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Justify and compare how a change (rise and drop) in temperature will affect how spontaneous the reaction will become.
Using the Clayperon equation from part a, justify the difference in the solid-liquid phase boundary for water versus most other material.
How much heat is involved in the complete combustion of 12.5L C3H8(g) at 25 degrees C and 790 mmHg?
75.0g of Ca(AW = 40.08) are reacted with 40.0 H20 (MW = 18.02) according to the above equation if 30.0 L of H2 (g)(MW = 2.016) are produced at 20 0C.
When a 3.88g sample of solid ammonium nitrate dissolves in 60g of water in a coffee-cup calorimeter, the temperature drops from 23 degrees C to 18.4 degrees C.
The complete combustion of acetic acid, HC2H3O2(l) to form H2O(l) and CO2(g) at a constant pressure releases 871.7kJ of heat per mole of HC2H3O2.
What mass of water at 100 degrees Celsius would raise the temperature of 30.00g of water at 23.0 degrees C to 32.6 degrees C?
When two liquids are mixed together in different mole fractions, the mole fractions of their vapors will also be different.
By comparing your answers for partcs b and c, propose a relationships between hydrogen content and fuel value in hydrocarbons.
Carbon dioxide is a greenhouse gas, so over-production can have negative effects on the environment.
Calculate delta Hm, delta Sm and delta Gm. (Look up the standard enthalpy of vaporization at the normal boiling point. Give your source).
You are out camping with your family and you decide that you would heat some water for cooking your food.
How much did the temperature of the hot water change? How much did the temperature of the cold water change?
Calculate the pressure at which diamond and graphite are in equilibrium with each other at 25 degree Celsius.
Calculate the work W in an isothermal reversible process when volume changes from V1 to V2.
If 8675 J of heat flows into 135.0 g of water initially at 20.0°C, find the final temperature of the water. The specific heat of water is 4.18 J g^-1 K^-1.
A 8.375g sample of NaNO3 (F.W. = 85 amu) is added to a calorimeter with 100.0mL of water at 23.0 degrees celcius.
Consider a physical explanation for the difference of vapour pressure of miscible and immiscible solutions.
Given the following thermochemical equations: 2KCl(s) + 3O2(g) .......2KClO3(s) Change in H = 78.0kJ
The standard heat of combustion of liquid ethyl alcohol is -227 kcal/mol and that of acetic acid is -209 kcal/mol.
The compound carbon suboxide, C3O2, is a gas at room temperature. Use the data supplied the calculate the heat of formation of carbon suboxide.
Discuss how to determine the enthalpy of a chemical reaction primarily using Hess's law.
The elementary steps for the catalyzed decomposition for dinitrogen monoxide are shown below. Identify the catalyst.
What is the net ionic equation for the reaction of NaCl with a strong base?
Select the correct balanced net ionic equation for each of the following reactions, occuring in aqueous solution.