In a generic chemical reaction involving reactants A and B and products C and D, aA + 6B>cC+ dD, the standard enthalpy A;H° of the reaction is given by A,H° = CA¢H° (C) +dA; H° (D) -aA; H°(A) – bA;H° (B) Notice that the stoichiometric coefficients, a, b, c d, are an important part of this equation. This formula is often generalized as follows, where the first sum on the right-hand side of the equation is a sum over the products and the second sum is over the reactants: A;H° =Lproducts nAç H° – Ereactants mAç H° where m and n represent the appropriate stoichiometric coefficients for each substance. Part A What is A,H° for the following chemical reaction? CO(g) + NH3(9)→HCN(g)+H2O(g) You can use the following table of standard heats of formation (Af H°) to calculate the enthalpy of the given reaction. Standard Heat of Standard Heat of Element/ Compound Formation Element/ Compound Formation (kJ mol-1) (kJ mol-') H(g) 218 N(g) 473 H2(9) O2 (g) NH3(g) 45.90 O(g) 249 CO(g) -110,5 H2O(g) -241.8 C(g) 71 HCN(g) 130.5 C(s) HNO3 (aq) -206.6 Express the standard enthalpy of reaction to three significant figures and include the appropriate units.

In a generic chemical reaction involving reactants A and B and products C and D, aA + 6B>cC+ dD, the standard enthalpy A;H° of the reaction is given by A,H° = CA¢H° (C) +dA; H° (D) -aA; H°(A) – bA;H° (B) Notice that the stoichiometric coefficients, a, b, c d, are an important part of this equation. This formula is often generalized as follows, where the first sum on the right-hand side of the equation is a sum over the products and the second sum is over the reactants: A;H° =Lproducts nAç H° – Ereactants mAç H° where m and n represent the appropriate stoichiometric coefficients for each substance. Part A What is A,H° for the following chemical reaction? CO(g) + NH3(9)→HCN(g)+H2O(g) You can use the following table of standard heats of formation (Af H°) to calculate the enthalpy of the given reaction. Standard Heat of Standard Heat of Element/ Compound Formation Element/ Compound Formation (kJ mol-1) (kJ mol-') H(g) 218 N(g) 473 H2(9) O2 (g) NH3(g) 45.90 O(g) 249 CO(g) -110,5 H2O(g) -241.8 C(g) 71 HCN(g) 130.5 C(s) HNO3 (aq) -206.6 Express the standard enthalpy of reaction to three significant figures and include the appropriate units.

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

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 68E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of...

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In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of 25.00C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.34C. Assuming the solution has a heat capacity of 4.18 J/C g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
Given that the standard enthalpy of formation of HI(aq) is −55 kJ mol−1, what is the value of ΔfH⦵(I−, aq)?
Given that the standard enthalpy of formation of HCl(aq) is −167 kJ mol−1, what is the value of ΔfH⦵(Cl−, aq)?
Express the standard enthalpy of the reaction in 4 sig figs and include the appropriate units.
When 0.560g of NaF(s) reacts with excess F2(g) to form NaF(s), 13.8kJ of heat is evolved at standard-state conditions. What is the standard enthalpy of foundation (H*f) of NaF(s)?
In a generic chemical reaction involving reactants A and B and products C and D, aA+bB→cC+dD, the standard enthalpy ΔH∘rxn of the reaction is given by ΔH∘rxn=cΔH∘f(C)+dΔH∘f(D) −aΔH∘f(A)−bΔH∘f(B) Notice that the stoichiometric coefficients, a, b, c, d, are an important part of this equation. This formula is often generalized as follows, where the first sum on the right-hand side of the equation is a sum over the products and the second sum is over the reactants: ΔH∘rxn=∑productsnΔH∘f−∑reactantsmΔH∘f where m and n represent the appropriate stoichiometric coefficients for each substance. What is ΔH∘rxnΔHrxn∘ for the following chemical reaction? CO(g)+NH3(g)→HCN(g)+H2O(g) You can use the following table of standard heats of formation (ΔH∘f)(ΔHf∘) to calculate the enthalpy of the given reaction. Element/ Compound Standard Heat of Formation (kJ/mol) Element/ Compound Standard Heat of Formation (kJ/mol) H(g) 218218 N(g) 473473 H2(g) 00 O2(g) 00 NH3(g) −45.90 O(g) 249 CO(g)…
The standard enthalpy change of combustion [to CO2(g) and H2O()] at 25°C of the organic solid isophthalic acid, C8H6O4(s), is determined to be -3185.8 kJ mol-1. What is the Hf° of C8H6O4(s) based on this value?
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At constant pressure and 25℃, what is ∆H° for the following reaction 2C2H6 (g)+7O2 (g)→4CO2 (g)+H2O(l) If the complete consumption of 38.2g of C2H6 liberates 1981 kJ of heat energy?
5.25mL of a 1.35M solution of sodium hydroxide is combined with 6.90mL of a 810.mM solution of monoprotic acid, in a calorimeter, resulting in the temperature increasing from 19.7°C to 23.0°C. Thus, the standard enthalpy of this neutralisation is exothermic by what amount (in units of kcalmol-1)?
The standard nthalpy of neutralization of a weak hydrogen cyanide acid, HCN (aq), by a stong base, NaOH (aq), is -12.1 kj/mol. Using Hess's Law and your experimental data on standard enthalpy of neutralization from Part A to calculate standard enthalpy of ionization of HCN (aq): HCN (aq) --> H+ (aq) + CN- (aq)), Hioniz (HCN) Part A= enthaply of neut= -60.066 kj/mol
An equilibrium constant for the reaction decreases twice when temperature increases from 300 K to 350 K. What is the standard enthalpy for the reaction? Round off your answer to 3 significant figures and enter it correct units.