Answer:
The answer to your question is:
a) Hydrogen
b) 850 g of NH3
c) 300 g of N2
Explanation:
N2 + 3H2 ⇒ 2NH3
N2 = 1000 g
H2 = 150 g
a. Identify the limiting reactant.
MW N2 = 28 g
MW H2 = 2 g
MW NH3 = 17g
N2 + 3H2 ⇒ 2NH3
28g ------ 3(2)
1000 g ------ x
x = (1000 x 6)/ 28
x = 214.3 g of H2
Then, the limiting reactant is H2, because is necessary to have 214.3 g of H2 to react with 1000 g of N2, and there are only 150 g.
b. Calculate the theoretical yield in grams of NH3. __________
N2 + 3H2 ⇒ 2NH3
6g -----------2(17)g
150g --------- x
x = (150 x 34) / 6
x = 850 g of NH3
c. Calculate the grams of excess reactant. __________
N2 + 3H2 ⇒ 2NH3
28g -------- 6 g
x ----------- 150 g
x = (150 x 28)/ 6
x = 700 g of N2
Excess reactant = 1000g - 700g
= 300 g of N2
In an endothermic change, temperature is absorbed from surrounding molecules to continue reacting. If these molecules are losing heat, that means their temperature will drop, resulting in a temperature decrease.
The heat that is released by the combustion of 3.5 moles of methane is 3115 kJ/mol.
<h3>What is a thermochemical equation?</h3>
A thermochemical equation is a reaction equation that incorporates the amount of heat lost/gained.
In this case, the reaction equation is; CH4 + O2 ----->CO2 + 2H2O dH = -890 kJ/mol
If 1 mole of methane releases 890 kJ/mol
3.5 moles of methane will release 3.5 moles * 890 kJ/mol/1 mole
= 3115 kJ/mol
Learn more about combustion reaction:brainly.com/question/12172040?
#SPJ1
The answer would be false:)
in my opinion
The mass of Ca(CN)2 : 92,11 g/mol
<h3>Further explanation</h3>
Given
0.0321 moles of Ca(CN)2
Required
The mass
Solution
The mole is the number of particles contained in a substance
1 mol = 6.02.10²³
Moles can also be determined from the amount of substance mass and its molar mass
mol(n) = mass(m) : MW(molecular weight)
Input the value :
mass = mol x MW Ca (CN)2
mass = 0.0321 x 92,11 g/mol
mass = 2.957 g
