The variation in the results of the experiment has to be given if the reaction was endothermic. Concept Introduction: Calorimetry can be defined as the measurement of changes in heat. Two types of Calorimetry are coffee cup calorimeter and bomb calorimeter. The change in heat of the system can be determined with the value of the heat capacity of the calorimeter. The heat capacity of the calorimeter can be given as, C cal = q cal ΔT Exothermic and Endothermic reactions: Heat is flow of thermal energy involving two bodies at various temperatures. The flow of thermal energy involving two bodies at various temperatures is called as heat. The flow of heat implies that energy is either released or absorbed on describing about energy changes that takes place during a process. Exothermic process is the chemical process in which heat is released to the surroundings. Endothermic process is the chemical process in which heat is absorbed from the surroundings.

Question

Want to see the full answer?

Answer 1

Question

Chapter 10, Problem 10.4VC

Interpretation Introduction

Interpretation:

The variation in the results of the experiment has to be given if the reaction was endothermic.

Concept Introduction:

Calorimetry can be defined as the measurement of changes in heat.

Two types of Calorimetry are coffee cup calorimeter and bomb calorimeter.

The change in heat of the system can be determined with the value of the heat capacity of the calorimeter.

The heat capacity of the calorimeter can be given as,

Ccal=qcalΔT

Exothermic and Endothermic reactions:

Heat is flow of thermal energy involving two bodies at various temperatures. The flow of thermal energy involving two bodies at various temperatures is called as heat. The flow of heat implies that energy is either released or absorbed on describing about energy changes that takes place during a process.

Exothermic process is the chemical process in which heat is released to the surroundings.

Endothermic process is the chemical process in which heat is absorbed from the surroundings.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Target Equation: (1) Mg(s) + 1/2 O2 (g) → MgO(s)Reactions: (2) MgO (s) + 2 HCl (aq) → MgCl2 (aq) + H2O (l) ΔH2 = ?(3) Mg (s) + 2 HCl (aq) → MgCl2 (aq) + H2 (g) ΔH3 = ?(4) H2 (g) + 1/2 O2 (g) → H2O (l) ΔH4 = -285.8 kJ Reaction Mass (grams) of MgO(s) Mass (grams) of Mg(s) Volume (mL) of HCl(aq) Concentration of HCl (mol/L) Initial Temp (°C) Final Temp (°C) 2 0.40 n/a 50.0 1.00 21.5 26.5 3 n/a 0.25 50.0 1.00 22.5 34.0 Using the data above, determine the enthalphy change (ΔH) for reactions (2) and (3). List any assumptions you make.Reaction (2): MgO (s) + 2 HCl (aq) → MgCl2 (aq) + H2O (l)Reaction (3): Mg (s) + 2 HCl (aq) → MgCl2 (aq) + H2 (g)

Consider the combustion of a single molecule of CH4(g),forming H2O(l) as a product. (a) How much energy, in J,is produced during this reaction? (b) A typical X-ray lightsource has an energy of 8 keV (see inside back cover forconversion between eV and J). Is the energy released by thecombustion of a CH4 molecule larger or smaller than the energyof an X-ray from this source?

2. Does an exothermic reaction go more to completion if I raise the temperature, lower the temperature, or perform the experiment at room temperature? Briefly explain.