(a)
Interpretation:
The balanced chemical equation for the reaction of phosphorus with chlorine to form
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 enthalpy change of the reaction of
Concept Introduction:
Bond energy or more correctly the bond dissociation enthalpy is the enthalpy change when breaking a bond in a molecule with the reactant and products in the gas phase.
Enthalpy of formation:
(c)
Interpretation:
The bond dissociation enthalpy for
Concept Introduction:
Bond energy or more correctly the bond dissociation enthalpy is the enthalpy change when breaking a bond in a molecule with the reactant and products in the gas phase.
Enthalpy of formation:
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Chapter 8 Solutions
Chemistry & Chemical Reactivity
- Compounds such as NaBH4, Al(BH4)3, and LiAlH4 are complex hydrides used as reducing agents in many syntheses. (a) Give the oxidation state of each element in these compounds. (b) Write a Lewis structure for the polyatomic anion in NaBH4, and predict its shape.arrow_forwardThe elements sodium, aluminum, and chlorine are in the same period. (a) Which has the greatest electronegativity? (b) Which of the atoms is smallest? (c) Which is the largest possible oxidation state for each of these elements? (d) Will the oxide of each element in the highest oxidation state (write its formula) be acidic, basic, or amphoteric?arrow_forwardIn a hydrogen molecule, the two hydrogen atoms are held together by a single bond with a bond energy of 436 kJ/mol of hydrogen. In other words, to break the H-H bonds in one mole of molecular hydrogen requires the expenditure of 436 kJ of energy. Using the balanced chemical equation for the formation of water from oxygen and hydrogen (shown above), and interpreting the stoichiometric coefficients as mole amounts, how much energy must be expended in breaking the H-H bonds? kJarrow_forward
- How many kj of heat are needed to produce 6.47 g NH 3 ? 4NO+6H 2 O 4NH 3 +5O 2; triangle H=906 kJarrow_forwardUsing Lewis symbols and Lewis structures, diagram the formation of SiCl4 from Si and Cl atoms.arrow_forwardAcetylene (C2H2) and nitrogen (N2) both contain a triplebond, but they differ greatly in their chemical properties.(a) Write the Lewis structures for the two substances. (b) By referring to Appendix C, look up the enthalpies of formationof acetylene and nitrogen. Which compound is more stable?(c) Write balanced chemical equations for the completeoxidation of N2 to form N2O5(g) and of acetylene to formCO2(g) and H2O(g). (d) Calculate the enthalpy of oxidationper mole for N2 and for C2H2 (the enthalpy of formationof N2O5(g) is 11.30 kJ/mol). (e) Both N2 and C2H2 possesstriple bonds with quite high bond enthalpies (Table 8.3).Calculate the enthalpy of hydrogenation per mole for bothcompounds: acetylene plus H2 to make methane, CH4;nitrogen plus H2 to make ammonia, NH3.arrow_forward
- 29) a 2.50 g sample of gallium absorbe 4.56 x 10^-3 kj of heat upon heating. What is the change of temperature in unit of degree Celsius of the gallium sample? Specific heat of gallium is 0.372 J/g °Carrow_forwardThe first four ionization energies of an element X are 578, 1817, 2745, and 11,577 kJ·mol–1. What is the most likely formula for the most stable ion of Xarrow_forward(b) aluminum AGO = AH° = || hydride: AIH 3(S)→ Al(s) + 3/2 H₂(g) kJ/mol kJ/molarrow_forward
- (e) The mean bond enthalpy for chlorine is +242 kJ mol·l and that for fluorine is +158 kJ mol-". The enthalpy of formation of CIF (g) is 56 kJ mol·l (ii) Calculate the enthalpy of formation of, gaseous Chlorine Trifluoride, CIF3 (g), using the bond enthalpy value you obtained in part (i). (iii) The bond enthalpy of CIF3 calculated in part (ii) is likely to be different than that determined from experiment. Explain.arrow_forwardCompounds such as NaBH₄, Al(BH₄)₃, and LiAlH₄ arecomplex hydrides used as reducing agents in many syntheses.(a) Give the oxidation state of each element in these compounds.(b) Write a Lewis structure for the polyatomic anion in NaBH₄,and predict its shape.arrow_forwardWhat is the equation for the formation reaction for gaseous hydrazine, N2H4, at 25ºC and 1 atm pressure?arrow_forward
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