A researcher reacted nitrogen with oxygen to produce nitrogen monoxide. (a) Write a balanced equation. (b)...
A researcher reacted nitrogen with oxygen to produce nitrogen monoxide.
(a) Write a balanced equation.
(b) A glass cylinder contains 22.4 L of nitrogen at a pressure of 1.00 atm and a temperature of 25 ∘C. How many moles of nitrogen are in the cylinder.
(c) The limiting reactant for the reaction is oxygen. The researcher used 16.0 g of oxygen. What is the theoretical yield of nitrogen monoxide.
(d) The researcher isolated 14.8 g of nitrogen oxide. What is the percent yield?
Homework Answers
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A researcher reacted nitrogen with oxygen to produce nitrogen
monoxide.
(a) Write a balanced equation.
(b)...
5. If 1.00 mol of nitrogen monoxide gas and 1.00 mol of oxygen gas react, what...
5. If 1.00 mol of nitrogen monoxide gas and 1.00 mol of oxygen gas react, what is the limiting reactant and how many moles of NO are produced from the reaction? 2 NO(g) + O2(g) -> 2 NO(g)
It is desired to produce 7.69 grams of nitrogen monoxide by the following reaction. If the...
It is desired to produce 7.69 grams of nitrogen monoxide by the following reaction. If the percent yield of nitrogen monoxide is 71.9 %, how many grams of oxygen gas would need to be reacted? nitrogen(g) + oxygen( nitrogen monoxide() grams oxygen gas
Nitrogen and oxygen can react to form nitrogen monoxide. Write a balanced chemical equation for this...
Nitrogen and oxygen can react to form nitrogen monoxide. Write a balanced chemical equation for this equilibrium reaction (including states of matter). -Start this reaction by adding 0.012 moles of both nitrogen and oxygen to a 500-mL flask. If Kc = 4.35x10-31, what are the equilibrium concentrations of my three chemicals?
2. a. Nitrogen dioxide and hydrogen are reacted in the gas phase, in the presence of...
2. a. Nitrogen dioxide and hydrogen are reacted in the gas phase, in the presence of a catalyst, to produce ammonia and water; write a balanced equation for this reaction. (2 pts) b. If 73.2 g of nitrogen dioxide and 10.6 g of hydrogen are mixed together and react to form ammonia, identify the limiting reactant and calculate the theoretical yield (in grams) of ammonia produced. (6 pts) c. 12.9 g of ammonia is actually produced in this reaction; based...
3. Consider the potential combustion of nitrogen gas with oxygen to produce nitrogen monoxide. The K...
3. Consider the potential combustion of nitrogen gas with oxygen to produce nitrogen monoxide. The K for this reaction is 4.8 x 10-31 at 25°C. (a) Write the balanced chemical reaction for this equilibrium (b) At equilibrium, what species would be predominately present in a reaction flask (c) In the atmosphere at 25°C and latm pressure, the concentration of nitrogen gas is 0.0330 M and that of oxygen is 0.00810 M. Using these as initial concentrations, determine the concentration of...
7, (16 points) Nitrogen reacts with oxygen to produce nitrogen monoxide. At 2200 °C, Kc =...
7, (16 points) Nitrogen reacts with oxygen to produce nitrogen monoxide. At 2200 °C, Kc = 0.050 for the reaction N2(g) + O2(g) さ 2 NO(g) Find Kp, and the equilibrium partial pressures of NO, N2 and O at equilibrium when each reactant was placed in a flask at initial pressures in which PN, Po, -1.2 atm and PNo -0.022 atm
5. Under a high-pressure atmosphere of oxygen, the compound C7H11O4NS2 is burned. A. Write the balanced...
5. Under a high-pressure atmosphere of oxygen, the compound C7H11O4NS2 is burned. A. Write the balanced equation for this reaction. You may assume all the nitrogen is converted to NO2 and the sulfur is converted to SO3. Coefficients should represent the smallest whole number ratio of all reactants and products – no fractional coefficients. (7.5 pts.) B. If 77.6 g of the compound is burned, what is the mass of each product? (7.5 pts 6. Consider the reaction: Fe2O3(s) +...
Experiment 9-Post-lab Questions 1. Methanol (CH,OH) can be produced by the reaction of carbon monoxide (CO)...
Experiment 9-Post-lab Questions 1. Methanol (CH,OH) can be produced by the reaction of carbon monoxide (CO) with hydrogen (H,). The balanced chemical reaction is: cO@)+2 H, (g)CH,OH() Suppose 14.0 g of carbon monoxide is reacted with 8.0 g of hydrogen. a. Which reactant is the limiting reagent? b. What is the theoretical yield for methanol? c. At the completion of the reaction, how many grams of the excess reagent will remain? 2. Iron(III) oxide (Fe,O,) can be converted to iron...
Ammonia (NH3) gas burns in oxygen to form nitrogen monoxide gas and water vapor. Write the...
Ammonia (NH3) gas burns in oxygen to form nitrogen monoxide gas and water vapor. Write the balanced equation for this reaction (including all physical states). How many litres of nitrogen monoxide are obtained from 1.0 litre of ammonia at the same temperature and pressure throughout the reaction?
Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced...
Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is: 2Mg(s)+O2(g)→2MgO(s) When 10.1 g of Mg are allowed to react with 10.5 g of O2, 13.1 g of MgO are collected. -Determine the limiting reactant for the reaction. -Determine the theoretical yield for the reaction. -Determine percent yield for the reaction.
5. If 1.00 mol of nitrogen monoxide gas and 1.00 mol of oxygen gas react, what is the limiting reactant and how many moles of NO are produced from the reaction? 2 NO(g) + O2(g) -> 2 NO(g)
It is desired to produce 7.69 grams of nitrogen monoxide by the following reaction. If the percent yield of nitrogen monoxide is 71.9 %, how many grams of oxygen gas would need to be reacted? nitrogen(g) + oxygen( nitrogen monoxide() grams oxygen gas
2. a. Nitrogen dioxide and hydrogen are reacted in the gas phase, in the presence of a catalyst, to produce ammonia and water; write a balanced equation for this reaction. (2 pts) b. If 73.2 g of nitrogen dioxide and 10.6 g of hydrogen are mixed together and react to form ammonia, identify the limiting reactant and calculate the theoretical yield (in grams) of ammonia produced. (6 pts) c. 12.9 g of ammonia is actually produced in this reaction; based...
3. Consider the potential combustion of nitrogen gas with oxygen to produce nitrogen monoxide. The K for this reaction is 4.8 x 10-31 at 25°C. (a) Write the balanced chemical reaction for this equilibrium (b) At equilibrium, what species would be predominately present in a reaction flask (c) In the atmosphere at 25°C and latm pressure, the concentration of nitrogen gas is 0.0330 M and that of oxygen is 0.00810 M. Using these as initial concentrations, determine the concentration of...
7, (16 points) Nitrogen reacts with oxygen to produce nitrogen monoxide. At 2200 °C, Kc = 0.050 for the reaction N2(g) + O2(g) さ 2 NO(g) Find Kp, and the equilibrium partial pressures of NO, N2 and O at equilibrium when each reactant was placed in a flask at initial pressures in which PN, Po, -1.2 atm and PNo -0.022 atm
Experiment 9-Post-lab Questions 1. Methanol (CH,OH) can be produced by the reaction of carbon monoxide (CO) with hydrogen (H,). The balanced chemical reaction is: cO@)+2 H, (g)CH,OH() Suppose 14.0 g of carbon monoxide is reacted with 8.0 g of hydrogen. a. Which reactant is the limiting reagent? b. What is the theoretical yield for methanol? c. At the completion of the reaction, how many grams of the excess reagent will remain? 2. Iron(III) oxide (Fe,O,) can be converted to iron...
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