$ A chemist measures the enthalpy change AH during the following reaction: 3 CH₂ Br(g) + NH3(g)-(CH3)₂N(1) + 3 HBr(g) Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction 12CH₂Br(g) + 4NH₂(g) → 4(CH₂),N(1) + 12HBr (g) 5(CH₂)₂N(1) + 15HBr (g) + 15HBr (g) 15CH, Br(g) + 5NH₂(g) 1 AH=73. kJ (CH₂) N() + 3HBr (g) 3CH, Br(g) + NH, (g) - ΔΗ kJ kJ

$ A chemist measures the enthalpy change AH during the following reaction: 3 CH₂ Br(g) + NH3(g)-(CH3)₂N(1) + 3 HBr(g) Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction 12CH₂Br(g) + 4NH₂(g) → 4(CH₂),N(1) + 12HBr (g) 5(CH₂)₂N(1) + 15HBr (g) + 15HBr (g) 15CH, Br(g) + 5NH₂(g) 1 AH=73. kJ (CH₂) N() + 3HBr (g) 3CH, Br(g) + NH, (g) - ΔΗ kJ 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 following thermochemical equation is for the reaction of water(l) to form hydrogen(g) and oxygen(g). 2H2O(l) -> 2H2(g) + O2(g) ΔH = 572 kJ How many grams of H2O(l) would be made to react if 110 kJ of energy were provided? _____ grams.
The propane fuel (C3H8) used in gas barbeques burns according to this thermochemical equation. C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) If a pork roast must absorb 1.5×103 kJ to fully cook, and if only 11 % of the heat produced by the barbeque is actually absorbed by the roast, what mass of CO2 is emitted into the atmosphere during the grilling of the pork roast?
When methanol, CH3OH, is burned in the presence of oxygen gas, O2, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH3OH(g)+32O2(g)⟶CO2(g)+2H2O(l)Δ?=−764 kJ How much methanol, in grams, must be burned to produce 943 kJ of heat? mass: g
Hi, hope you're doing great. I just need help with this question. Thank you.
For which reaction below does the enthalpy change under standard conditions correspond to a standard enthalpy of formation? 2H2(g) + C(s) → CHĄ(g) CO2(g) + C(s) → 2CO(g) 2NO2(3) → N204(g) CO(g) + H2O(g) → CO2(g) + H2(g) CO2(g) + H2(g) –→ CO(g) + H2O(g)
thermochemical 1. Use the equation given below to determine how much heat is released to the surrounding, surr when 350 g of propane, C₂Hg(g), is burnt completely in a backyard barbecue at 25°C. C3H8(g) +50₂(g) → 3CO₂(g) + 4H₂O(1) AH = -2220 kJ.
Solid aluminum metal and gaseous oxygen combine in the reaction below to form aluminum oxide: 2Al(s) + 3O2(g) → 2 Al2O3(s) If ∆Hº for this reaction is -3353.4 kJ, what is the standard enthalpy of formation, Hfº, for solid Al2O3 in kJ? Express your answer to one decimal place. Do NOT include units!
A chemist measures the enthalpy change AH during the following reaction: 2 Al(OH)3(s)-Al₂O3(s) + 3H₂O(1) ΔΗ = 41. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ALO3(s) + 3H₂O(1)→ 2Al(OH), (s) 4A1 (OH), (s) → 2AL₂O₂ (s) + 6H₂0 (1) — Al₂O3(s) + H₂O0(1) — AI(OH), (s) ΔΗ kJ KJ X S
Hydrogen sulfide, H2S, is a foul-smelling gas. It burns to form sulfur dioxide. 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔH = −1036 kJ Calculate the enthalpy change to burn 30.5 g of hydrogen sulfide. kJ
Baking soda is sodium bicarbonate (NaHCO3). When you heat baking soda, it breaks down into sodium carbonate powder (Na2CO3), water vapor, and carbon dioxide. The enthalpy of this reaction is 129 kJ. Write a correct thermochemical equation for this reaction, explain how you came up with this equation, and explain what it tells you about the reaction.
Using Hess's Law to calculate net reaction enthalpy Nitric oxide (NO) can be formed from nitrogen, hydrogen and oxygen in two steps. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3H₂(g) → 2NH3(g) In the second step, ammonia and oxygen react to form nitric oxide and water: 4 NH3(g) + 50₂(g) → 4NO(g) + 6H₂O(g) ΔΗ= - 905. kJ ΔΗ= - 92. kJ Calculate the net change in enthalpy for the formation of one mole of nitric oxide from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ. kJ X S
1