A sample of 263.0 mL of wet nitrogen gas was collected over water at a total pressure of 756 torr and a temperature of 21.0 °C. (The vapor pressure of water at 21.0 °C is 18.7 torr.) The nitrogen was produced by the reaction of sulfamic acid, HNH,SO3, with 368.5 mL of a solution of sodium nitrite according to the following equation. NaNO2 + HNH2SO3- N2 + NaHSO4 + H20 Calculate what must have been the molar concentration of the sodium nitrite.

A sample of 263.0 mL of wet nitrogen gas was collected over water at a total pressure of 756 torr and a temperature of 21.0 °C. (The vapor pressure of water at 21.0 °C is 18.7 torr.) The nitrogen was produced by the reaction of sulfamic acid, HNH,SO3, with 368.5 mL of a solution of sodium nitrite according to the following equation. NaNO2 + HNH2SO3- N2 + NaHSO4 + H20 Calculate what must have been the molar concentration of the sodium nitrite.

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: Fe(s) + H2SO(aq) → FeS0.(aq) + H2(g) The volume of the balloon was 4.8 x10° L. What mass of Fe was…

A: Equation can be written as: Fe(s)+H2SO4→FeSO4(aq)+H2(g) Molar mass of Fe = 56 g/mol H2 = Molar mass…

Q: A 4.0 liter rigid, indestructible metal can is filled with nitrogen gas at 45 °C to a pressure of…

Q: The vapor pressure of mercury at 20 oC is 1.7 x 10-6 atm. Your lab partner breaks a mercury…

A: Given temperature, T = 20 oC + 273.15 = 293.15 K Pressure, P = 1.7*10-6 atm 1 atm = 101325 Pa or…

Q: A 2.00 L reaction container at 25.0 °C contains CO2 (g) and O2 (g). The total pressure of the gases…

A: In this question, total volume of the container is to be determined on addition of 15.0 g of…

Q: A sample of CO2 gas at 150.°C has a volume of 350. mL at 760. mm Hg. How many moles of CO2 are…

A: Ideal gases are those gases which follow ideal gas equation. The relation between pressure, volume,…

Q: A 6.75 g sample of potassium chlorate (KClO4) is heated and decomposes into potassium chloride and…

A: Using Dalton's law of partial pressure to fins oxygen's partial pressurePtotal = PO2 + PH2O and…

Q: In a laboratory where gases are being collected, the atmospheric pressure is 753.5 mm Hg, and the…

A: In a laboratory where gases are being collected, the atmospheric pressure is 753.5 mm Hg, and the…

Q: A 4.0-liter rigid metal can is filled with nitrogen gas at 45 °C to a pressure of 1.125 atm. The can…

Q: A sample of nitrogen gas was collected via water displacement. Since the nitrogen was collected via…

Q: A 0.6333 g sample of a metal carbonate was reacted with hydrochloric acid. The carbon dioxide gas…

A: Given data, Mass of sample = 0.6333 g temperature = 26.0oC Volume of gas over water = 103.80 kPa…

Q: A sample of argon measuring 3.00 L at 27.0°C and 765 torr was bubbled through and collected over…

Q: A sample of 257.0 mL of wet nitrogen gas was collected over water at a total pressure of 759 torr…

Q: Oxygen gas can be prepared by heating potassium chlorate according to the following equation:…

Q: A sample of nitrogen gas had a volume of 500. mL, a pressure in its closed container of 740 torr,…

A: According to ideal gas law, the volume of a gas is directly proportional to the number of moles,…

Q: Hydrogen gas is collected over water at 23.5 °C and an atmospheric pressure of 765 mmHg. Calculate…

A: Hydrogen gas is collected over water at 23.5 °C and an atmospheric pressure of 765 mm Hg. Calculate…

Q: What is the experimental molar mass (that is, calculated from the data given and not taken from the…

A: Given: The volume of hydrogen gas generated = 16.99 mL The mass of magnesium taken = 0.0163 g The…

Q: Suppose that a 26.7-mL volume of HCl solution reactions completely with 55.0 mL of aqueous Na2CO3.…

Q: The vapor pressure of liquid carbon tetrachloride, CCI4, is 100. mm Hg at 296 K. A 0.261 g sample of…

A: Here vapour pressure of liquid CCl4 is 100 mm Hg at 296K .Here 0.261 g of CCl4 was placed in 400 ml…

Q: A sample of 4.72 mol of krypton is confined at low pressure in a volume at a temperature of 68 °C.…

A: Number of mol of Krypton (initial) = 4.72 mol Temperature = 680C Root-mean square speed formula is

Q: A sample of nitrogen gas kept in a container of volume 2.40 L and at a temperature of 27. °C exerts…

A: Ideal gas equation is PV = nRT Where, P is pressure of the gas V is volume of the gas n is no.…

Q: An 89.3 mL sample of wet O2(g) is collected over water at 21.3°C at a barometric pressure of 756…

A: Given :- Volume of wet oxygen = VwO2 = 89.3 mL Total Pressure = Ptotal = PdO2 = 756 mmHg Vapor…

Q: A sample of oxygen gas was collected over water at a barometric pressure of 757.2 mm Hg and a…

Q: The temperature of your water was 22.4 degrees Celsius. The volume of hydrogen collected was 35.5…

A: Temperature = T = 22.4 °C V = 35.5 mL P = 28.32 inches Hg What was the mass of the magnesium…

Q: The partial pressures of CH 4, N 2, and O 2 in a sample of gas were found to be 135 mmHg, 508 mmHg,…

A: Given : Partial pressure of CH4 = 135 mm Hg Partial pressure of N2 = 508 mm Hg And partial pressure…

Q: For many purposes we can treat ammonia (NH3) as an ideal gas at temperatures above its boiling point…

Q: Given the reaction: 2 Al (s) + 6 HCI (aq) --> 2 AICI3 (aq) + 3 H2 (g) A strip of aluminum of unknown…

Q: A 2.43 L volume of hydrogen measured at −150. °C is warmed to 100.°C. Calculate the volume (in L) of…

A: Given: Initial Volume V1 = 2.43 L Initial Temperature T1 = -150 oC= 123 K Final Temperature T2 = 100…

Q: Elemental analysis is performed on an organic liquid with a fishy odor. Vaporization of 275.0 mg of…

A: Given:Mass of compound = 275.0 mg = 275.0 ×10-3 g.Volume of Solution = 110 mL = 110×10-3…

Q: A sample of nitrogen gas has a volume of 167.0 mL at STP. What volume (in mL) does the gas occupy if…

A: 1) Given that: Volume of nitrogen (V1) = 167.0 mL = 0.167 L at STP that is Temperature (T1) = 273 K…

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

A sample of 263.0 mL of wet nitrogen gas was collected over water at a total pressure of 756 torr and a temperature of 21.0 °C. (The
vapor pressure of water at 21.0 °C is 18.7 torr.) The nitrogen was produced by the reaction of sulfamic acid, HNH,SO3, with 368.5 mL
of a solution of sodium nitrite according to the following equation.
NaNO2 + HNH2SO3- N2 + NaHSO4 + H2O
Calculate what must have been the molar concentration of the sodium nitrite.
M

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step by step

Solved in 4 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 student collected 500. mL of nitrogen at a temperature of 20.°C. The next day the student found that the volume had changed to 525 mL. What was the new temperature of the gas?
Water can be decomposed by electrolysis to hydrogen gas and oxygen gas. If 2.33 g of water is decomposed to H2(g) and O2(g) and the gases are collected in a 1.00 L flask over water at 25°C (vapor pressure H2O(l) = 23.8 mm Hg), what is the pressure in the flask?
A 2.62 L volume of hydrogen measured at −148 °C is warmed to 100.°C. Calculate the volume (in L) of the gas at the higher temperature, assuming no change in pressure.
When 0.1 mol of HCl gas is placed in a 10 liter box at 25 degree C, the pressure is about the same as that observed when 0.1 mol of NH3 is placed in an identical box at the same temperature. However, when 0.05 mol of HCl and 0.05 mol of NH3 are mixed in a 10 Liter box at 25 degree C, a noticeable lower pressure is observed. Explain this behavior.
Given the reaction: 2 Al (s) + 6 HCI (ag) --> 2 AICI3 (aq) + 3 H2 (g) A strip of aluminum of unknown mass is reacted with excess hydrochloric acid. When the hydrogen gas is collected over water, it is done so at a temperature of 22.0 °C and fills a flask of volume 32.5 mL. The pressure inside the collection tube is 756.1 mmHg and the water vapor pressure at 22.0 °C is 19.83 torr. Determine the mass of the aluminum strip in milligrams (mg).
A sample of H2(g) was collected over water in a volume of 12.0 mL at 18 °C under atmospheric pressure of 770. Torr. Partial pressure of water is P(H2O, 18 °C) = 16 Torr. Find the mol’s of H2(g) in the sample
73. A 500.-mL sample of O2 gas at 24 °C was prepared by decomposing a 3% aqueous solution of hydrogen peroxide, H2 O2, in the presence of a small amount of manganese catalyst by the reaction 2H2 O2 (aq) → 2H2O (g) + The oxygen thus prepared was collected by displacement of water. The total pressure of gas collected was 755 mm Hg. What is the partial pressure of O2 in the mixture? How many moles of O2 are in the mixture? (The vapor pressure of water at 24 °C is 23 mm Hg.)
A 2.39 L volume of hydrogen measured at −154°C is warmed to 100.°C. Calculate the volume (in L) of the gas at the higher temperature, assuming no change in pressure.