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The concentration of a solution of 192 grams dissolved to make 2150 mL of solution is 0.93M. Details about concentration can be found below.
<h3>How to calculate concentration?</h3>
The concentration of a solution can be calculated by dividing the number of moles of the substance by its volume.
no of moles of NH42CO3 = 192g ÷ 96g/mol = 2 mol
Concentration of solution = 2 moles ÷ 2.15L
Concentration of solution = 0.93M
Therefore, the concentration of a solution of 192 grams dissolved to make 2150 mL of solution is 0.93M.
Learn more about concentration at: brainly.com/question/22997914
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The change is that the water will freeze to 0 or minus I don’t know as I’m not to sure
Answer:
30.58 atm
Explanation:
Now recall that the ideal gas equation is given as ;
PV=nRT
Where;
P= pressure of the gas (the unknown)
V= volume of the gas= 2.00L
n= number of moles of the gas= 2.50 mol
T= temperature of the gas= 25.0° + 273 = 298K
R= ideal gas constant = 0.0821 L·atm/mol·K
Given all these parameters, we can now substitute into PV= nRT
Making P the subject of the formula;
P= nRT/V
substituting the given values into the equation;
P= 2.50 × 0.0821 × 298/2.00
P= 30.58 atm
Therefore, the pressure of the gas is 30.58 atm
Answer:
0.33 M
Explanation:
From the question given above, the following data were obtained:
Mass of K₂Cr₂O₇ = 9.67 g
Volume of solution = 100 mL
Molarity =?
Next, we shall determine the number of mole in 9.67 g of K₂Cr₂O₇. This can be obtained as follow:
Molar mass of K₂Cr₂O₇ = (39×2) + (52×2) + (16×7)
= 78 + 104 + 112
= 294 g/mol
Mass of K₂Cr₂O₇ = 9.67 g
Mole of K₂Cr₂O₇ =?
Mole = mass /Molar mass
Mole of K₂Cr₂O₇ = 9.67 / 294
Mole of K₂Cr₂O₇ = 0.033 mole
Next, we shall convert 100 mL to litre (L). This can be obtained as follow:
1000 mL = 1 L
100 mL = 100 mL × 1 L / 1000 mL
100 mL = 0.1 L
Finally, we shall determine the molarity of the solution. This can be obtained as follow:
Mole of K₂Cr₂O₇ = 0.033 mole
Volume of solution = 0.1 L
Molarity =?
Molarity = mole / Volume
Molarity = 0.033 / 0.1
Molarity = 0.33 M
Thus, the molarity of the solution is 0.33 M