Well weathering adds different elements to rocks which they might not be used to. For example, very hard rain & harsh winds could push a rock, causing it to fall & break off into smaller rocks.
Answer:
O2 is the limiting reactant.
Explanation:
Step 1: Data given
Mass of NH3 = 2.00 grams
Mass of O2 = 2.50 grams
Molar mass NH3 = 17.03 g/mol
Molar mass O2 = 32 g/mol
Step 2: The balanced equation
4NH3(g) + 5O2 (g) → 4NO(g) + 6H2O (g)
Step 3: calculate moles NH3
Moles NH3 = mass NH3 / molar mass NH3
Moles NH3 = 2.00 grams / 17.03 g/mol
Moles NH3 = 0.117 moles
Step 4: Calculate moles O2
Moles O2 = mass / molar mass O2
Moles O2 = 2.50 grams / 32 g/mol
Moles O2 = 0.0781 moles
Step 5: Calculate the limiting reactant
For 4 moles NH3 we need 5 moles O2 to produce 4 moles NO and 6 moles H2O
O2 is the limiting reactant. It will completely be consumed. (0.0781 moles). NH3 is in excess. There will react 4/5 * 0.0781 moles = 0.0625 moles
There will remain 0.117 - 0.0625 = 0.0545 moles NH3
O2 is the limiting reactant.
Your answer would be D. As the circulatory system pumps oxygen rich blood through the body, and the respiratory system helps you to breath. Hope this helps!
Answer:
Mass = 0.697 g
Explanation:
Given data:
Volume of hydrogen = 1.36 L
Mass of ammonia produced = ?
Temperature = standard = 273.15 K
Pressure = standard = 1 atm
Solution:
Chemical equation:
3H₂ + N₂ → 2NH₃
First of all we will calculate the number of moles of hydrogen:
PV = nRT
R = general gas constant = 0.0821 atm.L/mol.K
1atm ×1.36 L = n × 0.0821 atm.L/mol.K × 273.15 K
1.36 atm.L = n × 22.43 atm.L/mol
n = 1.36 atm.L / 22.43 atm.L/mol
n = 0.061 mol
Now we will compare the moles of hydrogen and ammonia:
H₂ : NH₃
3 : 2
0.061 : 2/3×0.061 = 0.041
Mass of ammonia:
Mass = number of moles × molar mass
Mass = 0.041 mol × 17 g/mol
Mass = 0.697 g
Answer:
D. C > B >A
Hope it helps!
Explanation:
From strongest to weakest, the intermolecular forces rank in the following way:
Strongest: Hydrogen bonding. This occurs when compounds contain #"O"-"H"# , #"N"-"H"# , or #"F"-"H"# bonds. ...
Less strong: Dipole-dipole forces. ...
Weakest: London Dispersion Forces.
