Please! Answer for ALLL for 5 stars and point! Experiment 4 Experiment 4? Chemic
ID: 805419 • Letter: P
Question
Please! Answer for ALLL for 5 stars and point!
Experiment 4
Experiment 4? Chemical Equilibrium 1. What is LeChatelier's Principle? 2. What is equilibrium? When does it happen? 3. What factors affect a system at equilibrium? 4. Predict what will happen to the concentration of oxygen gas when each of the following changes is applied: 2H2O2(g) arrow 2H2O(g)+ O2(g); deltaHm=-210kJ/mol a. Temperature is increased b. Pressure of the system doubles c. Concentration of H2O2 is doubled d. Liquid water is added to the above equilibrium 5. Be ready to write the equilibrium expression in terms of concentration for any of the reactions you will be working with during the experiment. 6. Identify for each of the following as strong or weak adds: a. H2SO4 b HNO3 c. CH3COOH d. HCl e. H2CO3 f. H3PO4 7. What is a buffer? How does it form? 8. Identify the buffer responsible for controlling pH in the blood? 9. For each of the following salts identify the acid and base that they came from: a. NaCl b. Na3PO4 c. NH4Cl d. CH3COONa e. NH4CH3COO 10. List two safety precautionsExplanation / Answer
1.In chemistry, Le Chatelier's principle, also called Chatelier's principle or "The Equilibrium Law", can be used to predict the effect of a change in conditions on a chemical equilibrium.
2.EQUILIBRIUM-State of stable conditions in which all significant factors remain more or less constant over a period, and there is little or no inherent tendency for change. For example, a market is said to be in equilibrium if the amount of goods that buyers wish to buy at the current price is matched by the amount the sellers want to sell at that price. Also called steady state.
In chemistry, Equilibrium Occurs when the rate of the forward reaction is Equal to the rate of the reverse reaction, so applying this to physics i would say it is all of the above.
3. 1) Effect of change of concentration
2) Effect of change of pressure
3) Effect of change in temperature
4) Effect of catalyst
4. a. Temperature is increased
5.CO(g)+2H2(g)?CH3OH(g)
6. a.strong acid
b.weak acid
c.weak acid
d.strong acid
e.weak acid
f.weak acid
7.A buffer is an aqueous solution that has a highly stable pH . If you add acid orbase to a buffered solution, its pH will not change significantly. Similarly, adding water to a buffer or allowing water to evaporate will not change the pH of a buffer.
A buffer is made by mixing a large volume of a weak acid or weak base together with its conjugate. A weak acid and its conjugate base can remain in solution without neutralizing each other. The same is true for a weak base and its conjugate acid .
8.The bicarbonate buffering system
9. a.Nacl- HCL and NaOH
b.HCL and H3PO4
c.NH3 and HCL
d.Nacl and CH3COOH
e.NH3 and CH3COOH
10. 1)Safety goggles must be worn at all times while in the laboratory. This rule must be followed whether you are actually working on an experiment or simply writing in your lab notebook. You must wear safety goggles provided by the chemistry department
2)Contact lenses are not allowed. Even when worn under safety goggles, various fumes may accumulate under the lens and cause serious injuries or blindness.