Homework Answers
16. The mole no of Cr = 0.7655/51.996 = 0.01472
The mole no of Cl = 1.566/35.453 = 0.04417
The empirical formula will be CrCl3
17. In a chemical reaction, the substance which gets used up first is called reactant.
18. In a chemical reaction, the maximum amount of product which can be made when one of two starting materials is completely used up is called the reagent.
19. The equation which relates the light absorbed through a solution to the concentration of that solution is A = e bc and it is called Beer's law.
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16. A student reacted 0.7655 g of chromium (at. wt = 51.996 g/mol) with exactly 1.566...
16 A student reacted 0.7655 g of chromium (at. wt 51.996 g/mol) with exactly 1.566 chlorine...
16 A student reacted 0.7655 g of chromium (at. wt 51.996 g/mol) with exactly 1.566 chlorine (at. wt.-35.453 g/mol). Convert both these masses to moles and determine the empirical formula (like A x) of the compound of Cr and CL. SHOW YOUR WORK gof 17. In a chemical reaction, the substance which gets used up first (or runs out first) is called the (write in the correct words). 18. In a chemical reaction, the maximum amount of product which can...
15. Use the Ideal Gas Law and the answers to questions 12, 13 and 14 to calculate the number of moles of hydrogen g...
15. Use the Ideal Gas Law and the answers to questions 12, 13 and 14 to calculate the number of moles of hydrogen gas present. R 0.0821 Leatm/mol K (watch sig figs.) 16. A student reacted 0.7655 g of chromium (at. wt - 51.996 g/mol) with exactly 1.566 g of chlorine (at. wt. - 35.453 g/mol). Convert both these masses to moles and determine the empirical formula (like AX) of the compound of Cr and CL SHOW YOUR WORK 17....
A rigid container initially contains only 0.25 mol of NH3 (g) in a 5.0 L volume. We introduce 0.20 mol of HCI (g) at 25 °C. a. Write the chemical equation for this reaction assuming that it forms one...
A rigid container initially contains only 0.25 mol of NH3 (g) in a 5.0 L volume. We introduce 0.20 mol of HCI (g) at 25 °C. a. Write the chemical equation for this reaction assuming that it forms one product. b. Calculate the final pressure in the container after the reaction in a. is complete If some of this product were added to water, what would happen to the pH of solution relative to pure water? c. Instead of the...
Professor Edixordyh conducted an experiment in her laboratory. She reacted 25.0 g of solid cobalt(III) carbonate wi...
Professor Edixordyh conducted an experiment in her laboratory. She reacted 25.0 g of solid cobalt(III) carbonate with 50.0 cm2 of 2.00 mol dm dilute nitric acid. (a) Write a balanced chemical equation, including state symbols, for the reaction. (b) Write an ionic equation for the reaction. (c) Determine if there is any excess reagent and if yes, calculate the amount of excess reagent. (d) Draw a fully labelled diagram to illustrate the method which Professor Edixordyh.can Use to remove any...
1.How many grams of glucose (C6H12O6) are produced if 17.3 mol of H2O are reacted according...
1.How many grams of glucose (C6H12O6) are produced if 17.3 mol of H2O are reacted according to this balanced chemical equation? 6CO2 + 6H2O → C6H12O6 + 6O2 2. Nitroglycerin [C3H5(ONO2)3] is made by reacting nitric acid (HNO3) with glycerol [C3H5(OH)3] according to this reaction: C3H5(OH)3 + 3HNO3 → C3H5(ONO2)3 + 3H2O If 87.4 g of HNO3 is reacted with excess glycerol, what mass of nitroglycerin can be made? 3. Precipitation reactions, in which a solid (called a precipitate) is...
What would be for the mol reacted,, mol NH4X in sample, and yhr average molar mass?...
What would be for the mol reacted,, mol NH4X in sample, and yhr
average molar mass?
CALCULATIONS A. NaOH Preparation: Approximate molarity of NaOH 0.48 M B. NaOH Standardization: Trial # Mass of KHP E 1.7249 1.9569 1.8799 Volume of NaOH 18.58 L 20.58mLihat 19.71 mL Molarity of NaOH 0.4544 M 0.4654M 0. 3 M 0.4668M Average molarity of NaOH: 0.4668 M 0.4622 M C. Molar Mass of NH X Salt 1. Volume of NaOH 0.025 0.025 0.025L 2. Molarity...
The standard enthalpy of formation (ΔH∘f) is the enthalpy change that occurs when exactly 1 mol of a compound is formed...
The standard enthalpy of formation (ΔH∘f) is the enthalpy change that occurs when exactly 1 mol of a compound is formed from its constituent elements under standard conditions. The standard conditions are 1 atm pressure, a temperature of 25 ∘C , and all the species present at a concentration of 1 M . A "standard enthalpies of formation table" containing ΔH∘f values might look something like this: Substance ΔH∘f H(g) 218 kJ/mol H2(g) 0 kJ/mol Ba(s) 0 kJ/mol Ba2+(aq) −538.4...
Materials: NaOH MW = 40 g/mL, KHP - potassium hydrogen phthalate, KHC8H404, MW = 204.23 g/mol....
Materials: NaOH MW = 40 g/mL, KHP - potassium hydrogen phthalate, KHC8H404, MW = 204.23 g/mol. Acetic acid, HC2H302, MW = 60.05 g/mol Part 1: Standardization of NaOH Assume 0.951 g of KHP is weighed and transferred to a 250 mL Erlenmeyer flask. Approximately 50 ml water is added to dissolve the KHP. Note that the exact volume of water is not important because you only need to know the exact number of moles of KHP that will react with...
Materials: NaOH MW = 40 g/mL, KHP - potassium hydrogen phthalate, KHC8H404, MW = 204.23 g/mol....
Materials: NaOH MW = 40 g/mL, KHP - potassium hydrogen phthalate, KHC8H404, MW = 204.23 g/mol. Acetic acid, HC2H302, MW = 60.05 g/mol Part 1: Standardization of NaOH Assume 0.951 g of KHP is weighed and transferred to a 250 mL Erlenmeyer flask. Approximately 50 ml water is added to dissolve the KHP. Note that the exact volume of water is not important because you only need to know the exact number of moles of KHP that will react with...
please show steps. thanks ! Experiment 19 Gas Stoichiometry and the Gas Laws The relationship between...
please show steps. thanks !
Experiment 19 Gas Stoichiometry and the Gas Laws The relationship between the physical properties of a gas, and the moles, is given by the “Ideal Gas Law:" PV=nRT where n-number of moles R=the ideal gas constant: 0.0821 atm L mole 'Kor 62.4 L torr molek In this experiment, the theoretical yield of gas, will be compared to the experimental yield. The reaction of aluminum with hydrochloric acid produces hydrogen according to the balanced equation below....
16 A student reacted 0.7655 g of chromium (at. wt 51.996 g/mol) with exactly 1.566 chlorine (at. wt.-35.453 g/mol). Convert both these masses to moles and determine the empirical formula (like A x) of the compound of Cr and CL. SHOW YOUR WORK gof 17. In a chemical reaction, the substance which gets used up first (or runs out first) is called the (write in the correct words). 18. In a chemical reaction, the maximum amount of product which can...
15. Use the Ideal Gas Law and the answers to questions 12, 13 and 14 to calculate the number of moles of hydrogen gas present. R 0.0821 Leatm/mol K (watch sig figs.) 16. A student reacted 0.7655 g of chromium (at. wt - 51.996 g/mol) with exactly 1.566 g of chlorine (at. wt. - 35.453 g/mol). Convert both these masses to moles and determine the empirical formula (like AX) of the compound of Cr and CL SHOW YOUR WORK 17....
A rigid container initially contains only 0.25 mol of NH3 (g) in a 5.0 L volume. We introduce 0.20 mol of HCI (g) at 25 °C. a. Write the chemical equation for this reaction assuming that it forms one product. b. Calculate the final pressure in the container after the reaction in a. is complete If some of this product were added to water, what would happen to the pH of solution relative to pure water? c. Instead of the...
Professor Edixordyh conducted an experiment in her laboratory. She reacted 25.0 g of solid cobalt(III) carbonate with 50.0 cm2 of 2.00 mol dm dilute nitric acid. (a) Write a balanced chemical equation, including state symbols, for the reaction. (b) Write an ionic equation for the reaction. (c) Determine if there is any excess reagent and if yes, calculate the amount of excess reagent. (d) Draw a fully labelled diagram to illustrate the method which Professor Edixordyh.can Use to remove any...
What would be for the mol reacted,, mol NH4X in sample, and yhr
average molar mass?
CALCULATIONS A. NaOH Preparation: Approximate molarity of NaOH 0.48 M B. NaOH Standardization: Trial # Mass of KHP E 1.7249 1.9569 1.8799 Volume of NaOH 18.58 L 20.58mLihat 19.71 mL Molarity of NaOH 0.4544 M 0.4654M 0. 3 M 0.4668M Average molarity of NaOH: 0.4668 M 0.4622 M C. Molar Mass of NH X Salt 1. Volume of NaOH 0.025 0.025 0.025L 2. Molarity...
Materials: NaOH MW = 40 g/mL, KHP - potassium hydrogen phthalate, KHC8H404, MW = 204.23 g/mol. Acetic acid, HC2H302, MW = 60.05 g/mol Part 1: Standardization of NaOH Assume 0.951 g of KHP is weighed and transferred to a 250 mL Erlenmeyer flask. Approximately 50 ml water is added to dissolve the KHP. Note that the exact volume of water is not important because you only need to know the exact number of moles of KHP that will react with...
Materials: NaOH MW = 40 g/mL, KHP - potassium hydrogen phthalate, KHC8H404, MW = 204.23 g/mol. Acetic acid, HC2H302, MW = 60.05 g/mol Part 1: Standardization of NaOH Assume 0.951 g of KHP is weighed and transferred to a 250 mL Erlenmeyer flask. Approximately 50 ml water is added to dissolve the KHP. Note that the exact volume of water is not important because you only need to know the exact number of moles of KHP that will react with...
please show steps. thanks !
Experiment 19 Gas Stoichiometry and the Gas Laws The relationship between the physical properties of a gas, and the moles, is given by the “Ideal Gas Law:" PV=nRT where n-number of moles R=the ideal gas constant: 0.0821 atm L mole 'Kor 62.4 L torr molek In this experiment, the theoretical yield of gas, will be compared to the experimental yield. The reaction of aluminum with hydrochloric acid produces hydrogen according to the balanced equation below....
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