1. Zinc metal reacts with aqueous hydrochloric acid to produce zinc(II) chloride and hydrogen gas. a. Write a balanced chemical equation including phase tags for this reaction. b. What volume of 0.118 M HCl is required to completely react with 0.103 g of solid zinc? c. When 0.103 g of solid zinc is combined with enough hydrochloric acid to make 50.0 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.5 °C to 23.7 °C. Determine \( q_{\text{rxn}} \) using 1.0 g/mL for the density of the solution and 4.184 J/g°C as the specific heat of the solution. d. Determine \( \Delta H_{\text{rxn}} \) when 1.00 mole of zinc reacts and add this information to your balanced chemical equation to make it a thermochemical equation. e. Use your thermochemical equation to determine \( \Delta H_{\text{rxn}} \) for the following reactions: i. 2 moles of Zn are reacted with excess hydrochloric acid ii. 5.67 g of Zn is reacted with excess hydrochloric acid iii. The reverse reaction occurs.

Since you have posted a question with multiple sub parts, we are entitiled to answer only first 3…

1. Zinc metal reacts with aqueous hydrochloric acid to produce zinc(II) chloride and hydrogen gas. a. Write a balanced chemical equation including phase tags for this reaction. b. What volume of 0.118 M HCI is required to completely react with 0.103 g of solid zinc? c. When 0.103 g of solid zinc is combined with enough hydrochloric acid to make 50.0 ml of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.5 °C to 23.7°C. Determine qran Using 1.0 g/ml for the density of the solution and 4.184 J/g°C as the specific heat of the solution.

1. Zinc metal reacts with aqueous hydrochloric acid to produce zinc(II) chloride and hydrogen gas. a. Write a balanced chemical equation including phase tags for this reaction. b. What volume of 0.118 M HCI is required to completely react with 0.103 g of solid zinc? c. When 0.103 g of solid zinc is combined with enough hydrochloric acid to make 50.0 ml of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.5 °C to 23.7°C. Determine qran Using 1.0 g/ml for the density of the solution and 4.184 J/g°C as the specific heat of the solution.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Many reactions are done in aqueous solution. How much NaOH would you need to weigh out to prepare 250.0 mL of a 0.200 M NaOH solution? A. 0.500 g B. 2.00 g C. 1.00 g D. 2.00 x 103 g
A student performs a titration by combining a 0.890 M hydrobromic acid solution with 65.0 mL of a 0.225 M manganese (III) hydroxide solution. A. Write the complete and balanced equation for the neutralization reaction of hydrobromic acid and manganese (III) hydroxide. DO NOT INCLUDE STATES OF MATTER. B. Calculate the volume of hydrobromic acid, in liters, that was used in this reaction. SHOW ALL WORK FOR FULL CREDIT. T T T F Paragraph 3 (12pt) += - E - T Arial EE T T, @ ABC fx Mashups HTML CSS Path: p Words:0 KA
I only need help with the highlighted ones please :)
If magnesium carbonate is combined with 100.0 mL of 0.50 mol/L hydrochloric acid solution, determine the mass of carbon dioxide gas produced. The unbalanced reaction is provided below. MgCO3 + HCI H,O + CO2 + MgCl,
A chemist wants to determine the concentration of an acidic solution. They start by placing 25.0 mL of the acid in a flask. Then, they titrate it with 13.0 mL of 0.10 M NaOH. a. How many moles of NaOH were added to the acid? b. Assuming the acid and base react in a 1:1 ratio, how many moles of acid are in the flask? c. What is the molarity of the unknown acid?
A solution with a total volume of 300 mL contains 37.85 g of NaCl. a. Determine the molarity of NaCl in the solution b. Suppose that the entire solution from part a is mixed with 400 mL of a different solution in order to perform a chemical reaction. Before this reaction happens, what is the concentration of NaCl in the combined solution? (Hint: The NaCl is being diluted by the other solution).
s) 0.250 g of HI is dissolved in 300. mL of a 0.00520 M solution of Ca(OH)2. (Assume this does not change the volume). The dissolved salts then proceed to react. a. What is the balanced chemical reaction (include states)? b. What type of reaction is this? С. What is the limiting reactant? d. How many grams of water are produced from this reaction?
6. Sodium sulfide reacts with hydrochloric acid to produce hydrogen sulfide and sodium chloride. How many grams of sodium sulfide are required for complete reaction with 15.0 mL of 0.250 M hydrochloric acid? The molar mass of sodium sulfide is 78.046 g/mol. (Hint: start by writing the balanced equation for the reaction.)
8. A student adds 22.36 mL of 1.366 x 10¹ M Mg(OH), in order to completely neutralize 25.00 mL of H₂PO acid. Calculate the original concentration of the acid solution.
Consider the neutralization reaction that takes place when hydrochloric acidreacts with aqueous sodium hydroxide.a. Write a conversion factor that relates moles of HCl to moles of NaOH forthis reaction.b. What is the minimum volume of 6.00 M HCl necessary to neutralizecompletely the hydroxide in 750.0 mL of 0.107 M NaOH
1. If 10. g of AgNO3 is available, what volume of 0.40 M AgNO3 solution can be prepared? Volume = mL? 2. A 7.52-g sample of a diprotic acid requires 179.0 mL of a 0.750 M NaOH solution for complete neutralization. Determine the molar mass of the acid. g/mol?
Please answer all