Answer:
54 g is the theoretical yield
Explanation:
This is the reaction:
2H₂ + O₂ → 2H₂O
So 2 moles of hydrogen react with 1 mol of oxygen, to produce 2 mol of water.
If I have 3 moles of H₂ and 2 moles of O₂, the my limiting reactant is the hydrogen.
1 mol of O₂ react with 2 moles of H₂
S 2 mol of O₂ would react with 4 moles (I only have 3 moles)
Then, ratio is 2:2 the same as 1:1
As 2 mol of H₂ produce 2 moles of water, 3 moles of H₂ will produce 3 moles of H₂O.
This is the theoretical yield in moles. Let's convert them to mass (mol . molar mass)
3 mol . 18g/m = 54 g
Answer:
Explanation:
Calcium carbonate decomposes at high temperatures to give calcium oxide and carbon
dioxide as shown below.
CaCO3(s) = CaO(s) + CO2(g)
The Kp for this reaction is 1.16 at 800°C. A 5.00 L vessel containing 10.0 g of CaCO3(s)
was evacuated to remove the air, sealed, and then heated to 800°C. Ignoring the volume
occupied by the solid, what will overall mass percent of carbon in the solid once equilibrium is reached?
Chromium is a metal in nature. So when one chromium is
bonded to another chromium, there is a weak intermolecular forces which helds
them together which we call as “metallic bonding”.
Metallic bonding is the intermolecular force of attraction which
exist between valence electrons and the metal atoms. It is considered as the
sharing of various detached electrons between many positive ions, whereby the
electrons serve as a "glue" which gives the substance a definite
structure.
It’s is 130 that is the answer!!!!
Answer:
mass of hydrogen collected is 0.016 gram
Explanation:
Given values:
For calculating mass we have to find the number of moles first
Ideal gas equation PV =nRT
Volume= 195 ml
Pressure: 753 torr =0.99 atm
Temperature: 25+273= 298 Kelvin
Ideal gas constant R= 0.0821 Latm/molK
Number of moles n= ?
So n= PV/RT
Adding the values
n= = (753 torr)(1 atm/760 torr)(195 mL)(1 L/1000 mL)/(0.0821 L·atm/mol·K)(273 K)
n = 0.007897 moles of H₂
Now mass of hydrogen collected = number of moles x Molar mass of H₂
= 0.007897 x 2
= 0.0157 g H₂
Now mass of hydrogen collected is 0.016 gram (rounding the amount)