Nitrous oxide (dinitrogen monoxide) is an anesthetic often referred to as laughing gas. What is its...
Dinitrogen monoxide, commonly known as laughing gas, is used in dental procedures as an anesthetic. At elevated temperatures, dinitrogen monoxide can be produced from the reaction of ammonia and oxygen: 2 NH3 (g) + 2 O2 (g) ---> N2O (g) + 3 H2O (g) If you begin with 7.8 L of NH3 (g), what is the theoretical yield of H2O in liters?
Dinitrogen oxide, commonly called laughing gas, is sometimes used as an anesthetic in dentistry. It is produced by the decomposition of ammonium nitrate. The other product of this reaction is water. A balanced equation indicates the mole ratios of reactants and products. The molar mass of a substance allows you to convert between moles and mass. ______________________________________________________________________________ Write the balanced equation for the production of dinitrogen oxide and water from ammonium nitrate. How many grams of ammonium nitrate are required...
Nitrous oxide (N2O) is used as an anesthetic (laughing gas) and in aerosol cans to produce whipped cream. It is also a potent greenhouse gas. The decomposition of N2O is first order. It decomposes slowly to N2 and O2: How many half-lives will it take for the concentration of the N2O to reach 25.00 % of its original concentration?
Part A Nitrous axide, N20, is a common anesthetic also known as laughing gas, or simply "Cnitrous If a cylinder of nitrous contains 3.1 kg of NgO what volume of N,O can be obtained from this cinder temperature of 20 C and standard pressure of 1.00 atm? (R 0.0821 L atm/(moke K)) Express your answer to two significant figures and include the appropriate units. uA Value Umits Volume Request Answer Submt Provide Feedback
1A. The decomposition of dinitrogen monoxide (nitrous oxide) occurs in two steps. The mechanism that has been proposed is as follows: Step 1: N2O (g) à N2(g) + O(g) Step 2: N2O (g) + O(g) à N2(g) + O2(g) Write the chemical equation for the overall reaction and identify any reaction intermediates (spectators). What is the molecularity of each of the elementary (steps) reactions?
A 10.00 L tank at 23.2 degrees Celsius is filled with 15.8 g of dinitrogen monoxide gas and 4.94 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. What is the mole fraction and partial pressure for dinitrogen monoxide? Mole fraction: ? Partial pressure: ? atm What is the mole fraction and partial pressure for sulfur tetrafluoride? Mole fraction:? Partial pressure: ? atm What is the total pressure in the tank? Round...
A 10.00 L tank at 9.3 °C is filled with 14.3 g of dinitrogen monoxide gas and 2.62 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas dinitrogen monoxide sulfur tetrafluoride mole fraction Chock Explanation
A 8.00 L tank at 4.51 C is filled with 7.57 g of dinitrogen monoxide gas and 6.21 R of sulfur tetrafluoride gas. You can assure both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: dinitrogen monoxide partial pressure: X 5 ? mole fraction: ultur teruoride partial pressure Total pressure in tank
When dinitrogen pentoxide reacts with nitrogen dioxide, the products are nitrogen monoxide and molecular oxygen. If 50.00 g of dinitrogen pentoxide reacts with excess molecular oxygen at 28.0oC and the products are collected in a 700.0 L tank, what is the partial pressure of each gas and what is the total pressure in the tank assuming the reaction goes to completion? The unit for pressure should be in atm. NOTE: YOU MUST USE MOLE FRACTIONS FOR THE PARTIAL PRESSURES
You have (6.01x10^2) ml of dinitrogen monoxide gas at (9.330x10^-1) atm and (6.350x10^1)°C. What is the mass (in g) of the sample?