Question: At constant pressure, the decomposition of I mol of methanol, CHsOH, in the 19 gaseous phase requires 90.7 kJ of heat to produce carbon monoxide and hydrogen gases. a) Write the thermochemical equation for the reaction. b) Calculate the amount of heat required when 1.60 kg of gaseous methanol decomposes. c) The enthalpy change for a given sample of methanol for the above reaction is + 64.7 kJ. calculate the mass of hydrogen gas produced.

Question: At constant pressure, the decomposition of I mol of methanol, CHsOH, in the 19 gaseous phase requires 90.7 kJ of heat to produce carbon monoxide and hydrogen gases. a) Write the thermochemical equation for the reaction. b) Calculate the amount of heat required when 1.60 kg of gaseous methanol decomposes. c) The enthalpy change for a given sample of methanol for the above reaction is + 64.7 kJ. calculate the mass of hydrogen gas produced.

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

If 585 J of energy are absorbed by 125.6 g of aluminum and the initial temperature is from 20.0 oC, what is the final temperature? Is this endothermic or exothermic?
A chunk of gold (specific heat: 0.126) initially at 82.2 ˚C is placed in 75.5 g of water (specific heat: 184) initially at 22.0 ˚C. After a short time, both the water and the gold are at 41.0 ˚C. What was the mass of the gold?
If 67.2 J of heat is added to a 24.6 g sample of silver, how much will the temperature increase by? The specific heat of silver is 0.235 J/goC.
n the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction.A student heats 63.03 grams of chromium to 98.03 °C and then drops it into a cup containing 79.71 grams of water at 23.19 °C. She measures the final temperature to be 28.85 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.57 J/°C.Assuming that no heat is lost to the surroundings calculate the specific heat of chromium. Specific Heat (Cr) = ____________J/g °C.
Assuming no heat loss by the system, what will be the final temperature when 65.0 g of water at 10.0 oC are mixed with 73.0 g of water at 50.0 oC?
4. 30.0 g of a substance (molar mass: 46 g/mo) required 262 J of heat to raise its temperature from 32.0°C to 37.4°C. What is the specific heat per gram and per mole of this substance?
During an experiment, 98 g of water is used in the Styrofoam cup. The initial temperature of water was 23.7°C. A 39.9-g piece of metal with initial temperature of 100.3°C (after removing from the boiling water) is added to the calorimeter. The final temperature of water was 28.2°C. a) Calculate the specific heat of the metal. b) Identify the metal c) Calculate the percent error.
Show work to support your answer to this question. a) In a study of gaseous xenon, a chemist finds that 27.6 J of energy must be added to increase the temperature of 10.7 g of xenon from 22.7° C to 39.9° C. What is the experimental specific heat value for xenon gas? b) Using the specific heat you calculated for gaseous xenon, how much heat will be required to heat the 10.7 g sample of xenon from 39.9° C to 278.9° C?
Nitric acid and plumbous carbonate react: a) Write a balanced equation for this reaction. b) Calculate the enthalpy of the reaction. Show the enthalpy in the balanced equation (thermochemical equation). c) Calculate the enthalpy change of the reaction when 252 grams of nitric acid react with plumbous carbonate. NOTE: The enthalpies of formation for: Nitric Acid: -207 kJ/mole Plumbous Carbonate: -699 kJ/mole The Salt Formed: -421 kJ/mole.
E Reading list [References) Use the References to access important values if needed for this question. In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. A student heats 63.30 grams of nickel to 99.15 °C and then drops it into a cup containing 76.81 grams of water at 23.29 °C. She measures the final temperature to be 29.57 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.51 J/°C. Assuming that no heat is lost to the surroundings calculate the specific heat of nickel. Specific Heat (Ni) J/g°C. Submit Answer Try Another Version 1 item attempt remaining
In order to break water into hydrogen and oxygen, water is heated to more than 500°C. Which kind of reaction is this and why? It is exothermic because heat needs to be released by the reactants to form the products. It is endothermic because heat needs to be released by the reactants to form the products It is exothermic because heat needs to be absorbed by the reactants to form the products. It is endothermic because heat needs to be absorbed by the reactants to form the products.
Write the balanced chemical equation and draw an enthalpy diagram for the formation of 1 molof sodium chloride from its elements (heat is released).