In an industrial process, nitrogen has to be heated to 500 K in a vessel of constant volume. If it enters the vessel at a pressure of 100 atm and a temperature of 300 K, what pressure does it exert at the working temperature?
Glucose reacts with oxygen to form carbon dioxide and water: If the heat of formation of glucose, carbon dioxide, and water are -1273.3 kJ mol-1, -393.5 kJ mol-1 and -285.8kJ mol-1. How many grams of glucose must react in order to release (1.00)(10^3)kJ of heat?
Calculate the bond energy of the reaction: 2 H2 + O2 ---> 2 H2O
Glucose reacts with oxygen to form carbon dioxide and water: If the heats of formation of glucose, carbon dioxide, and water are -1273.3 kJ mol-1, -393.5 kJ mol-1, and -285.8 kJ mol-1, how many grams of glucose must react in order to release (1.00)(10^3) kJ of heat? What is the difference between bond energy, H minus the to
The reaction of 4.49 g of carbon and 9.21 g of oxygen, produced carbon dioxide, and 113.2 kJ of heat. What is the enthalpy of formation of carbon dioxide?
Find the work done, w, when a system absorbs 104 J of heat and its internal energy decreases by 55 J.
Copper has a specific heat of 0.382 J g-1 degrees Celsius -1. The temperature of an unknown mass of copper increases by 4.50 degrees Celsius when it absorbs 3.97 J of heat. What is the mass of copper?
What mass of water rises by 15 degrees Celsius when it absorbs 2646 Joules?
Delta G sub f for Al203 = -1582 kJ/mol delta H sub f for Al203 = -1676 kJ/mol 1. Calculate absolue entropy for S for oxygen (g) if: S for Al(s) = 164 J/mol K S for Al2O3 (s) = 51.0 J/mol K 2. Calculate the heat required to raise the temperature of 35.0 g of aluminum from 800 degrees C to 2600 degrees C 3. To c
Chemistry review problems, please see the attachment. PART QUESTION 1: A) i) Sketch the galvanic cell based on the following two half-reactions. Indicate (i) the balanced cell reaction, (ii) Eo for the cell, (iii) which electrode is the anode and which the cathode, (iv) the direction of electron flow. Au3+ (aq) + 3e- ïƒ
When calculating the amount of heat emitted (q): In which of these situations should you add the weight of what is added to the water, to the weight of the water itself? - 17g stick of boiled metal added to water in a calorimeter. or - 2g of NaOH added to water to measure the heat of dissolving.
I'm having problems understanding the ideas in the topic of thermal chemistry and would appreciate any sort of overview of the main concepts you could provide.
If you boil water are you increasing delta H (heat), delta E (energy), or delta S (entropy)?
Liquid methanol has a heat capacity of 81.6 J/(K mol). How much heat is required to raise the temperature of 20.0 g of liquid methanol from 25 C to 40.0 C?
Considering the Reaction: 2H2O(l) => 2H2(g) + O2 (g) This reaction has dispersal of matter since a liquid produces two gases, yet the reaction is not spontaneous. Why is this so?
Which reaction is more exothermic? A reaction with Keq=500 or a reaction with Keq=0.002?
The attached problem file shows the standard Gibbs Free Energy Change for two reactions. Considering these values, which reaction is more favoured or spontaneous? A reaction with a delta Go = 16 kcal mole-1? Or a reaction with a delta Go = -16 kcal mole-1?
A reaction vessel contained 5 liters of a mixture of N2 and O2 gases at 25oC and 2 atm pressure. The oxygen in the mixture was completely removed by causing it to oxidize with an excess of electrically heated zinc wire contained in the vessel to non-volatile solid ZnO. The pressure of N2 that remained (measured again at 25oC) wa