Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s) + 2HCI(aq) ZnCl2(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 754 mm Hg. If the vet H2 gas formed occupies a volume of 6.46 L, the number of moles of Zn reacted was The mol. vapor pressure of water is 23.8 mm Hg at 25 °C.

Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s) + 2HCI(aq) ZnCl2(aq) + H2(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 754 mm Hg. If the vet H2 gas formed occupies a volume of 6.46 L, the number of moles of Zn reacted was The mol. vapor pressure of water is 23.8 mm Hg at 25 °C.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

In a space shuttle, the CO2 that the crew exhales is removed from the air by a reaction within canisters of lithium hydroxide. On average, each astronaut exhales about 20.0 mol of CO2. The reaction between carbon dioxide and lithium hydroxide is shown below: CO2(g) + 2LiOH(s) ⟶⟶ Li2CO3(aq) + H2O(l) What volume of water will be produced when this amount (20.0 mol) of CO2 reacts with an excess of LiOH? (Hint: Use the density of water 1.00 g/mL in your solution)
Q/ Gaseous hydrogen sulfide and gaseous sulfur dioxide are combined in a 250. mL flask. The gas mixture is heated to 100. °C where they react according to the following equation. 2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(l) a) If H2S has a partial pressure of 2.00 atm, and that of SO2 is 1.50 atm, determine the maximum yield possible of sulfur, in grams. Show all work. b) If you collected 0.55 grams of sulfur, what was your percent yield for the reaction? Show all work.
Consider the reaction: Li2O(aq) + CO2(g) Lİ2CO3(s) ----> What volume of cabon dioxide will react completely with 1.00 g of lithium oxide (Li20; 29.88 g/mol) at 25 °C and 1.00 atm?
If boron hydride, B4H10, is treated with pure oxygen, it burns to give B2O3 and H2O: 2 B4H10(s) + 11 O2(g) ®4 B2O3(s) + 10 H2O(g) If a 0.050-g sample of the boron hydride burns completely in O2, what will be the pressure of the gaseous water in a 4.25-L flask at 30.0°C?
Chemistry iIi) What will be the pressure of SO4 gas when 189 gram of Aluminium potassium sulfate AlK(SO4)2) is heated ?
What volume of H2 gas, measured at 9 °C and 722 torr, can be obtained by reacting 8.40 g of zinc metal with 185 mL of 0.425 M HCl? (6 marks) Zn(s) + 2 HCl (aq) → ZnCl2(aq) + H2(g) (1 atm = 760 torr)
37. What volume of H, gas, measured at 27°C and 700. torr, can be obtained by reacting 5.00 g of zinc metal with 100. mL of 0.350 M HCI? The equation is Zn(s) + 2 HCl(aq) – → ZnCl(ag) + H2(g)
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)
How many liters of CO2 are produced when 3.46 Fe2O3 is converted to cast Fe at STP? Fe2 O3 (s) + 3CO(g) -> 2Fe(s) + 3CO2 (g)
1. A student following the procedure described in this module collected the following data: mass Mg, g 0.0243 initial syringe volume, mL 1.0 final syringe volume, mL 26.5 barometric pressure, torr 754 temperature, K 298 Determination#1 The value of the gas law constant (R) is 0.0822 L.atm/mol.K Determination #2 he volume of hydrogen gas produced by the reaction of 0.243 g of magnesium metal and collected at 750 torr and 298 K = 248 mL The results of this experiment are greatly affected by the care with which each of the steps is completed (a) Describe the error that would occur if the magnesium were to slide into the HCl in the test tub before the system is sealed off (b) What would be the effect on the results of a rise in the room temperature from 22.0 celcius, when determination #1 was done, to 25.3 celcius, when determination #2 was made? (c) Why must the surface coating of MgO be removed prior to determining the mass of magnesium used in the experiment? (d) What would be the…
Zinc metal reacts with excess hydrochloric acid to produce hydrogen gas according to the following equation: Zn(s) + 2HCl(aq) → ZnCl₂ (aq) + H₂(g) The product gas, H2, is collected over water at a temperature of 25 °C and a pressure of 752.0 mm Hg. If the wet H₂ gas formed occupies a volume of 7.62 L, the number of grams of H₂ formed is g. The vapor pressure of water is 23.8 mm Hg at 25 °C.
Calculate the amount of Cl2 (g) produced in L at STP and calculate the percent yield of Cl2(g) in the electrolytic decomposition of hydrogen chloride if 25.8 g of HCl produces 4.29 L of chlorine gas in a laboratory environment. 2HCl (g) →H2 (g)+ Cl2 (g)