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Calculate the pressure of a gas at 237 K if the concentration is 0.150 mol/L
awnser in kPa
P=____kPa
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- 1. A 0.68 gram sample of a volatile liquid was heated to 358 K. The gas occupied 265 mL of space at a pressure of 0.95 atm. What is the molecular weight of this gas? PV = nRT and R = 0.082 atmL/moleK. (Make sure that all your units agree/match R)2. An aspirin sample, 0.62 grams, was titrated with 28 mL of 0.105 M NaOH solution. What is the percent purity of this aspirin sample? (MM of Aspirin = 180. g/mol)3. A sample of hydrate was heated thoroughly. How many waters of hydration are there if the anhydrous salt had a dry mass of 12 grams and a molar mass of 185 g/mol? The mass of water evaporated from the hydrate was 5.0 g.4.A sample of water (80 grams) had a temperature change of 6. ℃. What was the heat change of this sample? (q = m c ΔT, c = 4.18 J/ g ℃)5. A 6.0 gram sample of epsom salt, MgSO4 ·nH2O, was heated. After heating, 2.9 grams of anhydrous salt remained. How many waters of hydration does epsom salt contain?6. What is the theoretical yield of aspirin if you started your…Calculate what volume of concentrated hydrochloric acid, 37.2 % (w/w), that you would need to produce a 3.00 L stock of 2.00 mol dm–3 HCl. [Mr (HCl) = 36.5 g mol–1; density of 37.2% HCl = 1.19 g mL–1]In one experiment, 0.0995M HCl was used to analyze soda ash and the following data were obtained: 0.2980 g Mass of Na2CO3 Initial reading of HCI Final reading of HCI 0.20mL 20.00mL What is the net volume in liters of HCl used? How many moles of Na2CO3 was used in the analysis? What is the corresponding Normality of the HCl used? What is the percent Na2CO3 in the soda ash sample?
- 1. 500.0 mL 0.2 M KI2. 500.0 mL 0.2 M KCl3. 500.0 mL 0.1 M K2S2O84. 500.0 mL 0.1 M K2SO45. 500.0 mL 4.0 mM Na2S2O3 (from Na2S2O3∙5H2O)pls compelete the 2nd table given the datavolume HCl (mL) mass unknown sample (g) 0.5007 molarity HCl (mol/L) 25.00 12.1 . Write a balanced chemical equation for the reaction between NaHCO; and HCl. Calculate the moles of HCl by multiplying the volume of HCl in liters and the molarity of HCl in mol/L. (Keep four significant digits in all of the calculations.)What is the maximum solubility of silver carbonate, Ag2CO3, in g/L, if the solubility product for Ag2CO3 is 8.4x10-12 and the molar mass is 275.75 g/mol. Express your answer to the correct number of significant figures, in scientific notation and include the unit with your answer.
- Materials Needed solid I2 solid CUSO4-5H20 food dye solid (NH4)2SO4 heavy metals waste container halogenated waste container non-halogenated waste container semi-micro test tubes and rack regular test tubes and rack squash pipettes acetone cyclohexane propan-2-ol Method Part A: Solubility of ionic and molecular solids 1. Place a small amount (about the size of 1 grain of rice, see picture) of copper sulfate into each of three DRY semi-micro test tubes. Add 20 drops of water to the first test tube and gently flick the test tube with your finger to ensure mixing. 2. Repeat step 1 using acetone in place of water as the solvent in the second test tube. 3. Repeat step 2 replacing acetone with cyclohexane in the third test tube. Hold the test tubes against a white background to compare the solubility of copper sulfate in the three solvents and record your results. Discard these mixtures into the heavy metals waste container in the fume cupboard. Once these test tubes have been emptied you…if 0.200 L of 0.335 M Ca(NO3)2 and 0.300 L of 0.077 M Na2CrO4 are mixed, what is the Qip? Ksp for CaCrO4(s)= 7.1 x10^-4(a) One particular pungent gas is the toxic hydrogen sulphide (H2S). Hydrogen sulphide develops an odour of rotten eggs at a partial pressure of 0.13 ppm or 0.0132 Pa. If the aqueous concentration of hydrogen sulphide in the stream is 2.5 x 10–6 M, determine through calculations if the hydrogen sulphide in the water may be responsible for the odour detected near the vicinity of the stream. KH (H2S) = 0.087 M/atm) (b) In the leachate pond the conditions are more acidic causing NH3 to exist as NH4+. NH4+ can react with nitrites in the pond to form the less hazardous N2 and H2O as seen below: NH4+ + NO2– → N2 + 2H2O You want to investigate methods of speeding up this reaction but you first conducted an initial rates test to determine the rate law equation for the reaction. Using the data in the table below determine the rate law equation for the reaction above. Experiment Number Initial NH4+ M Initial NO2– Initial Rate (M/s) 1 0.0100 0.200 5.4 x 10 –7…
- 14. Consider the following chemical reaction: N2O3 (g) + H2O (l) ------------------> HNO3 (aq) 220 mL. of N2O3 (g) at the pressure of 1.22 atm. and temperature of 25 oC is bubbled into 155 mL. of water. Calculate the molarity of nitic acid. H = 1.008 g/mole, N = 14.00 g/mole, O = 16.00 g/mole Hint: the volume of solution = volume of water a. 4.50 M b. 0.0223 M c. 2.30 M d. 0.142 M14. Consider the following chemical reaction: N2O3 (g) + H2O (l) ------------------> HNO3 (aq) 220 mL. of N2O3 (g) at the pressure of 1.22 atm. and temperature of 25 oC is bubbled into 155 mL. of water. Calculate the molarity of nitic acid. H = 1.008 g/mole, N = 14.00 g/mole, O = 16.00 g/mole Hint: the volume of solution = volume of water a.2.30 Mb.0.0223 Mc.4.50 Md.0.142 MFe (55.85 g/mol) is precipitated as Fe(OH)3 (106.87 g/mol) which is typically ignited to form Fe2O3 (159.69 g/mol) prior to weighing. The Fe in a 2.00 L solution was precipitated and ignited, yielding 0.57 g of Fe2O3. Calculate the original ppm.
