1. How would using double the volume of hydrochloric acid have affected the empirical formula of...
1. How would using double the volume of hydrochloric acid have affected the empirical formula of zinc chloride?
2. Suppose that you had not driven off all the water from the zinc chloride. How would this error have affected the empirical formula for zinc chloride?
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1. How would using double the volume of hydrochloric acid have
affected the empirical formula of...
1. How would using double the volume of hydrochloric acid have affected the empirical formula of zinc chloride? 2. Suppose that you had not driven off all the water from the zinc chloride. How would t...
1. How would using double the volume of hydrochloric acid have affected the empirical formula of zinc chloride? 2. Suppose that you had not driven off all the water from the zinc chloride. How would this error have affected the empirical formula for zinc chloride?
Questions: 1. Write a balanced equation for the reaction of zinc with hydrochloric acid, including states....
Questions: 1. Write a balanced equation for the reaction of zinc with hydrochloric acid, including states. 2. In a separate reaction, 0.775g of zinc powder was reacted with 8.5 mL of hydrochloric acid solution. The hydrochloric acid solution has a density of 1.09 g/mL. Use this information to answer the questions below. a. What is the theoretical yield of zinc chloride that can be produced from this reaction? Show work. b. What is the limiting reactant? Which reactant is in...
1. How would you determine if you have heated the sample long enough to drive off...
1. How would you determine if you have heated the sample long enough to drive off all the water from the hydrate? 2. A compound is made of 30.9% of Cu, 13.6 % Si, and 55.5% F. a. What is the empirical formula of the anhydrous salt? b. 1.00 gram of this compound is subject to high moisture environment. The resulting hydrate weighs 1.53 grams. What is the formula of the hydrate?
1 Ka Cr Oy MI-A 3x1 C4 - NO STOR : The Empirical Formula of an...
1
Ka Cr Oy MI-A 3x1 C4 - NO STOR : The Empirical Formula of an Oxide analysis it was found to 2. A sample of ampound containing Co, and silver (Ag) weighed 1.372 g. On analysis it was 28 Oand 0974 g Ag. The molar mass of the compound is 303.8 g mol and the masses of c and Ag are 12.01 g mol-16.00 g mol), and 107.9 g mol, respectively. Dete the empirical and molecular formulas of the...
4. How would the calculated equivalent mass of the unknown acid in this experiment be affected if: (a) The buret was con...
4. How would the calculated equivalent mass of the unknown acid in this experiment be affected if: (a) The buret was contaminated with acid solution? (b) Not all of the unknown weighted acid was transferred to the titration beaker? (c) The volume of distilled water in which the unknown acid was dissolved was not accurately known?
For the following reaction, 28.4 grams of hydrochloric acid are allowed to react with 70.8 grams...
For the following reaction, 28.4 grams of hydrochloric acid are allowed to react with 70.8 grams of barium hydroxide. hydrochloric acid (aq) + barium hydroxide (aq) barium chloride (aq) + water (l) What is the maximum amount of barium chloride that can be formed? ____ grams What is the FORMULA for the limiting reagent? ___ What amount of the excess reagent remains after the reaction is complete? ________grams 2. According to the following reaction: 2HCl (aq) + Ba(OH)2 (aq) BaCl2 (aq)...
Commercial hydrochloric acid is available as a 10.17 molar solution. How would you use this to...
Commercial hydrochloric acid is available as a 10.17 molar solution. How would you use this to prepare 200 mL of a 1.00 molar solution? Select one: O a. 19.7 mL of HCl +water to make the total solution volume of 200 ml O b. 1.97 mL of HCI + water to make the total solution volume of 200 ml O C. 1.97 mL of HCl + 200 mL of water O d. 19.7 mL of HCI + 200 mL of...
How would the following errors affect the empirical formula of the compound for a hypothetical student...
How would the following errors affect the empirical formula of the compound for a hypothetical student performing s experiment? Note: Writing the answer will be incorrect is not sufficient for these questions. This student is not E) you nor is their data assumed to be the same as yours. student ran out of time and did not do the second heating. Explain thoroughly how this error will affect the water in the hydrate? Will the moles of water calculated be...
27 Aqueous hydrochloric acid (HCI) will react with solid sodium hydroxide (NaOH) to produce aqueous sodium...
27 Aqueous hydrochloric acid (HCI) will react with solid sodium hydroxide (NaOH) to produce aqueous sodium chloride (NaCl) and liquid water (H₂O). Suppose 7.7 g of hydrochloric acid is mixed with 5.29 g of sodium hydroxide. Calculate the maximum mass of sodium chloride that could be produced by the chemical reaction. Round your answer to 3 significant digits. ? The chemical formula for acetone is: (CH3),co Calculate the molar mass of acetone. Round your answer to 2 decimal places. -1...
the metal reacts with hydrochloric acid giving off hydrogen gas, Ha according to the equation: _Zn...
the metal reacts with hydrochloric acid giving off hydrogen gas, Ha according to the equation: _Zn (9) + HCl (= ZnCl (a* Họ tỏ a. Balance the equation Determine how many moles of zinc are required to produce 6.25 moles of hydrogen c. Determine how many grams of zinc are required to produce 4.5 moles of hydrogen gas? d. Determine how many grams of hydrogen gas are produced from 27.2 g of hydrochloric acid? 5. Glucose, CH20.(s) burns in air...
Questions: 1. Write a balanced equation for the reaction of zinc with hydrochloric acid, including states. 2. In a separate reaction, 0.775g of zinc powder was reacted with 8.5 mL of hydrochloric acid solution. The hydrochloric acid solution has a density of 1.09 g/mL. Use this information to answer the questions below. a. What is the theoretical yield of zinc chloride that can be produced from this reaction? Show work. b. What is the limiting reactant? Which reactant is in...
1. How would you determine if you have heated the sample long enough to drive off all the water from the hydrate? 2. A compound is made of 30.9% of Cu, 13.6 % Si, and 55.5% F. a. What is the empirical formula of the anhydrous salt? b. 1.00 gram of this compound is subject to high moisture environment. The resulting hydrate weighs 1.53 grams. What is the formula of the hydrate?
1
Ka Cr Oy MI-A 3x1 C4 - NO STOR : The Empirical Formula of an Oxide analysis it was found to 2. A sample of ampound containing Co, and silver (Ag) weighed 1.372 g. On analysis it was 28 Oand 0974 g Ag. The molar mass of the compound is 303.8 g mol and the masses of c and Ag are 12.01 g mol-16.00 g mol), and 107.9 g mol, respectively. Dete the empirical and molecular formulas of the...
Commercial hydrochloric acid is available as a 10.17 molar solution. How would you use this to prepare 200 mL of a 1.00 molar solution? Select one: O a. 19.7 mL of HCl +water to make the total solution volume of 200 ml O b. 1.97 mL of HCI + water to make the total solution volume of 200 ml O C. 1.97 mL of HCl + 200 mL of water O d. 19.7 mL of HCI + 200 mL of...
How would the following errors affect the empirical formula of the compound for a hypothetical student performing s experiment? Note: Writing the answer will be incorrect is not sufficient for these questions. This student is not E) you nor is their data assumed to be the same as yours. student ran out of time and did not do the second heating. Explain thoroughly how this error will affect the water in the hydrate? Will the moles of water calculated be...
27 Aqueous hydrochloric acid (HCI) will react with solid sodium hydroxide (NaOH) to produce aqueous sodium chloride (NaCl) and liquid water (H₂O). Suppose 7.7 g of hydrochloric acid is mixed with 5.29 g of sodium hydroxide. Calculate the maximum mass of sodium chloride that could be produced by the chemical reaction. Round your answer to 3 significant digits. ? The chemical formula for acetone is: (CH3),co Calculate the molar mass of acetone. Round your answer to 2 decimal places. -1...
the metal reacts with hydrochloric acid giving off hydrogen gas, Ha according to the equation: _Zn (9) + HCl (= ZnCl (a* Họ tỏ a. Balance the equation Determine how many moles of zinc are required to produce 6.25 moles of hydrogen c. Determine how many grams of zinc are required to produce 4.5 moles of hydrogen gas? d. Determine how many grams of hydrogen gas are produced from 27.2 g of hydrochloric acid? 5. Glucose, CH20.(s) burns in air...
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