ydrogen cyanide is a highly poisonous, volatile liquid. It can be prepared by the reaction CH4 (9) +NH3 (9)HCN(9) +3H, (9) what is the heat of reaction at constant pressure? Use the following thermochemical equations: N2 (g) + 3H2 (g) 2NH3 (9); AH =-91.8 kJ C(graphite) + 2H2 (g) → CH4(g); AH = -74.9 kJ H2 (g) + 2C(graphite) + N2 (9) → 2HCN(9); AH = 270.3 kJ Heat = kJ

ydrogen cyanide is a highly poisonous, volatile liquid. It can be prepared by the reaction CH4 (9) +NH3 (9)HCN(9) +3H, (9) what is the heat of reaction at constant pressure? Use the following thermochemical equations: N2 (g) + 3H2 (g) 2NH3 (9); AH =-91.8 kJ C(graphite) + 2H2 (g) → CH4(g); AH = -74.9 kJ H2 (g) + 2C(graphite) + N2 (9) → 2HCN(9); AH = 270.3 kJ Heat = kJ

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

the first picture is the question and the second picture is the expected answer (please apply thermochemistry and their formula)
Thermochemistry and Stoichiometry
Given the following thermochemical equations: C2H29) + 5 02(9) 2C02(g) + H201) AH° = -1229.5 kJ AH° = -393.5 kJ C(6) + 02(g) → C02(g) 1 H2(9) +5 02(9) → H20) AH° = -285.5 kJ 2 Calculate the enthalpy (in kJ) for this reaction: 206) + H2(g) → C,H2(9)
Hydrogen cyanide is a highly poisonous,volatile liquid.One way in which it can be prepared is by the reaction: CH4 + NH3 producing HCN + 3H2 Use Hess' Law and the following thermochemical equations to find the heat of the above reaction at constant pressure. N2+3H2 producing 2NH3 ;change in heat=-91,8 KJ C(graphite)+2H2 producing CH4; change in heat=-74,9 KJ H2+2C(graphite)+N2 producing 2HCN; change in heat =270,3 KJ
THERMODYNAMICS: Calculate the value of AH (in kJ) for the reaction, 2AR3 (g) + Q (s)→ A2R4 (g) + QR2 (s) given the following hypothetical thermochemical equations: 2AR3 (g) + 2AX (g) → A2R4 (g) + 2XAR (g) AH = -87.2 kJ AX (g) + ½R2 (g) → XAR (g) AH = -157.3 kJ Q (s) + R2 (g) – QR2 (s) AH = -510.2 kJ (Round off the final answer to ONE decimal place. Do not include the unit.)
Acetylene, C2H2, is a gas commonly used in welding. It is formed in the reaction of calcium carbide, CaC2, with water. Given the thermochemical equations, calculate the value of AH'† for acetylene in units of kilojoules per mole. CaO(s) + H2O(1) → Ca(OH)2(s) AH°=-65.3 kJ 2CaO(s) + 5C(s) → 2CAC2(s) + CO2(g) AH°=+753 kJ CaCO3(s) → CaO(s) + CO2(g) AH° = +178 kJ CaC2(s) + 2H2O(1) → Ca(OH)2(s) + C2H2(g) AH°=-126 kJ C(s) + O2(3) → CO2(3) AH°=-393.5 kJ 2H20(1) → 2H2(g) + O2(g) AH°=+572 kJ i kJ/mol
Use the thermochemical equations shown below to determine the enthalpy for the reaction: C3H8(g) + 502(g) +3CO 2 + 4H2O(1) CO2 C(graphite) + 02 HE = 221.6KJ H2(g) + 1/2O2(g) H2O(1) HE= -160.3KJ 3 C(graphite) + 4 H2(g) C3H8(g) HE= -58.5KJ
A bomb calorimeter can be used to measure the enthalpy of reaction for combustions, such as the combustion of diborane represented by the following balanced equation:B2H6(g)+3O2(g)➔B2O3(s)+3H2O(g)ΔHcombustion for this process is –1958 kJ/mol. Assume that 0.411 g of diborane is combusted in a calorimeter whose heat capacity (Ccalorimeter) is 7.854 kJ/°C at 22.61°C. What is the final temperature of the calorimeter? The answer is not 18.922°C
The following thermochemical equation is for the reaction of Fe,0, (s) with hydrogen (g) to form iron(s) and water (g). Fe₂O₂ (s) + 4H₂(g) 3Fe(s) + 4H₂O(g) AH = 151 kJ Use the References to access important values if needed for this question. When 86.8 grams of Fe₂O4(s) react with excess hydrogen(g). Hint: An amount of energy is expressed as a positive number. The sign of AH in the thermochemical equation indicates whether the energy is absorbed or evolved. Submit Answer kJ of energy are
The balanced combustion reaction for C,H, is 2C,H,(1) + 15 0,(g) → 12 CO,(g) + 6 H,O(1) + 6542 kJ If 7.600 g C,H, is burned and the heat produced from the burning is added to 5691 g of water at 21 °C, what is the final temperature of the water? final temperature: °C
12. Calculate the heat of formation for the following reactions from the standard enthalpies of formation listed in Appendix 2: (a) 2H2(g) + O2 (g) 2H20(1) (b) 2C2H2 (g) + 502(g) 4CO2(g) + 2H2O(1) (c) 2C2H4(g) + 3 02 (g)- 2002(9) acOt + 2H2O(1)
THERMODYNAMICS: Calculate the value of AH (in kJ) for the reaction, 2AR3 (g) + Q (s) → A2R4 (g) + QR2 (s) given the following hypothetical thermochemical equations: 2AR3 (g) + 2AX (g) → A2R4 (g) + 2XAR (g) AH = -89.3 kJ AX (g) + ½R2 (g) → XAR (g) AH = -152.2 kJ Q (s) + R2 (g) –→ QR2 (s) AH = -533.9 kJ (Round off the final answer to ONE decimal place. Do not include the unit.)