Concept explainers
(a)
Interpretation:
The given reaction equation should be balanced.
Concept introduction:
In a balanced equation the number of atoms of each element as a reactant is equal to the number of atoms of that element as a product.
Coefficient is a number placed before a formula in a chemical equation.
A balanced equation should be obeying the law of conservation of mass. Law of conservation of mass states that, the number of atoms remains constant throughout the reaction, simply it can be stated as follows, “during a
(b)
Interpretation:
The given reaction equation should be balanced.
Concept introduction:
In a balanced equation the number of atoms of each element as a reactant is equal to the number of atoms of that element as a product.
Coefficient is a number placed before a formula in a chemical equation.
A balanced equation should be obeying the law of conservation of mass. Law of conservation of mass states that, the number of atoms remains constant throughout the reaction, simply it can be stated as follows, “during a chemical reaction atoms are neither be created nor be destroyed”.
(c)
Interpretation:
The given reaction equation should be balanced.
Concept introduction:
In a balanced equation the number of atoms of each element as a reactant is equal to the number of atoms of that element as a product.
Coefficient is a number placed before a formula in a chemical equation.
A balanced equation should be obeying the law of conservation of mass. Law of conservation of mass states that, the number of atoms remains constant throughout the reaction, simply it can be stated as follows, “during a chemical reaction atoms are neither be created nor be destroyed”.
(d)
Interpretation:
The given reaction equation should be balanced.
Concept introduction:
In a balanced equation the number of atoms of each element as a reactant is equal to the number of atoms of that element as a product.
Coefficient is a number placed before a formula in a chemical equation.
A balanced equation should be obeying the law of conservation of mass. Law of conservation of mass states that, the number of atoms remains constant throughout the reaction, simply it can be stated as follows, “during a chemical reaction atoms are neither be created nor be destroyed”.
(e)
Interpretation:
The given reaction equation should be balanced.
Concept introduction:
In a balanced equation the number of atoms of each element as a reactant is equal to the number of atoms of that element as a product.
Coefficient is a number placed before a formula in a chemical equation.
A balanced equation should be obeying the law of conservation of mass. Law of conservation of mass states that, the number of atoms remains constant throughout the reaction, simply it can be stated as follows, “during a chemical reaction atoms are neither be created nor be destroyed”.
Want to see the full answer?
Check out a sample textbook solution
Chapter 5 Solutions
EBK FUND.OF GENERAL,ORG.+BIO.CHEMISTRY
- For the following reaction, 4.91 grams of water are mixed with excess chlorine gas. The reaction yields 12.5 grams of hydrochloric acid.chlorine (g) + water (l) hydrochloric acid (aq) + chloric acid (HClO3) (aq) What is the theoretical yield of hydrochloric acid ? grams What is the percent yield of hydrochloric acid ? %arrow_forwardConsider the following reaction at 25°C with the ΔG°’ = +1800 J/mol for the forward reaction.The molar concentrations at the beginning of the reaction were [A] = 19 mM and [B] = 10 mM.After 1 hour, the concentrations were [A] = 16 mM and [B] = 13 mM. Calculate the ΔG of the reaction at the 1 hour timepoint. Please round to 1 decimal point.Gas constant = 8.315 J/mol Karrow_forwardWhich of the following correctly explains why the vapor pressure of water has to be included in the calculations? Some of the liquid water evaporates into the gas, and increases the total pressure generated by the trapped gas. As the H2(g) is bubbled up the reaction solution, some of the H2(g) molecules are solubilized by water in the aqueous solution, effectively decreasing the measured pressure above. The pressure contributed by the H2(g) is greater than the measured total pressure because of the contribution of partial pressure of water vapor. The pressure exerted by the evolved H2(g) is reduced because of the co-presence of water vapor, thus Pwater vapor has to be added to Pdry gas. Overview of the experiment:arrow_forward
- Calculate ΔG° (answer in kJ/mol) for each of the following reactions from the equilibrium constant at the temperature given. (d)CoO(s)+CO(g)⇌Co(s)+CO2(g) T=550°C Kp=4.90×102 (e)CH3NH2(aq)+H2O(l)⟶CH3NH3+(aq)+OH−(aq) T=25°C Kp=4.4×10−4 (f)PbI2(s)⟶Pb2+(aq)+2I−(aq) T=25°C Kp=8.7×10arrow_forward1. What is a “dNTP” and why are they included in the reaction mixture? 2. What will be the final concentration of 25 mM MgCl2, 5 mM dNTPs, and each 25 µM primer in one of the reaction tubes with the final volume of 50 microliters? Hint: use the information in the left column of Table 1 to help you with these calculations. (For one reaction) item 5.25x master mix – add things in order 32.7 µl ddH2O 171.7 µl 10 µl 5x reaction buffer 52.5 µl 3 µl 25 mM MgCl2 15.75 µl 0.5 µl 5 mM dNTPs 2.63 µl 1 µl 25 µM “forward” primer (#3012) 5.25 µl 1 µl 25 µM “reverse” primer (#3013) 5.25 µl 0.8 µl thermostable polymerase 4.2 µl (do not add until needed) Total: 49 µl Total: 257.3 µlarrow_forwardPotassium nitrate is widely used in industries. The reaction for the industrial production of KNO3 is summarized in the equation below; 4KCl + 4 HNO3 + O2 → 4 KNO3 + 2 Cl2 + 2 H2O Which of the following statements below is correct about the production of KNO3? a. A redox reaction; KCl is a reducing agent and O2 is an oxidizing agent b. A redox reaction; HNO3 is a reducing agent and Cl is an oxidizing agent c. Not a redox reaction d. A redox reaction; KCl is a reducing agent and KNO3 is an oxidizing agent e. A redox reaction; HNO3 is a reducing agent and KNO3 is an oxidizing agentarrow_forward
- When the following equation of a redox reaction in acidic solution is properly balanced, what are the coefficients for Cr2O72–, Fe2+ H+, Cr3+, Fe3+, and H2O, respectively? __Cr2O72– + __Fe2+ + __H+ --> __Cr3+ + __Fe3+ + __H2O (A) 1, 3, 14, 2, 3, 7; (B) 1, 6, 14, 2, 6, 7; (C) 2, 10, 14, 2, 10, 7; (D) 2, 12, 28, 4, 12, 14arrow_forwardFor this reaction: 6CO2 + 6H2O → C6H12O6 + 6O2, the products have 2760 kJ/mole more free energy than the reactants. So, which of the following statements best describes the reaction? a The reaction is endergonic because it converts molecules with less free energy to those with more free energy. b The reaction is exergonic because it converts molecules with less free energy to those with more free energy. c The reaction is exergonic because it converts molecules with more free energy to those with less free energy d The reaction is endergonic because it converts molecules with more free energy to those with less free energy.arrow_forwardThe formation constants at 25°C for Fe(CN)4-6 and Fe(EDTA)2– are 1.00 x 1037 and 2.10 x 1014, respectively. Answer the questions below. 1) Calculate K under standard conditions for the reaction Fe(EDTA)2−(aq) + 6CN−(aq) ----> Fe(CN)4−6(aq) + EDTA4−(aq) 2) Calculate ΔG° for the reaction. (kJ/mol)arrow_forward
- Two solutions, 250.0 mL of 1.00 M CaCl2(aq) and 250.0 mL of 1.00 M K2SO4(aq), are combined, and the temperature decreased by 2.40 degrees C. Determine qrxn per mole of CaSO4(s) formed in the reaction. A) +12.0 kJ/mol B) -12.0 kJ/mol C) +6.00 kJ/mol D) -6.00 kJ/molarrow_forwardConsider the following chemical equation whose delta(G) = 9kcal/mol: AC + BD ---> AB + CD what are the reactants and what are the products is this reaction spontaneous? How do you know? Is energy released or consumed by this reaction? If an enzyme, which catalyzes this reaction is added, what will happen to delta (G) If this reaction is coupled to another reaction, whose delta(G) is -12 kcal/mol, what will be the net delta(G) value? will the overall reaction be spontaneousarrow_forwardFor the reaction A → B at 298 K, the change in enthalpy is −7 kJ · mol−1and the change in entropy is −25 J · K−1 · mol−1. Is the reaction spontaneous? If not, should the temperature be increased or decreased to make the reaction spontaneous?arrow_forward
