A previous Chem 100 student carried out the experiment you did by reacting 0.035 g of magnesium. The following data was collected in their lab notebook. The water temperature was 19.8°C.  The barometer in the lab read 756.9 mm Hg and 31.97 mL of gas was collected The vapor pressure of water at this temperature is 17.32 mm Hg. Calculate the student’s experimental value of R. Report your answer to four places after the decimal.

A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.

Ether was one of the first anesthetics discovered. Assume that several mL of ether is placed in an Erlenmeyer flask with a volume of 293 mL, and the flask is immersed in water at 36.0 °C until the last drop of liquid disappears, leaving the flask filled with ether vapor. The flask is then removed from the water bath, and the weight of ether that condenses in the flask is measured. If 0.801 grams of ether collect in this experiment at a pressure of 104.3 KPa, what is the molecular weight of ether from the experiment? 1 molecule unknown substance = ________ amu

What is the Molecular weight of a certain volatile liquid which is placed in 225 g flask which has total capacity volume of 251.16 ml where after the liquid was heated to 90.2 °C, the gas volatilized and the weight of the flask measured 227.59g.? Round you answer in one decimal place

A hot air balloon is filled with 1.13×106 L of an ideal gas on a cool morning (11°C). The air is heated to 121°C volume of the air in the balloon after it is heated? Assume that none of the gas escapes from the balloon. Do not give handwriting solution.

6. The ideal gas law is a very simple mathematical relationship that relates several physical properties of a gas. This law is only valid when the behavior of a gas is idealized according to three principal assumptions. (i) State the three assumptions made about an ideal gas, and for each assumption (ii) explain which physical property of a gas would be affected if that assumption was not made.

When collecting a gas over water it is necessary to correct for the vapor pressure of water in order to determine the pressure of the gas you are collecting. We will do this by using a graph of ln P in mmHg versus 1/T where T is the temperature in Kelvin. The equation is y = -5206.4 x + 20.621 (With an R^2 = 0.9999). If you collect a gas at 26.8 ℃, what is the value of “x” that you want to use in the equation. (Keep the answer for the next question). (Keep extra digits, you do not want to round in the middle of this calculation). Select one:   a. 0.003660992 b. 0.037313433 c. 0.003378378 d. 299.95 e. 0.0273150 f. 273.15 g. None of these h. 0.003333889 i. 0.0027315

Use the ideal gas law equation to find the gas constant in R.   Here is your data:   Patm = 760 mmHg   PH2O = 20 mmHg   mMg = 0.040 g, must be expressed in moles, so nMg = nH2 = 0.040 g / 24 g/mol Mg   mol Mg = mol H2   Volume of H2 = 41.0 mL   Must calculate the pressure of H2, express the Pressure in atm, Temperature in Kelvin and Volume in Liters.

Study the following phase diagram of Substance X. pressure (atm) 1.6- 0.8- solid 200 liquid temperature (K) 400 - gas Use this diagram to answer the following questions.

Please see question 28, just the top one. I figure in this system the pressure is changing and my answer is the original pressure divided by the final pressure is equal to X.  Do I have this correct?     pv= nRT      N and T and R are constants   thus P1V1 = P2V2.