You conducted an experiment in which you measured the molar volume of an ideal gas at STP. In this experiment, you formed hydrogen gas by reacting magnesium metal with hydrochloric acid: Mg (s) + 2 HCl (aq)àMgCl2 (aq) + H2 (g). The hydrogen gas was collected in a tube that contained the metal sample and which was submerged in the solution. a) Explain why hydrogen gas is a good choice of gas to use in an ideal gas experiment such as this.  b) (i) Explain why the pressure of the hydrogen gas collected in the tube is not equal to the surrounding atmospheric pressure and (ii) describe the mathematical correction(s) that must be made to obtain the correct pressure.

How many grams of AL were reacted with excess HCI if 4.78L of hydrogen gas were collected at STP in the following reaction? 2 AL (s) + 6 HCI (aq) = 2 AICI3 (aq) + 3 H2 (g)

what is the correct answer in this question

A mixture of helium and neon gases at 291 K contains 3 times the number of helium atoms as neon atoms. The concentration (n/V) of the mixture is found to be 0.150 mol/L. Assuming ideal behavior, what is the partial pressure of helium? PHe = kPa

#50 Part: (a) and (b)

8-7. Suppose a 185 gram sample of hydrogen reacts with an excess of nitrogen dioxide as follows: 2 NO2 (g) + 7 H2 (g) → 2 NH3 (g) + 4 H2O(g) Both products are collected together (separate from any remaining reactants) in a 325 liter vessel at 512 K. a. How many moles of ammonia gas are produced? b. How many moles of water vapor are produced? c. What is the total pressure in the product collection vessel after the reaction is complete?  8-8. Suppose 93.4 grams of aluminum sulfide are added to 5.00 liters of a 0.844 M hydrochloric acid solution and the following reaction takes place: 6 HCl (aq) + Al2S3 (s) → 3 H2S (g) + 2 AlCl3 (aq) a. Which reactant is the limiting reactant? b. Briefly explain how you know which reactant is limiting. Be specific. Use complete sentences. c. What volume of hydrogen sulfide gas is collected at STP? d. How many grams of aluminum sulfide will be left over at the end? e. What is the final molarity of HCl?

A gaseous mixture consists of 1.26 mol of helium, 0.36 mol of neon, and 1.58 mol of argon. What is the mole fraction of helium in the mixture?

Imagine that a chemist puts 4.33 mol each of C3H8 and O₂ in a 1.00-L container at constant temperature of 505 °C. This reaction occurs: C3H8(g) + 502(g) 3C0₂(g) + 4H₂O(g) When equilibrium is reached, 0.645 mol of CO₂ is in the container. Find the value of Keq for the reaction.

The catalytic decomposition of hydrogen peroxide yields oxygen gas and water, according to the reaction given below. In an experiment, the decomposition of hydrogen peroxide yielded 75.3 mL of gas collected over water at 25°C and 0.976 atm. (Pwater = 0.032 atm at 25°C) 2 H2O2(aq) → 2 H2O(l) + O2(g) If the original H2O2 solution had a volume on 500 mL, what was the molar concentration of hydrogen peroxide prior to decomposition?                          A)    1.8 * 10-4 M                                B)    0.058 M                        C)    0.0062 M                        D)    0.060 M                        E)    0.012 M

Mass→Mass & Mass→Vol : Zinc citrate is used in toothpaste it is synthesized from zinc carbonate and citric acid according to the following reaction. A) What mass of Zn₃(C₆H₅O₇)₂ can be produced from 2240. g of ZnCO₃? B) How many L of CO₂ will be produced at STP by this amount?