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weeeeeb [17]
3 years ago
8

In a group assignment, students are required to fill 10 beakers with 0.720 M CaCl2. If the molar mass of CaCl2 is 110.98 g/mol a

nd each beaker must have 250. mL of solution, what mass of CaCl2 would be used? 3.13 g 38.5 g 200 g 617 g
Chemistry
2 answers:
8_murik_8 [283]3 years ago
8 0
The answer is 200 g.

If the molar mass of CaCl2 is 110.98 g/mol, this means there are 110.98 g in 1 L of 1 M solution.
Let's find how many g of CaCl2 are present in 0.720 M.
110.98 g : 1 M = x : 0.720 M
x = 110.98 g * 0.720 M : 1 M 
x = 79.90 g

So there are 79.90 g in 0.720 M. In other words, in 1 L of 0.720 M solution there will be  79.90 g.

Now, we need to prepare ten beakers with 250 mL of solutions:
10 * 250 mL = 2500 mL = 2.5 L

79.90 g : 1 L = x : 2.5 L
x = 79.90 g * 2.5 L : 1 L
x = 199.75 g ≈ 200 g
inn [45]3 years ago
8 0

Answer: C. 200g

Explanation: Just took the test, it's correct.

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Explanation:

An ideal gas is a theoretical gas that is considered to be made up of point particles that move randomly and do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

The Pressure (P) of a gas on the walls of the container that contains it, the Volume (V) it occupies, the Temperature (T) at which it is located and the amount of substance it contains (number of moles, n) are related from the equation known as Equation of State of Ideal Gases:

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