please answer 1 & 2 thank you 1. limiting Reactant - Mass to Mass: Perform two...
please answer 1 & 2 thank you
1.
limiting Reactant - Mass to Mass: Perform two calculations to determine the limiting reactant and amount of product produced.
Hydrogen cyanide, a highly toxic compound, is made by the following reaction:
2 CH4(g) + 2 NH3(g) + 3
O2(g) → 2 HCN(g) + 6
H2O(g)
What is the limiting reagent with respect to HCN production if 45.4
g of O2 are added to 23.8 g of NH3? (assume
CH4 is in excess)
ammonia
oxygen
What is the mass of HCN that can be produced from these reactants?
Express your answer to two decimal places.
g
10.
1.2/1.81 pointsPrevious AnswersMy Notes
2.
Limiting Reactant - Mass to Mass - Percent Yield: Perform two calculations to determine the limiting reactant and theoretical amount of product produced. For percent yield, compare the experimental mass to theoretical mass (experimental / theoretical * 100).
Balance the following equation for the formation of ammonia from nitrogen gas and hydrogen gas (if the coefficient = 1, you must enter 1 into the box):
a. If 7.73 g of nitrogen gas and 5.2 g of hydrogen gas are used,
what is the limiting reactant?
nitrogen
hydrogen
b. What is the theoretical yield of ammonia? Express your answer to
two decimal places.
g
c. What is the percent yield for this reaction if 9.211762154 g of
ammonia are obtained experimentally? Express your answer to two
significant figures.
%
Homework Answers
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please answer 1 & 2 thank you
1.
limiting Reactant - Mass to Mass: Perform two...
1. Moles of Reactant to Mass of Reactant: Identify the iodide ions and ozone in the...
1. Moles of Reactant to Mass of Reactant: Identify the iodide ions and ozone in the balanced chemical equation. Use mole ratio, then convert to grams. A method used by the EPA for determining the ozone concentration in the air is to pass an air sample through a bubbler containing iodide ions. The iodide ions remove the ozone according to the following reaction: O3(g) + 2 I-(aq) + H2O(l) → O2(g) + I2(aq) + 2 OH-(aq) How many grams of ozone...
Identify limiting reactants (maximum product method). Consider the reaction of methane with ammonia and oxygen. 2CH4...
Identify limiting reactants (maximum product method). Consider the reaction of methane with ammonia and oxygen. 2CH4 (g) + 2NH3(g) + 302 (g) —2HCN (g) + 6H20 (1) Determine the limiting reactant in a mixture containing 175 g of CH4, 160 g of NH3, and 607 g of O2. Calculate the maximum mass (in grams) of hydrogen cyanide, HCN, that can be produced in the reaction. The limiting reactant is: CH4 O2 NH3 Amount of HCN formed = g
Consider the reaction of methane with ammonia and oxygen. 2CH4 (g) + 2NH3 (g) + 3O2...
Consider the reaction of methane with ammonia and oxygen. 2CH4 (g) + 2NH3 (g) + 3O2 (g) -> 2HCN (g) + 6H2O (l) Determine the limiting reactant in a mixture containing 136 g of CH4, 231 g of NH3, and 501 g of O2. Calculate the maximum mass (in grams) of hydrogen cyanide, HCN, that can be produced in the reaction. The limiting reactant is: 1. O2 2. CH4 3. NH3 Amount of HCN formed = g
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...
1) If the percent yield for the following reaction 80.0%, how many grams of KClO3 are...
1) If the percent yield for the following reaction 80.0%, how many grams of KClO3 are needed to produce 42.0 g of O2? 2 KClO3 (s) > 2 KCl (s) + 3O2 (g) A) 134g B) 10.5g C) 63.0g D) 62.5g 2) 5.0g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below. Which one of the following statements is false? N2 (g) + 3 H2 (g) > 2 NH3 (g)...
Please help with these questions 1. Methane (CH4) burns in air to form carbon dioxide and...
Please help with these questions
1. Methane (CH4) burns in air to form carbon dioxide
and water as shown below.
CH4(g) + 2 O2(g) → CO2(g) + 2
H2O(l)
If a sample of methane occupies 802. mL at 3.23 atm, what
pressure (in atm) of oxygen gas with the same temperature and
volume is required to complete the reaction?
2. Consider the reaction between hydrogen gas and nitrogen gas
to form ammonia:
3 H2(g) + N2(g) → 2 NH3(g).
What...
Limiting Reactants, Excess Reactant, and % Yield Name H2+Cl2HCI A gaseous mixture containing 7.5 g of H; gas and 9....
Limiting Reactants, Excess Reactant, and % Yield Name H2+Cl2HCI A gaseous mixture containing 7.5 g of H; gas and 9.00 g of Cl2 gas react to form hydrogen chloride gas. а) Which is the limiting reactant? If all the limiting reactant is consumed, how many grams of HCl are produced? How many grams of excess reactant remain un-reacted? b) c) Cl2+3F22CIF Chlorine reacts with fluorine to form gaseous chlorine trifluoride. You start with 50.0g of chlorine and 95.0g of fluorine....
--xal Yield and Percent Yield combusts with oxygen to form carbon dioxide and water by the...
--xal Yield and Percent Yield combusts with oxygen to form carbon dioxide and water by the following reaction: pentane combud CsHız(l) + 8 O2(g) → 5 CO2(g) + 6 H2O(g) a. If 8.00 g of pentane is mixed with 10.0 g of oxygen, which is the limiting reactant? (Hint: compare it to either of the products). b. What is the theoretical yield (in grams) of carbon dioxide and water for this reaction? Hydrogen reacts with nitrogen to form ammonia by...
Identity limiting reactants (maximum product method). Consider the reaction of methane with ammonia and oxygen 2CH,...
Identity limiting reactants (maximum product method). Consider the reaction of methane with ammonia and oxygen 2CH, (g) + 2NH3 (9) +302 (9) —2HCN) + 6H20 (1) Determine the limiting reactant in a mixture containing 129 g of CH, 152 g of NH3, and 348 g of Oz Calculate the maximum mass (in grams) of hydrogen cyanide, HCN, that can be produced in the reaction The limiting reactant is. OCH4 O NH3 Amount of HCN formed
Ammonia NH3 may react with water to form oxygen and nitrogen gas . if 2.55g of...
Ammonia NH3 may react with water to form oxygen and nitrogen gas
.
if 2.55g of NH3 reacts with 3.83g O2 and produces .950L of N2
at 295k and 1.00atm , which reactant is limiting ?
what is the percent yeild of the reaction ?
Ammonia, NH3, may react with oxygen to form nitrogen gas and water. 4NH,(aq) +30,(8) 2N,(s) + 6H,0(1) if 2.55 g of NH3 reacts with 3.83 g Og and produces 0.950 L of N2, at 295...
Identify limiting reactants (maximum product method). Consider the reaction of methane with ammonia and oxygen. 2CH4 (g) + 2NH3(g) + 302 (g) —2HCN (g) + 6H20 (1) Determine the limiting reactant in a mixture containing 175 g of CH4, 160 g of NH3, and 607 g of O2. Calculate the maximum mass (in grams) of hydrogen cyanide, HCN, that can be produced in the reaction. The limiting reactant is: CH4 O2 NH3 Amount of HCN formed = g
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...
Please help with these questions
1. Methane (CH4) burns in air to form carbon dioxide
and water as shown below.
CH4(g) + 2 O2(g) → CO2(g) + 2
H2O(l)
If a sample of methane occupies 802. mL at 3.23 atm, what
pressure (in atm) of oxygen gas with the same temperature and
volume is required to complete the reaction?
2. Consider the reaction between hydrogen gas and nitrogen gas
to form ammonia:
3 H2(g) + N2(g) → 2 NH3(g).
What...
Limiting Reactants, Excess Reactant, and % Yield Name H2+Cl2HCI A gaseous mixture containing 7.5 g of H; gas and 9.00 g of Cl2 gas react to form hydrogen chloride gas. а) Which is the limiting reactant? If all the limiting reactant is consumed, how many grams of HCl are produced? How many grams of excess reactant remain un-reacted? b) c) Cl2+3F22CIF Chlorine reacts with fluorine to form gaseous chlorine trifluoride. You start with 50.0g of chlorine and 95.0g of fluorine....
--xal Yield and Percent Yield combusts with oxygen to form carbon dioxide and water by the following reaction: pentane combud CsHız(l) + 8 O2(g) → 5 CO2(g) + 6 H2O(g) a. If 8.00 g of pentane is mixed with 10.0 g of oxygen, which is the limiting reactant? (Hint: compare it to either of the products). b. What is the theoretical yield (in grams) of carbon dioxide and water for this reaction? Hydrogen reacts with nitrogen to form ammonia by...
Identity limiting reactants (maximum product method). Consider the reaction of methane with ammonia and oxygen 2CH, (g) + 2NH3 (9) +302 (9) —2HCN) + 6H20 (1) Determine the limiting reactant in a mixture containing 129 g of CH, 152 g of NH3, and 348 g of Oz Calculate the maximum mass (in grams) of hydrogen cyanide, HCN, that can be produced in the reaction The limiting reactant is. OCH4 O NH3 Amount of HCN formed
Ammonia NH3 may react with water to form oxygen and nitrogen gas
.
if 2.55g of NH3 reacts with 3.83g O2 and produces .950L of N2
at 295k and 1.00atm , which reactant is limiting ?
what is the percent yeild of the reaction ?
Ammonia, NH3, may react with oxygen to form nitrogen gas and water. 4NH,(aq) +30,(8) 2N,(s) + 6H,0(1) if 2.55 g of NH3 reacts with 3.83 g Og and produces 0.950 L of N2, at 295...
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