After 0.600 L of Ar at 1.49 atm and 221°C is mixed with 0.200 L of O, at 403 torr and 1 400.-mL flask at 25°C, what is the pressure in the flask? atm
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Q: A 250.0 mL flask contains 0.200 g of a gas at 212 mmHg and 23oC, what is the molar mass of the gas?
A: Given:Volume = 250.0 mL = 0.250 L.Temperature = 23oC = 296 KPressure = 212 mmHg = 0.279 atm.Mass =…
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Q: When 1.070 g of an unknown gas is held in an otherwise-empty 265-mL container, the pressure is 877.5…
A: Given: Mass of gas = 1.070 gVolume of container = 265 mLPressure = 877.5 mm HgTemperature = 20 °C
Q: A 1.92 L flask is filled with 2.52 g of some gas (molar mass 42.100g/mol) at 23.1°C. A different…
A: Given: Volume , V = 1.92 L Temperature = 23.1°C = 296.25K No. Of moles gas= 2.52g/42.1gmol-1= 0.0598…
Q: After 0.600 L of Ar at 1.49 atm and 201°C is mixed with 0.200 L of O₂ at 557 torr and 150°C in a…
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A: Dear Subscriber! You have posted multipart questions. As per our policy, we have addressed first…
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Q: When 0.600 liters of Ar at 1.20 atm and 227 degree Celsius it is mixed with 0.200 liters of O2 at…
A: Given Argon Volume = 0.600 L pressure = 1.20 atm Temperature = 227°C Oxygen Volume = 0.200 L…
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Q: After 0.600 L of Ar at 1.27 atm and 225°C is mixed with 0.200 L of O2 at 600 torr and 106°C in a…
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Q: A sample of a gas weighs 4.65 g and has a volume of 1086 mL at 765.0 torr and 21.0 °C. What is its…
A: Given data: Mass of gas = 4.65 g Volume = 1086 mL = 1.086 L Temperature = 21 oC = 294 K Total…
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Q: After 0.600 L of Ar at 1.20 atm and 227°C is mixed with 0.200 L of O₂ at 501 torr and 127°C in a…
A: Total moles of gas = moles of Ar + moles of O2 PVRT = P1V1RT1+P2V2RT2 P x 0.400R x 300 = 1.20 x…
Q: After 0.6 L of Ar at 1.20 atm and is mixed 127°C in a 4O0 mL flask at 27°C, what is the pressure in…
A: Given that - Volume of Argon = 0.6 L Pressure = 1.20 atm Temperature = 227°C = 227+273 = 500 K…
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Q: When 0.582 L of Ar at 1.20 atm and 227°C is mixed with 0.162 L of O2 at 501 torr and 127°C in a 400.…
A: From ideal gas equation, PV = nRT PV = nRT For Ar gas: Where P = pressure of the gas = 1.20…
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- 1)Please express the normal salt (NaCl) concentration in body fluid into molarity (mM).2) Commercial fuming Sulphuric acid (Oleum-H2S2O6) is 99.9%. solution. Please convert it into molarity.3) Find out the Volume (dm3) of product (gas) at RTP when 0.58 M, 150 mL NaOH (aq.) reacts with 350 mL, 0.25 NH4Cl.4) The above reaction has the product Ammonia, which when dissolved in 650 mL ethanol makes an alkaline ethanolic solution. Find its molarity (M) 5) Calculate the adult dose as per the BW of the baby. (Child dose-50 mg and the BW of the baby is 48 lb (British pound) (1lb=0.453 Kg)50.00 cm3 of a 1.5784 mol.dm-3 solution of potassium hydroxide is transferred to an empty 700.00 cm3 volumetric flask. This flask is made up to the mark with distilled water and then shaken well. The concentration of the potassium hydroxide in this second flask is:7. Consider a1Msolution ofNa3AsO4. Write the charge and mass balance equations for this system. (please type answer not write by hend)
- Which of the following is a spontaneous reaction.? a. Rxn with ΔH =- 10Kj/mol ΔS= -5J/mol T= 300K b. NaCl +H20 -> NaOH + HCl 25C c. H20(l) -> H2O(s) Temp: 25C d. Dissolution of 100g of solid sugar in 100 mL ice tea. Consider following reaction: HgO (s) -> Hg(l) + ½ O2 (g) Delta H = +90.7 kj/mol. What quantity of heat in kj/mol is required to produce one mole HgO? Write your answer without units. Given the following data 2ClF(g) + O2(g) --> Cl2O(g) + F2O (g) Delta H= 167.4 kJ I 2ClF3(g) + 2O2(g) --> Cl2O(g) + 3F2 O (g) Delta H= 341.4 kJ II 2 F2(g) + O2(g) ---> 2F2O (g) Delta H= -43.4 kJ III Calculate the delta H in kJ for below reaction: ClF(g) + F2(g) ---> ClF3(g)Why do you multipy the # of H2S mols by 4, when 4 corresponds to the reactory amount of O2?The logic there is somewhat confusing to me.I understand how/why you found out the mols of the equation but dividing the sample's MM by the equation confuses me.An aqueous waste stream that has a maximum concentrationof 0.50 M H₂SO₄ (d=1.030 g/mL at 25C) will be neutralized by controlled addition of 40% caustic soda (NaOH; d=1.430 g/L) before it goes to the process sewer and then to the chemical plant waste treatment facility. However, a safety re-view finds that the waste stream could meet a small stream of animmiscible organic compound, which could form a flammable vapor in air at 40.°C. The maximum temperature of the causticsoda and the waste stream is 31°C. Could the temperature in-crease due to the heat of neutralization cause the vapor to ex-plode? Assume the specific heat capacity of each solution is 4.184 J/gK.
- Initial concentrations For mixture #1 (see p.15 for preparation), show the worked out calculations for the initial concentrations of .... The first questionGood Day, Ive already had the first question answered for me. Can you please help me with 1.2 ? 1.1 It is well-known that te emission of greenhouse gasses such as carbon dioxide presents a very grave threat to the environment. Attempts are ongoing to absorb this gas by several means. One such approach involves the use of vegetation, as plants utilize the gas by means of photosynthesis. One such plant , which has shown great promise, is the "Spekboom" It has been estimated that fully-grown Spekboom can absorb 3.8 tonnes of carbon per hectare of plants per year. If the system is fully functional, South Africa can generate 234.5 x 109 kWh of electricity per year. Assume that 1559 pounds of CO2 is emmited per year per Megawatt-hour of electricity generated in the country. Determine, by means of the use of conversion factors, how many square kilometres of Spekboom could theoretically absorb all of this carbon dioxide ? 1.2 Consider the molecule, ClPO2 (The Phosphorus atom is the central…Potassium dichromate has several industrial applications. To determine the purity of the salt that will be used in different industrial processes, a sample mass equal to 2.660 g was dissolved and quantitatively transferred to a 500.00 mL flask. An aliquot of 25.00 mL of this solution was treated with excess KI and the released iodine was titrated with 0.1000 mol L-1 sodium thiosulfate, spending 27.00 mL. Calculate the purity of the analyzed salt. Data:K = 39.10 O = 16.00 Cr = 52.00 I = 126.9 S = 32.07
- One way to determine the hardness of a water sample is to precipitate the calcium out of solution as a carbonate. The net ionic reaction for this precipitation is: Ca2+(aq) + CO32-(aq) → CaCO3 (s) A 1.00 L sample of water is drawn from a Phoenix, AZ well and 0.534 g of calcium carbonate is recovered using the above reaction. What was the Ca2+ concentration of the original water sample in ppm? Show your work and include units. Hint: ppm stands for parts per million, and in the case of an aqueous solution, this is equivalent to mg/L.STRICTLY HANDWRITTEN ONLY... do ques 5... needed urgently...Beaker 0.00200 M Fe(NO3)3, mL 0.00200 M NaSCN, mL total volume, mL 1 3.000 2.000 10.00 2 3.000 3.000 10.00 3 3.000 4.000 10.00 4 3.000 5.000 10.00 5 (blank) 3.000 0.000 10.00 In Solutions 1-4 you are adding successively larger volumes of 0.00200M SCN- to the Fe3+ solution and diluting to 10.00 ml. Calculate the final diluted molarity of SCN- in solution #1 Your answer should have 3 sig figs =