Answer:
C- A solution of salt water
Explanation:
You cannot see the salt within the water, for it has already dissolved. The contents are uniformly distributed throughout the water's volume.
I hope this made sense! (^-^)
Answer:
62.98 % of the sample of hydrate is water
Explanation:
Step 1: Data given
Mass of the sample of a hydrate of sodium carbonate (Na2CO3) = 2.026 grams
After heating, the mass of the sample is 0.750 g
Molar mass H2O = 18.02 g/mol
Step 2: Calculate mass of water
Mass water = mass of hydrate - mass of sample after heating
Mass water = 2.026 grams - 0.750 grams
Mass water = 1.276 grams
Step 3: Calculate mass % percent of water
Mass % of water = (mass of water / total mass hydrate) * 100 %
Mass % of water = (1.276 grams / 2.026 grams) *100 %
Mass % of water = 62.98 %
62.98 % of the sample of hydrate is water
2H2O -> 2H2 + O2
Stoichiometric ratio:
2 : 2 : 1
H2O : O2
2 : 1
Mass of 1 mol of H2O = [(2 x 1) + 16] g = 18g
18g of H2O = 1 mol of H2O
90g of H2O = 90g x 1 mol / 18g
= 5 mol of H2O
2 mol of H2O : 1 mol of O2
5 mol of H2O : 5/2 mol of O2
1 mol of O2 = 22.4 L of O2
5/2 mol of O2 = 5/2 mol x 22.4 L / 1 mol
= 56 L of O2
Coal does not produce flame when burnt because it does not vapourizes
Answer: A) 0.20 L
Explanation:
Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.
According to the neutralization law,
![M_1V_1=M_2V_2](https://tex.z-dn.net/?f=M_1V_1%3DM_2V_2)
where,
= molarity of stock
solution = 10.0 M
= volume of stock
solution = ?
= molarity of dilute
solution = 0.50 M
= volume of dilute
solution = 4.0 L
![10.0\times V_1=0.50\times 4.0](https://tex.z-dn.net/?f=10.0%5Ctimes%20V_1%3D0.50%5Ctimes%204.0)
![V_1=0.20L](https://tex.z-dn.net/?f=V_1%3D0.20L)
Therefore, the volume of 10.0 M
solution needed to prepare 4.0 L of 0.50 M
is 0.20 L