In: Chemistry
The picture below shows two bulbs connected by a stopcock. The 6.00-L bulb contains nitric oxide at a pressure of 0.400 atm, and the 1.50-L bulb contains oxygen at a pressure of 2.50 atm. After the stopcock is opened, the gases mix and react: Determine which gases remain after the reaction goes to completion and calculate their partial pressures. The temperature at the beginnning and the end of the experiment is 22 °C. Which gases are present at the end of the experiment? What are the partial pressures of the gases? If the gas was consumed completely, put 0 for the answer.
In: Chemistry
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alculate the pH of the following solutions. |
Part A Solution prepared by dissolving 5.5g of lithium hydroxide in water to give 230mL of solution. Express your answer using two decimal places.
SubmitMy AnswersGive Up Part B Solution prepared by dissolving 0.96g of hydrogen chloride in water to give 0.48L of solution. Express your answer using two decimal places.
SubmitMy AnswersGive Up Part C Solution prepared by diluting 57.0mL of 0.120M HCl to a volume of 1.00L . Express your answer using two decimal places.
SubmitMy AnswersGive Up Part D Solution prepared by mixing 119.5mL of 1.3 |
In: Chemistry
Explain the IMFs for the Following and wether they are soluble, insoluble or partially insoluble:
-Acetone and Butanol, acetone and ethanol, acetone and CCl4, acetone and hexane, acetone and H2O
-Butanol and ethanol, butanol and CCl4, butanol and hexane, butanol and H2O
-CCl4 and ethanol, CCl4 and hexane, CCl4 and water
-Ethanol and hexane, and ethanol and H2O
-Hexane and water
In: Chemistry
calculate the ph of a solution when 15ml of 0.5M naoh is added to 30ml of a 0.8 M benzoic acid (Benzoic acid is a monoprotic acid and has a ka of 6.5 x 10^-5
In: Chemistry
A student conducted an experiment to determine what factors are important in the rate of a reaction between potassium carbonate and hydrochloric acid. The student diluted 2.000 mL of 4.000 M K2CO3 to 75.00 mL, then combined that solution with 75.00 mL of 2.000 M HCl.
The student tabulated the amount of CO2 gas collected over time and recorded the results in the columns to the left.
| Time (min) | Volume (mL) |
| 1 | 0.2 |
| 2 | 0.3 |
| 3 | 0.5 |
| 4 | 0.7 |
| 5 | 0.9 |
| 6 | 1 |
| 7 | 1.2 |
| 8 | 1.3 |
| 9 | 1.5 |
| 10 | 1.7 |
| 11 | 1.9 |
| 12 | 2 |
| 13 | 2.2 |
| 14 | 2.4 |
| 15 | 2.5 |
| 16 | 2.7 |
| 17 | 2.9 |
| 18 | 3 |
| 19 | 3.2 |
| 20 | 3.4 |
| 21 | 3.5 |
| 22 | 3.7 |
| 23 | 3.9 |
| 24 | 4.1 |
| 25 | 4.2 |
| 26 | 4.4 |
| 27 | 4.6 |
| 28 | 4.7 |
| 29 | 4.9 |
| 30 | 5.1 |
| 31 | 5.2 |
| 32 | 5.4 |
| 33 | 5.6 |
| 34 | 5.7 |
| 35 | 5.9 |
| 36 | 6.1 |
| 37 | 6.2 |
| 38 | 6.4 |
| 39 | 6.6 |
| 40 | 6.8 |
| 41 | 6.9 |
| 42 | 7.1 |
| 43 | 7.3 |
| 44 | 7.4 |
| 45 | 7.6 |
| 46 | 7.8 |
| 47 | 7.9 |
| 48 | 8.1 |
| 49 | 8.3 |
| 50 | 8.4 |
| 51 | 8.6 |
| 52 | 8.8 |
| 53 | 9 |
| 54 | 9.1 |
| 55 | 9.3 |
| 56 | 9.5 |
| 57 | 9.6 |
| 58 | 9.8 |
| 59 | 10 |
| 60 | 10.1 |
| 61 | 10.3 |
| 62 | 10.5 |
| 63 | 10.6 |
| 64 | 10.8 |
| 65 | 11 |
| 66 | 11.1 |
| 67 | 11.3 |
| 68 | 11.5 |
| 69 | 11.7 |
| 70 | 11.8 |
| 71 | 12 |
| 72 | 12.2 |
| 73 | 12.3 |
| 74 | 12.5 |
| 75 | 12.7 |
| 76 | 12.8 |
| 77 | 13 |
| 78 | 13.2 |
| 79 | 13.3 |
| 80 | 13.5 |
| 81 | 13.7 |
| 82 | 13.8 |
| 83 | 14 |
| 84 | 14.2 |
| 85 | 14.4 |
| 86 | 14.5 |
| 87 | 14.7 |
| 88 | 14.9 |
| 89 | 15 |
| 90 | 15.2 |
| 91 | 15.4 |
| 92 | 15.5 |
| 93 | 15.7 |
| 94 | 15.9 |
| 95 | 16 |
| 96 | 16.2 |
| 97 | 16.4 |
| 98 | 16.6 |
| 99 | 16.7 |
| 100 | 16.9 |
1. Use a rearrangement of PV = nRT to solve for the number of moles of CO2 produced. You may assume atmospheric pressure and room temperature. Enter (and fill down) your formula in column C.
This is suppose to be an excel file bt i do not know how to manipulate the formula where I can put it into excel and what information to extract from the problem to use in order to help solve the problem.
HELP PLEASE !!
In: Chemistry
Which of the following aqueous solutions are good buffer
systems? and Why?
.
0.19 M potassium hydroxide + 0.27 M potassium bromide.
0.28 M hydroiodic acid + 0.18 M sodium iodide.
0.30 M ammonia + 0.37 M ammonium nitrate.
0.17 M hypochlorous acid + 0.12 M hydrobromic acid.
0.38 M calcium bromide + 0.30 M barium bromide.
In: Chemistry
Part A
A solution of water (Kf =1.86 ∘C/m) and glucose freezes at − 4.75 ∘C. What is the molal concentration of glucose in this solution? Assume that the freezing point of pure water is 0.00 ∘C. Express your answer to three significant figures and include the appropriate units.
Part B
A solution of water (Kb =0.512 ∘C/m) and glucose boils at 101.56 ∘C. What is the molal concentration of glucose in this solution? Assume that the boiling point of pure water is 100.00 ∘C.
Express your answer to three significant figures and include the appropriate units.
In: Chemistry
What is the first f element in the 6th period to which Hund's rule must be applied when writing the orbital diagram?
In: Chemistry
Can someone please give me the chemical equation and directions on how to test for each individual solution below and how to tell if my solution has one of each category? So a test for HCl and HNO3 excetera.?
Acid-HCl,HNO3,H2SO4
Base-NaOH, NH3, Na2S
Chloride Salt-NaCl,BaCl2,CuCl2
Nitrate salt-AgNO3,Cu(NO3)2, Fe(NO3)3
Sodium Salt-NaI,Na2SO4,Na2CO3
In: Chemistry
Cu(II) sulfate exists as a hydrate. It has many practical uses including use as a fungicide and pesticide. When mixed with chromium and arsenic it forms the wood preservative called CCA. CCA was used in pressure treated wood to protect wood from rotting due to insects and microbial agents. Because CCA-treated wood contains toxic heavy metals, its use has been discontinued for home use and children’s play sets.
A chemist is given a sample of the CuSO4 hydrate and asked to determine the empirical formula of it. The original sample weighed 42.75 g. After heating to remove the waters of hydration, the sample weighed 27.38 g. Determine the formula for this hydrate.
Please show all work!
In: Chemistry
Q1)A compound of molar mass 213 contains only carbon, hydrogen, iodine, and oxygen. Analysis shows that a sample of the compound contains 6 times as much carbon as hydrogen, by mass.
Part A
Calculate the molecular formula of the compound.
Express your answer as a chemical formula. Enter the elements in the order: C, H, O, I.
Q2) A particular brand of beef jerky contains 6.01×10−2% sodium nitrite by mass and is sold in an 8.00-oz bag.
What mass of sodium does the sodium nitrite contribute to sodium content of the bag of beef jerky?
Express your answer to three significant figures and include the appropriate units.
In: Chemistry
calculate the partial pressure of CO2 over calcium carbonate at 1000K
In: Chemistry
Derive planar density expressions for BCC (110) planes in terms of the atomic radius R.
In: Chemistry
2. Which gas has the lowest density at 25 °C and 1 atm?
Select one:
a. O2
b. Ar
c. N2
d. F2
e. C3H8
4. If the volume of a confined gas is expanded to four times the original volume while its temperature remains constant, what change will be observed?
Select one:
a. The pressure of the gas will decrease to 1/4 its original value.
b. The pressure of the gas will decrease to 1/2 its original value.
c. The pressure of the gas will remain unchanged.
d. The pressure of the gas will increase to twice its original value.
e. The pressure of the gas will increase to four times its original value.
5. 36.6 L of He gas at STP is pumped into a 10.0-L tank containing 1.0 atm of O2 at 25 °C. What is the total pressure in a tank at 25 °C?
Select one:
a. 2.0 atm
b. 5.0 atm
c. 5.4 atm
d. 8.0 atm
e. 8.8 atm
In: Chemistry