A reaction of 0.028 g of magnesium with excess hydrochloric acid generated 31.0 mL of gas. The gas was collected by water displacement in a 22°C water bath. The barometric pressure in the lab that day was 746 mmHg. A. Using Dalton's Law and the vapor pressure of water at the given temperature to calculate the partial pressure of hydrogen gas in the collection tube. 7 B. Use the combined gas law to calculate the corrected volume of hydrogen at STP. C. What is the theoretical number of moles of hydrogen that cạn be produced from 0.028 g of magnesium reacting with excess hydrochloric acid?

Lab 7: Gas Law Pre-Lab Questions 3. Your cousin made a bad life choice and went to Dominican College instead of STAC. He is also taking General Chemistry Lab this semester. Instead of reacting Mg with HCl, he is supposed to react zinc, Zn with HCl and performed a similar experiment. He reacted a 0.063 g sample of zinc with excess 1 M HCl at 24 °C (both lab and water temperature). The reaction produced a gas that expanded to a volume of 25.0 mL. The atmospheric pressure was 760 mmHg on the day he performed the experiment. a. Write the balanced equation for this reaction. HCI b. What is the pressure (in atm) of the H₂ gas that was produced? Remember to take into account the vapor pressure of water. c. What is the temperature in Kelvin? Name: d. How many moles of H₂ moles of H₂ should you produce with this amount of starting material? 116 e. Using the P, V, T, and n listed above, solve for your experimentally determined value of the Ideal Gas Constant, R. ***

A quantity of helium gas is originally held under a pressure of 145 kPa at 18°C. If the volume of the container is tripled, and the temperature is increased to 30°C, what is the resulting pressure in kPa? (Hint, can you make up a volume?) H 322181 Li Na Mg Rb Be Sr Cs Ba Fr 22 Ca Sc Ti Ra Raden Lat 94.5 kPa 46.4 kPa 378.3 kPa 453.9 kPa 50.3 kPa MD 45 83-103 482.2 kPa Zr Hf Atvice Ac Th Series 23 VO Vieta VID 24 2 Ta W Tete 104 105 Rf Db Sg Cr Mn Periodic Table of the Elements VID 75 41. 34445 Nb Mo Tc Ru Rh Pd Ag Cd Abaline Tra Saber 26 27 28 29 30 Fe Co Ni Cu Zn Re Os Symbol S 13 13 FIA B Nawww Al Ga Halagan In La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho D IVA 70 Pt Au Hg Tl Pb B Mar 102108, 109 114 Bh Hs Mt Ds Rg Cn Uut "FI 590 U Np Pu Am Cm Bk Cf Es Sn Sb 14 15 16 17 18 Si CI Ar La 16 3514. Ge As Se Br Kr By 17 VIA 18 VELA He Hek 4000 Ne 62 63 64 SA Te I Xe 16 At Rn Fate Bi Po Uup "Lv Uus Uuo Er Tm Yb Lu C Henan 100 100 Fm Md No L

What volume of hydrogen gas will be produced when 5.00 g of calcium reacts with excess hydrochloric acid at STP? (STP is standard temperature and pressure. Standard temperature is 0oC and standard pressure is 1.00 atmospheres.) What is the name of this law?

Potassium reacts with water to release hydrogen gas according to the following equation 2K(s) + 2H2O(L) > 2KOH(aq) + H2(g) What mass of potassium is needed to produce 50 L of H2 at SATP a. 158 g b. 79 g c. 316 g d. 950 g

A flask at room temperature contains exactly the same amounts in terms of O2 and Neon. If a small hole were opened in the flask, which gas would effuse more quickly? A. It is the same. B. Neon C. O2