**Collection of Hydrogen Gas Over Water**In this experiment, hydrogen gas is formed through a chemical reaction and collected over water at a temperature of 30°C. The total pressure measured during this process is 733 mm Hg.**Question:**- **Part A:** Determine the partial pressure of the hydrogen gas collected.To find the partial pressure of hydrogen gas (\( P_{H_2} \)), you would typically subtract the vapor pressure of water at 30°C from the total pressure. This is because the total pressure includes both the hydrogen gas and the water vapor.Use the following formula:\[ P_{H_2} = P_{\text{total}} - P_{\text{water vapor}} \]Where:- \( P_{\text{total}} = 733 \text{ mm Hg} \)In this setup, input the calculated \( P_{H_2} \) in the provided box, measured in mm Hg.

Answered: Image /qna-images/answer/1845b6ae-611f-440e-8d75-24f752139184.jpg

The hydrogen gas formed in a chemical reaction is collected over water at 30 °C at a total pressure of 733 mm Hg. Part A What is the partial pressure of the hydrogen gas collected in this way? νο ΑΣφ PH2 mm Hg %3D

The hydrogen gas formed in a chemical reaction is collected over water at 30 °C at a total pressure of 733 mm Hg. Part A What is the partial pressure of the hydrogen gas collected in this way? νο ΑΣφ PH2 mm Hg %3D

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

Related questions

Q: A tank was filled with 12 g of oxygen (O2), 73 g of nitrogen (N2) and 4 g of carbon dioxide(CO2). At…

Q: A sample contains 10.5 g N2 (MW = 28.02 g/mol), 6.5 g He (MW = 4.00 g/mol), and 34.6 g CO2 (MW =…

A: Given : Mass of N2 = 10.5 g Mass of He = 6.5 g Mass of CO2 = 34.6 g And total pressure of mixture =…

Q: 2.25 grams of zinc metal is reacted with 54.3 mL of a 1.22 M HCl solution. If 1.52 L of hydrogen gas…

Q: 4.00 L flask contains 1.40 atm argon at 25°C. a) Calculate the moles of argon gas initially present…

A: We will calculate all parts

Q: An equimolar (i.e. containing same molar amount) mixture of O2, N2, Kr, and CO2 gases is placed in a…

A: The Scottish physical chemist Thomas Graham gives direct relation between rate of effusion of gas…

Q: A 1.00 L flask is filled with 1.00 g of argon at 25 ∘C. A sample of ethane vapor is added to the…

Q: 又.且 tBuOK, A - H20 A 1. LDA, - 78 °C + H20 2.

Q: 4. A mixture of helium and neon gases is collected over water at 28.0 °C and 745 mm Hg. If the…

A: The total pressure of the mixture is equal to the sum of the individual partial pressures of each…

Q: A steel cylinder contains 5.00 moles graphite (pure carbon) and 5.00 moles O2. The mixture is…

A: Given: Moles of graphite= 5.00 mol Moles of Oxygen =5.00 mol The pressure of the cylinder increases…

Q: Consider the following samples of gas: sample composition pressure temperature composition pressure…

A: The molecular speed of any gas depends on temperature and molar mass of the gas.The molecular speed…

Q: C 2.1 mol He (g) 2.8 atm F 1.9 mol Kr (g) 1.6 atm elect the set of graphs below that show the…

A: The objective of the question is to select the graphs that show the distributions of the speed of…

Q: For many purposes we can treat butane (C4H10) a as an ideal gas at temperatures above its boiling…

A: Gay- Lusaac'a law : This law states that the pressure (P) of a fixed mass of gas held at a constant…

Q: Determine the pressure (in mmHg) for the nitrogen gas sample that is collected when 53.0 g of NaN3…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: A sample of gas held at constant volume is cooled from 228 °C to -75.0 °C. The initial pressure is…

A: According to Gay-Lussac's Law, P ∝ Tor, P1T1 = P2T2 Given, T1 = 228 oC T1(K) = 228 + 273 = 501 K…

Q: . If pressure and temperature are kept constant, the reaction of 18 mL of N2 gas with 54 mL of H2…

A: Given data :

Q: At 1.00 atm pressure and a temperature of 25°C, the volume of 1.0 g water is 1.0 mL. At the same…

A: At constant mass gases have very large volume compared to the liquid state of the same substance.

Q: For many purposes we can treat butane (C,H10) as an ideal gas at temperatures above its boiling…

A: Given: Mass of sample= 36g T1= 45°C= 273+45= 318K T2 = ? P1= P…

Q: If a gas sample is 25% oxygen and 75% carbon dioxide with a total pressure of 255 kPa, what is the…

A: According to the kinetic molecular theory of gas, the pressure of a gas depends on the temperature,…

Q: For many purposes we can treat butane (C₂H₁0) as an ideal gas at temperatures above its boiling…

Q: The stopcock connecting a 1.00 L bulb containing xenon gas at a pressure of 454 mm Hg, and a 1.00 L…

Q: The generic reaction occurs in a closed container: 2A(g) +B(g) → 2Ce) A reaction mixture initially…

Q: 5. A student conducts a laboratory investigation of anaerobic respiration. The student places 10.0 g…

A: We are authorized to answer three subparts at a time since you have not mentioned which part you are…

Q: A tank was filled with 11 g of oxygen (O2), 87 g of nitrogen (N2) and 6 g of carbon dioxide(CO2). At…

A: we know, Molar mass of O2 = 32 g/mol Molar mass of N2 = 28.0134 g/mol Molar mass of CO2 = 44.01…

Q: What is the density of CH4 gas at 134 °C and at 737 mmHg? (1 atm = 760 mmHg) OA 0.0290 g/L OB.3.73…

Q: 37. Mixture of helium gas and oxygen gas are used in the "air" tank of underwater divers for deep…

A: Given: The given mass of O2=0.86 g. The mass of He=2.1 g. The molar mass of O2=32 g/mol. The molar…

Q: Consider the reaction N2(g) + 3H: (g) 2NH3 (g). What is the effect of decreasing the volume on the…

A: A system in its equilibrium state will remain in that state indefinitely as long as it is…

Q: partial pressure of each component of this gas

A: The total gas contains 90.0% of CH4, 8.9 % of C2H6 and 1.1% C3H8 So, Partial pressure of CH4 is –

Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

**Collection of Hydrogen Gas Over Water**

In this experiment, hydrogen gas is formed through a chemical reaction and collected over water at a temperature of 30°C. The total pressure measured during this process is 733 mm Hg.

**Question:**

- **Part A:** Determine the partial pressure of the hydrogen gas collected.

To find the partial pressure of hydrogen gas (\( P_{H_2} \)), you would typically subtract the vapor pressure of water at 30°C from the total pressure. This is because the total pressure includes both the hydrogen gas and the water vapor.

Use the following formula:
\[ P_{H_2} = P_{\text{total}} - P_{\text{water vapor}} \]

Where:
- \( P_{\text{total}} = 733 \text{ mm Hg} \)

In this setup, input the calculated \( P_{H_2} \) in the provided box, measured in mm Hg.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A mixture of He and CO2 is placed in a 7.5L flask at 22C. The partial pressure of the He is 2.2 atm and the partial pressure of the CO2 is 1.9 atm. What is the mole fraction of He?
For many purposes we can treat butane (C,H10) as an ideal gas at temperatures above its boiling point of – 1. °C. 3 Suppose the pressure on a 8.0 m° sample of butane gas at 11.0°C is reduced to one-third its initial value. O yes Is it possible to change the temperature of the butane at the same time such that the volume of the gas doesn't change? olo O no If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C. Explanation Check © 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility
215.0 mol of an unknown gas is stored at a temperature of 1110 K in a large, 395 L container. In atm, what is the approximate pressure of the gas? R=0.0821 Latm/(mol·K) O 180 atm 0.020 atm O 7,700 atm O 50.0 atm O 550 atm O 22.0 atm
5) Consider the reaction below. Co(g) + 2H¿(g) → CH,OH(g) 1.5 L of hydrogen gas and 3.5 L of carbon monoxide gas, both at 45 °C and 1.28 atm are in separate containers separated by a value. When the value is opened the two gases mix and react, according to the above reaction. a) Please determine the limiting reagent and the theoretical yield. b) If the percent yield is 67.3%, what is the concentration of the product in the final reaction mixture? c) What is the partial pressure of the product in the final reaction mixture?
Find the pressure in Torr of 0.0080 mol of an ideal gas contained in 125 L at 15 °C: R = 62.36 L·Torr/(mol·K)
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.
Consider the following samples of gas: sample composition pressure temperature A 2.0mol Xe (g) 1.7atm 228.°C B 2.0mol Xe (g) 1.4atm 258.°C C 2.0mol Xe (g) 1.6atm 280.°C sample composition pressure temperature D 1.5mol He (g) 1.5atm 41.°C E 1.5mol Ar (g) 2.4atm 41.°C F 1.5mol Ne (g) 1.2atm 41.°C Draw the set of graphs below that show the distributions of the speed of the atoms in each sample.
1.What is the temperature of the gas? 2.Determine the volume (in L)
10
Use the ideal gas equation to calculate the number of moles of hydrogen gas produced from a reaction between hydrochloric acid, HCl, and magnesium metal in which 12.0 liters of gas was collected at 22.0 C with a barometric pressure of 761.09 torr. The gas was collected over water with a vapor pressure pf 19.83 torr. R= 82.1 atm mL/mol K or R= 0.0821 atm mL/mol K
A sample of Cl2 with a pressure of 1.84 atm and a volume of 290 mL is allowed to react with excess Br2 at 182 °C. Br2 (g) +Cl2 (g) --> 2BrCl (g) Calculate the pressure of the BrCl produced in the reaction if it is transferred to a 2.16-L flask and cooled to 32 °C