the strength of hydrogen bond formed between molecules of ethyl ethanoate and trichloromethane. Procedure A. 1. 10 cm3 of ethanol was added into an insulated 50 cm3 beaker by
Premium Oxygen Energy Thermodynamics
II - Mole Calculations/ Limiting and Excess Reagent – Lecture Notes 1. Given the balanced equation N2(g) + 3H2(g) 2NH3(g) How many moles of ammonia are produced when 0.60 mol of nitrogen reacts with hydrogen? 2. Given the equation: SiO2 + HF SiF4 + H2O a. Calculate the number of moles HF that would completely react with 2.5 moles of SiO2. b. Calculate the number of moles SiF4 formed by completely reacting 2.5 moles SiO 2 with HF. c. Calculate the mass of water formed by reacting 2.5 moles SiO
Premium Chlorine Sodium Stoichiometry
are written with water separate by a dot (.). This (.) means for hydrated metal salt there are how many number of moles of water bound to each mole of that metal salt. Research Question: The aim of this experiment is to calculate the number of moles of water bounded to each mole of cobalt chloride ( CoCl2. H2O). This cobalt chloride hydrated may be monohydrate with 1 mole of water attracted to cobalt chloride. It may be dihydrate‚ trihydrate‚ tetrahydrate or pentahydrate; your task is
Premium Water Salt Sodium
50‚ 1.35 x 10‒5 and 8.70 moles respectively in a 12-L flask. Calculate the equilibrium constant 7 Kc. (1.08 x 10 ) 2. The number of moles of H2‚ O2‚ and H2O present at equilibrium for the reaction: 3. The equilibrium constant Kc for the reaction: 2HCl(g) ⇄ H2(g) + Cl2(g) is 0.0213 at 400 C. If 20.0 o moles of HCl(g) are heated at 400 C‚ what amounts of HCl(g)‚ H2(g) and Cl2(g) would be present in the equilibrium mixture? (H2 = Cl2 = 2.26 moles; HCl = 15.48 moles) o 4. The equilibrium
Premium Chemical equilibrium
Number | MS204-S/03 | Manufacturer | METTLE TOLEDO | Type | New Classic MF | Boiling chips detail:- VWR scientific‚ Inc. Porous boiling chips VWR cat. # 26397 - 409 Given sample: - 2-propanol (CH3CHOHCH3) Molecular weight: - 60.08 gm/mole Sample volume taken: - 2 mL | Flask 1 | Flask 2 | Flask 3 | Mass of flask and condensed vapour | 77.8735 gm | 77.8768 gm | 77.8750 gm | Mass of empty flask apparatus | 77.6050 gm | 77.6059 gm | 77.6055 gm | Mass of condensed vapour | 0.2685
Premium Water Atmospheric pressure Thermodynamics
C2H3O2NO2 2/3 Co(acac)3 + 2 C2H3O2NO2 ( 2/3 Co(acac-NO2)3 + 2 C2H3O2 • Moles of reagent used - Cu(NO3)2·3H2O‚ MW: 241.59 g/mol [pic] - Acetic anhydride‚ MW: 102.1 g/mol‚ D: 1.080 g/mL [pic] - Co(acac)3‚ MW: 356.24 g/mol [pic] • Limiting Reagent From the stoichiometry of the reactions‚ acetic anhydride is in excess‚ and 2/3 (0.67) mole Co(acac)3 should reaction with 1 mole copper nitrate trihydrate. The actual mole ratio when 0.49 g Co(acac)3
Premium Acetic acid Stoichiometry Sodium acetate
Formula: Number of Moles = Concentration x Volume Therefore‚ No of Kl Moles = Concentration x Volume = 0.30 x 0.01 ± 0.0005 = 0.003mol ± 0.000015mol No. of Pb(NO3)2 Moles = Concentration x Volume = 0.50 x 0.01 ± 0.0005 = 0.005mol ± 0.000025mol Also‚ The Theoretical Mole Ratio would be: 21=2 The Experimental Mole Ratio would be: 0.0030
Premium Stoichiometry Chemistry