What data should be plotted to show that experimental concentration data fits a first-order reaction? A) 1/[reactant] vs. time B) [reactant) vs. time C) In[reactant] vs. time D) In(k) vs. 1/1

Answers

Answer 1
Answer:

The data that should be plotted to show that experimental concentration data fits a first-order reaction is: C. In [reactant] vs. time.

What is a first-order reaction?

A first-order reaction can be defined as a type of chemical reaction in which the reaction rate (rate of reaction) is directly proportional to the concentration of the reacting chemical substance or elements.

Mathematically, the integrated rate law equation for a first-order reaction is given by this formula:

A=A_o e^(kt)

Where:

  • A is the concentration after time (t).
  • A_o is the initial concentration of the reactant.
  • t is the time.
  • k is the rate constant.

Taking the ln of both sides, we have:

ln(A)=ln(A_o)-kt

Therefore, the data that should be plotted to show that experimental concentration data fits a first-order reaction is In[reactant] versus time.

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Answer 2
Answer:

Answer:

C) In[reactant] vs. time

Explanation:

For a first order reaction the integrated rate law equation is:

A = A_(0)e^(-kt)

where A(0) = initial concentration of the reactant

A = concentration after time 't'

k = rate constant

Taking ln on both sides gives:

ln[A] = ln[A]_(0)-kt

Therefore a plot of ln[A] vs t should give a straight line with a slope = -k

Hence, ln[reactant] vs time should be plotted for a first order reaction.


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Answers

the answer for your question is Chemical energy is spontaneously converted to electrical energy.

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Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer. ResetHelp 1. NaCl ; ionic bonds{\rm NaCl} ; blank are stronger than the blank in {\rm HCl}. are stronger than the dispersion forces{\rm NaCl} ; blank are stronger than the blank in {\rm HCl} . in HCl. 2. H2O ; hydrogen bonds{\rm H_2O} ; blank are stronger than the blank in {\rm H_2Se}. are stronger than the dispersion forces{\rm H_2O} ; blank are stronger than the blank in {\rm H_2Se}. in H2Se. 3. NH3 ; hydrogen bonds{\rm NH_3} ; blank are stronger than the blank in {\rm PH_3}. are stronger than the dipole-dipole attractions{\rm NH_3} ; blank are stronger than the blank in {\rm PH_3}. in PH3. 4. HF ; hydrogen bonds{\rm HF} ; blank are stronger than the blank in {\rm F_2}. are stronger than the dispersion forces{\rm HF} ; blank are stronger than the blank in {\rm F_2}. in F2.

Answers

Answer:

The ionic bond in NaCl are stronger than the stronger than the dispersion forces in HCl.

The hydrogen bonds in H2O are stronger than the dispersion forces in H2Se

Hydrogen bonds in NH3 are stronger than the dipole-dipole attractions in PH3.

Hydrogen bonds in HF are stronger than the dispersion forces in F2

Explanation:

Ionic bonds occur in molecules with high differences in their electronegative value where there are actual transfer of electrons. HCl has a bond which is involved in the sharing of electrons.

Hydrogen bonds are present in H2O which is stronger than the dispersion forces.

PH3 is a larger molecule with greater dispersion forces than ammonia, NH3 has very polar N-H bonds leading to strong hydrogen bonding. This dominant intermolecular force results in a greater attraction between NH3 molecules than there is between PH3 molecules.

F2 is a non-polar molecule, therefore they have London dispersion forces between molecules while HF has a hydrogen bond because F is highly electronegative.

Final answer:

Ionic bonds are stronger than dispersion forces in HCl, while hydrogen bonds are stronger than dispersion forces in H2Se, PH3, and F2.

Explanation:

In the given sentences, the blanks represent the types of intermolecular forces. The options given are ionic bonds, hydrogen bonds, dispersion forces, and dipole-dipole attractions. Ionic bonds are stronger than the dispersion forces in HCl. Hydrogen bonds are stronger than the dispersion forces in H2Se. Hydrogen bonds are stronger than the dipole-dipole attractions in PH3. Hydrogen bonds are stronger than the dispersion forces in F2.

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(NH4)2S(aq)+SrCl2(aq)→Express your answer as a chemical equation. Enter NOREACTION if no reaction occurs. Identify all of the phases in your answer.

Answers

The chemical equation will be;  

(NH4)2S(aq)+SrCl2(aq)→ 2 NH4Cl(aq) + SrSO4(s)

Further Explanation  

Chemical equation  

  • A chemical equation is an equation showing chemical symbols of reactants and those of products. They represent a chemical reactions between reactants to form products.
  • For example; (NH4)2S(aq)+SrCl2(aq)→ 2 NH4Cl(aq) + SrSO4(s), where (NH4)2S and SrCl2 are reactants while NH4Cl and SrSO4 are products.

Types of chemical reactions  

Precipitation reaction

  • Precipitation reactions are reactions which involves the formation of a precipitate as one of the products. A precipitate is a compound that is insoluble in water.
  • An example of a precipitation reaction is; (NH4)2S(aq)+SrCl2(aq)→ 2 NH4Cl(aq) + SrSO4(s), where the compound SrSO4 is the precipitate.  

Displacement reaction

  • Displacement reactions are reactions where ions replace other ions in their compounds.
  • For example; ; (NH4)2S(aq)+SrCl2(aq)→ 2 NH4Cl(aq) + SrSO4(s) is an example of a double displacement reaction where NH4+ takes the place of Sr ions in SrCl2 and Sr2+ takes the place of NH4+ in (NH4)2SO4.

Decomposition reaction  

  • Decomposition reactions are reactions which involves break down of a compound to its constituent’s elements or other compounds by use of a catalyst or heat.
  • For example; Decomposition of lead (II) nitrate using heat to get lead (ii) oxide, oxygen and nitrogen (IV) oxide.

Neutralization reaction  

  • Neutralization reactions are reactions that involve reacting a base or an alkali and an acid to form a salt and water as the only product.

Redox reactions

  • Redox reactions are reactions that involve both reduction and oxidation. Some species in reactions undergo reduction while others undergo oxidation.  

Keywords: Chemical reactions, precipitation reactions, chemical equations

Learn more about:

Level: High school  

Subject: Chemistry  

Topic: Chemical reactions  

Sub-topic: Precipitation reactions  

Final answer:

No reaction is expected when (NH4)2S(aq) and SrCl2(aq) are mixed, as solubility rules suggest no insoluble salts will form, leading to NOREACTION.

Explanation:

When (NH4)2S(aq) and SrCl2(aq) are mixed together, we expect a reaction where the cations (NH4+ and Sr2+) and anions (S2- and Cl-) exchange partners if any of them can form an insoluble salt. Looking at solubility rules, we know that most sulfides are insoluble except those of alkali metals and ammonium, and most chlorides are soluble except for Ag+, Pb2+, and Hg22+. Given that neither NH4+ nor Sr2+ forms an insoluble chloride and SrS is not listed as an insoluble sulfide, we can predict that no visible reaction will occur when these solutions are mixed. Therefore, the chemical equation to represent this mixture is NOREACTION.

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Whats the difference between china and Europe

Answers

Answer:

the difference is they arnt close

Explanation:

Answer:

China is communist, Europe isn't.

Explanation:

Consider the neutralization reaction 2HNO3(aq) + Ba(OH)2 ( aq ) ⟶ 2H2O ( l ) + Ba ( NO3)2 ( aq ). A 0.125 L sample of an unknown HNO 3 solution required 32.3 mL of 0.200 M Ba ( OH ) 2 for complete neutralization. What is the concentration of the HNO 3 solution?

Answers

Answer:

The concentration of the HNO3 solution is 0.103 M

Explanation:

Step 1: Data given

Volume of the unknow HNO3 sample = 0.125 L

Volume of 0.200 M Ba(OH)2 = 32.3 mL = 0.0323 L

Step 2: The balanced equation

2HNO3(aq) + Ba(OH)2 ( aq ) ⟶ 2H2O ( l ) + Ba( NO3)2 (aq)

Step 3:

n2*C1*V1 = n1*C2*V2

⇒ n2 = the number of moles of Ba(OH)2 = 1

⇒ C1 = the concentration of HNO3 = TO BE DETERMINED

⇒ V1 = the volume of the HNO3 solution = 0.125 L

⇒ n1 = the number of moles of HNO3 = 2

⇒ C2 = the concentration of Ba(OH)2 = 0.200 M

⇒ V2 = the volume of Ba(OH)2 = 0.0323 L

1*C1 * 0.125 L = 2*0.200M * 0.0323 L

C1 = (2*0.200*0.0323)/0.125

C1 = 0.103 M

The concentration of the HNO3 solution is 0.103 M

A biochemist studying breakdown of the insecticide DDT finds that it decomposes by a first-order reaction with a half-life of 12.0 yr. How long does it take DDT in a soil sample to decompose from 809 ppbm to 10.0 ppbm (parts per billion by mass)

Answers

Answer:

76.0 years

Explanation:

Step 1: Given data

  • Half-life (t1/2): 12.0 y
  • Initial concentration of DDT ([A]₀): 809 ppbm
  • Final concentration of DDT ([A]): 10.0 ppbm
  • Time elapsed (t): ?

Step 2: Calculate the rate constant (k)

We will use the following expression.

k = ln 2/ t1/2 = ln 2 / 12.0 y = 0.0578 y⁻¹

Step 3: Calculate the time elapsed

For a first-reaction order, we will use the following equation.

ln [A]/[A]₀ = -k × t

t = ln [A]/[A]₀ / (-k)

t = (ln 10.0 ppbm/809 ppbm) / (-0.0578 y⁻¹)

t = 76.0 y