The reactant is the chemical reaction of 2 or more different elements.
The product is what is formed in a chemical reaction.
Example: H + O ----> H2O
H + O is the reactants, and H2O is the products.
Answer:
(a) 0.25 mol
(b) 0.11 mol
(c) 8.77 mol
Explanation:
(a)
We use the equation given by ideal gas which follows:
where,
P = pressure of the gas = 1.00 atm
V = Volume of the gas = 6.0 L
T = Temperature of the gas = 298 K
R = Gas constant =
n = number of moles = ?
Putting values in above equation, we get:
(b)
We use the equation given by ideal gas which follows:
where,
P = pressure of the gas = 0.296 atm
V = Volume of the gas = 6.0 L
T = Temperature of the gas = 200 K
R = Gas constant =
n = number of moles = ?
Putting values in above equation, we get:
(c)
We use the equation given by ideal gas which follows:
where,
P = pressure of the gas = 30 atm
V = Volume of the gas = 6.0 L
T = Temperature of the gas = 250 K
R = Gas constant =
n = number of moles = ?
Putting values in above equation, we get:
Answer:
16.27 g of CaCO3 are produced upon reaction of 45 g CaCN2 and 45 g of H2O.
Explanation:
Ca(CN)2 + 3H2O → CaCO3 + 2 NH3
First of all, let's find out the limiting reactant.
Molar mass Ca(CN)2.
Molar mass H2O: 18 g/m
Moles of Ca(CN)2: mass / molar mass
45 g / 92.08 g/m = 0.488 moles
Moles of H2O: mass / molar mass
45g / 18g/m = 2.50 moles
This is my rule of three
1 mol of Ca(CN)2 needs 3 moles of H2O
2.5 moles of Ca(CN)2 needs (2.5 . 3) / 1 = 7.5 moles
I need 7.5 moles of water, but I only have 0.488. Obviously water is the limiting reactant; now we can work on it.
3 moles of water __ makes __ 1 mol of CaCO3
0.488 moles of water __ makes ___ (0.488 . 1) / 3 = 0.163 moles
Molar mass CaCO3 = 100.08 g/m
Molar mass . moles = mass
100.08 g/m . 0.163 moles = 16.27 g
Acid-Base Reactions. When an acid and a base are placed together, they react to neutralize the acid and base properties, producing a salt. The H(+) cation of the acid combines with the OH(-) anion of the base to form water.
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