4. When 100 ml of 1.0 M HCl is added to 2 g of Na₂CO3 crystals, carbon dioxideis evolved. All of the following will increase the initial rate of the reactionEXCEPTa. addition of 100 mL of 2.0 M HCl instead of 1.0 M HCI.b. addition of 200 mL of 1.0 M HCl instead of 100 mL.c. addition of 100 mL of 1.0 M HCl to powdered Na₂CO3 instead ofcrystalline Na₂CO3.d. addition of 100 mL of hot 1.0 M HCl instead of 1.0 M HCl at roomtemperature.e. addition of 200 mL of 2.0 M HCl instead of 100 mL of 1.0 M HCl.

The objective of this question is to chose the given options that will not increase the rate of…

Answered: 4. When 100 ml of 1.0 M HCl is added to…

4. When 100 ml of 1.0 M HCl is added to 2 g of Na2CO3 crystals, carbon dioxide is evolved. All of the following will increase the initial rate of the reaction EXCEPT

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 68QAP: . Lead(II) chloride, PbCl2(s), dissolves in water to the extent of approximately 3.6102Mat 20 °C....

See similar textbooks

Related questions

Q: Which of the following will decrease the activation energy, Ea, of a reaction? O Decreasing the…

A: To find: reason for decrease in activation energy of a reaction.

Q: 8. Answer the following questions with words or phrases: a.) The proposes that in order for a…

A: NOTE: Since you've posted multiple sub-parts, we'll solve only the first three sub-parts for you. To…

Q: Images

A: Given that : We have to identify the correct statement for the above sentence out of the below four…

Q: Given the reaction SO2 + CO2 --> SO + CO, which atoms must collide for the reaction to occur…

Q: For the reaction 4A(g) + 3B(g) → 2C(g) the following data were obtained at constant temperature:…

A: Order of a reaction is the sum of the power to which concentration of reactants are raised in rate…

Q: A catalyst will... provide an alternate. pathway for a reaction that requires less activation energy…

Q: Explain on a molecular level how temperature, reactant concentration and the presence of a catalyst…

A: The rate of the reaction is affected by the following factors: Temperature Reactant concentration…

Q: 16. How can the effect of temperature on the reaction rate be explained by collision theory?

A: Collision theory is a principle in chemistry that explains how chemical reactions occur and why…

Q: reaction rates (speed) can be enhanced by catalysts. explain how a catalyst could affect rate of a…

A: A catalyst added in any reaction enhances the rate of reaction but does not participate in the…

Q: In terms of collision theory, When is a chemical reaction occurs? A. chemical bonds are broken by…

Question

4. When 100 ml of 1.0 M HCl is added to 2 g of Na₂CO3 crystals, carbon dioxide
is evolved. All of the following will increase the initial rate of the reaction
EXCEPT
a. addition of 100 mL of 2.0 M HCl instead of 1.0 M HCI.
b. addition of 200 mL of 1.0 M HCl instead of 100 mL.
c. addition of 100 mL of 1.0 M HCl to powdered Na₂CO3 instead of
crystalline Na₂CO3.
d. addition of 100 mL of hot 1.0 M HCl instead of 1.0 M HCl at room
temperature.
e. addition of 200 mL of 2.0 M HCl instead of 100 mL of 1.0 M HCl.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1: Writing the objective

VIEW

Step 2: Explanation

VIEW

Solution

VIEW

Step by step

Solved in 3 steps with 13 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Why are there no changes specified for NH4HS in Exercise 13.62, part (e)? What property of NH4HS does change?
What is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.
. The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of Fe(OH)3in moles per liter and in grams per liter.
How is the strength of an acid related to the position of its ionization equilibrium? Write the equations for the dissociation (ionization) of HCI, HNO3, and HClO4in water. Since all these acids are strong acids, what does this indicate about the basicity of the Cl-, NO3, and ClO4ions? Are aqueous solutions of NaCl, NaNO3, or NaClO4basic?
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
The following question is taken from a Chemistry Advanced Placement Examination and is used with the permission of the Educational Testing Service. Solve the following problem: MgF2(s)Mg2+(aq)+2F(aq) In a saturated solution of MgF2 at 18 C, the concentration of Mg2+ is 1.21103M . The equilibrium is represented by the preceding equation. (a) Write the expression for the solubility-product constant, Ksp, and calculate its value at 18 C. (b) Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2 solution at 18 C to which 0.100 mol of solid KF has been added. The KF dissolves completely. Assume the volume change is negligible. (c) Predict whether a precipitate of MgF2 will form when 100.0 mL of a 3.00103 -M solution of Mg(NO3)2 is mixed with 200.0 mL of a .2.00103 -M solution of NaF at 18 C. Show the calculations to support your prediction.. (d) At 27 C the concentration of Mg2+ in a saturated solution of MgF2 is 1.17103M . Is the dissolving of MgF2 in water all endothermic or an exothermic process? Give an explanation to support your conclusion.
In the reaction in Exercise 12.33, another trial was carried out. The reaction began with an initial concentration of N2 equal to the initial concentration of NO. Each had a concentration of 0.100 mol L-1. WTat were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L'1 ofO2, what were the equilibrium concentrations of all species?
A solution is prepared by adding 0.10 mole of Ni(NH3)6 Cl2 to 0.50 L of 3.0 M NH3. Calculate [Ni(NH3)62+] and [Ni2+] in this solution. Koverall for Ni(NH3)62+ is 5.5 108. That is, 5.5108=[Ni(NH3)62+][Ni2+][NH3]6 for the overall reaction Ni2+(aq)+6NH3(aq)Ni(NH3)62+(aq)
Ksp for CaSO4 at 100C is estimated to be1.6105. At 25C, 0.915 g of CaSO4 is added to one liter of water. (a) Will all the CaSO4 dissolve? (b) If the solution is heated to 100C, will all the CaSO4 dissolve?
. Under what circumstances can we compare the solubilities of two salts by directly comparing the values of their solubility products?
Write the reaction quotient expression for the ionization of NH3 in water.
How many grams of Milk of Magnesia, Mg(OH)2 (s) (58.3 g/mol), would be soluble in 200 mL of water. (KSP=7.11012). Include the ionic reaction and the expression for Ksp, in your answer. (Kw=11014=[H3O+][HO]).