When sulfuric acid is added to sodium hydroxide a reaction occurs to produce two products.
1 answer:
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126 grams of H2O is formed.
Explanation:
Data given:
volume of the gas = 88 Liters
pressure = 720 mm Hg or 0.947 atm
temperature T = 22 Degrees or 295.15 K
R = 0.08021 atm L/mole K
n =?
The formula is used is of ideal gas law to know the number of moles of CH4 undergoing combustion.
PV = nRT
n =
putting the values in the equation
= 0.947 X 88/ 0.08021 X 295.15
n = 3.5 moles
balanced reaction for combustion of methane
CH4 + O2 ⇒ CO2 + 2H20
1 mole of CH4 undergoes combustion to form 2 moles of water
3.5 moles will give x moles of water
2/1 = x/3.5
x = 7 moles of water (atomic mass of water = 18 gram/mole)
mass = atomic mass x number of moles
mass = 18 x 7
=126 grams of water is formed.
Answer:
a. 0.50 g, 1.0 g, 1.5 g, 2.0 g, 2.5 g;
g. 0.1 g, 0.5 g, 1.0 g, 1.5 g, 2.0 g
Explanation:
The percent mass is defined as a ratio between the mass of a solute and mass of a solution:
Since solution only consists of a solute and solvent, express its mass as:
Then:
Firstly, solve for how much mass is required to prepare 3.0 %. Let's say, we have x g of the solute:
Similarly, solve for 6.0 %, let's say, we have x g of the solute again:
Hence, masses should be in a range of 0.93 g to 1.91 g.