Answer:
Since Q > Ksp, a precipitate of AgCl will form.
Explanation:
Step 1: Data given
Molarity AgNO3 = 0.10 M
Molarity of NaCl = 0.075 M
Ksp AgCl = 1.77 * 10^-10
Step 2: The balanced equation
AgNO3 + NaCl → AgCl(s) + NaNO3(aq)
For 0.10 moles AgNO3 we have 0.10 moles Ag+ ( molarity = 0.10 M)
For 0.075 moles NaCl we have 0.075 moles Cl- (molarity = 0.075 M)
Step 3: Calculate Q
Q = [Ag+][Cl-]
Q = (0.10 M )(0.075 M ) = 0.0075
Ksp = 1.77 * 10^-10
Q >>> Ksp
Since Q > Ksp, a precipitate of AgCl will form.
The volume of the oxygen gas at standard temperature is 41.36 liters.
The given parameters;
- <em>initial volume of oxygen, V₁ = 45 L</em>
- <em>temperature of oxygen, T₁ = 24 ⁰C = 297 K</em>
- <em>standard temperature, T₂ = 0 ⁰C = 273 K</em>
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The volume of the oxygen gas at standard temperature is determined by applying Charles law as shown below;
![\frac{V_1}{T_1} = \frac{V_2}{T_2} \\\\V_2 = \frac{V_1 T_2}{T_1} \\\\V_2 = \frac{45 \times 273}{297} \\\\V_2 = 41.36 \ L](https://tex.z-dn.net/?f=%5Cfrac%7BV_1%7D%7BT_1%7D%20%3D%20%5Cfrac%7BV_2%7D%7BT_2%7D%20%5C%5C%5C%5CV_2%20%3D%20%5Cfrac%7BV_1%20T_2%7D%7BT_1%7D%20%5C%5C%5C%5CV_2%20%3D%20%5Cfrac%7B45%20%5Ctimes%20273%7D%7B297%7D%20%5C%5C%5C%5CV_2%20%3D%2041.36%20%5C%20L)
Thus, the volume of the oxygen gas at standard temperature is 41.36 L.
Learn more here:brainly.com/question/16927784
Answer is: C. a long chain of carbon atoms with hydrogen atoms attached to them.
Starch is example of polymer.
Main component of bread is flour and main component of flour is starch.
Starch is a polymeric carbohydrate consisting of a large number of glucose units bonded by glycosidic bond. Starch is a white, tasteless and odorless powder that is insoluble in cold water or alcohol.
Another example, polystyrene is a synthetic aromatic hydrocarbon polymer made from the monomer styrene.
Answer:
1. Why was the line of best fit method used to determine the experimental value of absolute zero?
The line of best fit method is used to determine the experimental value, because it most accurately shows where the line crosses the x-axis.
2. Which gas law is this experiment investigating? How does your graph represent the gas law under investigation?
This investigation is experimenting the “Ideal Gas Law”. This law by Gay-Lussac shows that when the volume in a container of a gas is held constant, while the temperature is increased, the pressure will also increase.
3. Using your knowledge of the kinetic molecular theory of gases, describe the relationship between volume and temperature of an ideal gas. Explain how this is reflected in your lab data.
As temperature increases, volume increases when pressure is held constant. As seen in the chart, as the temperature increases the volume in each gas also increases slightly.
4. Pressure and number of moles remained constant during this experiment. If you wanted to test one of these variables in a future experiment, how would you use your knowledge of gas laws to set up the investigation?
Supposedly at a constant temperature, the gas volume and pressure stay constant. Therefore, the amount of moles also remains constant. So perhaps, the temperature could fluctuate, meaning it will not only increase or decrease, but do both. This will avoid consistency and prove the Ideal Gas Law to be true.
Explanation:
Carbon dioxide nitrous oxide methane and ozone