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zmey [24]
2 years ago
12

How many moles of cacl2 are in 250 ml of a 3.0 m of cacl2 solution?

Chemistry
2 answers:
Margarita [4]2 years ago
8 0
The appropriate response is Proximity. Purposes behind going out on a limb of living unlawfully in another nation are not just the normal upgrades in pay and living conditions yet, in addition, the expectation of in the long run being permitted to stay in the nation legitimately, as there might be a way to getting to be plainly naturalized. Living in another nation wrongfully incorporates an assortment of confinements, and additionally the danger of being kept and expelled or of confronting different authorizations
posledela2 years ago
7 0
To determine the number of moles of CaCl2 in 250 mL of a 3.0 M of CaCl2 solution, first note that the unit M refers to molarity which is a unit of concentration that means moles per liter of solution. Thus, simply convert 250 mL to liters then multiply it to 3.0 M. We then have:

250 mL x 1 L/1000 mL x 3 mol/L CaCl2 = 0.75 mol CaCl2

Thus, there are 0.75 mol CaCl2 in 250 mL of a 3.0 M of CaCl2 solution.  
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Combined gas law problem: a balloon is filled with 500.0 mL of helium at a temperature of 27 degrees Celsius and 755 mmHg. As th
Papessa [141]
The statement of the combined gas law for a fixed amount of gas is,
PV/T = constant
Here, the units of pressure and volume must be consistent and the temperature must be the absolute temperature (Kelvin or Rankine).
0.65 atm is equivalent to 494 mmHg
Using the equation:
(755 x 500) / (27 + 273) = (494 x V) / (-33 + 273)
V = 3396 ml = 3.4 liters
8 0
2 years ago
What elements are in NaC2HO4 and how many atoms are in each element​
JulijaS [17]

Answer:

Each molecule contains one atom of A and one atom of B. The reaction does not use all of the atoms to form compounds.

                 A + B ⟶ Product

Particles: 6      8              6

If six A atoms form six product molecules, each molecule can contain only one A atom.

The formula of the product is ABₙ.

If n = 1, we need six atoms of B.

If n = 2, we need 12 atoms of B. However, we have only eight atoms of B, so the formula of the product must be AB.

Thus, 6A + 6B ⟶ 6AB, with two B atoms left over.

Explanation:

Credit goes to @znk

Hope it helps you :))

7 0
2 years ago
A student has a mixture of salt (NaCl) and sugar (C12H22O11). To determine the percent composition, the student measures out 5.8
ra1l [238]

Answer:

<u>1. Net ionic equation:</u>

  • Cl⁻(aq) +  Ag⁺(aq) → AgCl(s)

<u />

<u>2. Volume of 1.0M AgNO₃</u>

  • 41ml

Explanation:

1. Net ionic equation for the reaction of NaCl with AgNO₃.

i) Molecular equation:

It is important to show the phases:

  • (aq) for ions in aqueous solution
  • (s) for solid compounds or elements
  • (g) for gaseous compounds or elements

  • NaCl(aq) + AgNO₃(aq) → AgCl(s) + NaNO₃(aq)

ii) Dissociation reactions:

Determine the ions formed:

  • NaCl(aq) → Na⁺(aq) + Cl⁻(aq)
  • AgNO₃(aq) → Ag⁺(aq) + NO₃⁻(aq)
  • NaNO₃(aq) → Na⁺(aq) + NO₃⁻(aq)

iii) Total ionic equation:

Substitute the aqueous compounds with the ions determined above:

  • Na⁺(aq) + Cl⁻(aq) +  Ag⁺(aq) + NO₃⁻(aq) → AgCl(s) +  Na⁺(aq) + NO₃⁻(aq)

iv) Net ionic equation

Remove the spectator ions:

  • Cl⁻(aq) +  Ag⁺(aq) → AgCl(s) ← answer

2.  How many mL of 1.0 M AgNO₃ will be required to precipitate 5.84 g of AgCl

i) Determine the number of moles of AgNO₃

The reaction is 1 to 1: 1 mole of AgNO₃ produces 1 mol of AgCl

The number of moles of AgCl is determined using the molar mass:

  • number of moles = mass in grams / molar mass
  • molar mass of AgCl = 143.32g/mol
  • number of moles = 5.84g / (143.32g/mol) = 0.040748 mol

ii) Determine the volume of AgNO₃

  • molarity = number of moles of solute / volume of solution in liters

  • 1.0M = 0.040748mol / V

  • V = 0.040748mol / (1.0M) = 0.040748 liter

  • V = 0.040748liter × 1,000ml / liter = 40.748 ml

Round to two significant figures: 41ml ← answer

4 0
2 years ago
Acetaminophen (pictured) is a popular nonaspirin, "over-the-counter" pain reliever. what is the mass % (calculate to 4 significa
77julia77 [94]

Acetaminophen as a chemical formula of C8H9NO2. The molar masses are:

C8H9NO2 = 151.163 g/mol

C = 12 g/mol

H = 1 g/mol

N = 14 g/mol

O = 16 g/mol

 

<span>TO get the mass percent, simply multiply the molar mass of each elements  with the number of the element divide by the molar mass of acetaminophen, that is:</span>

%C = [(12 * 8) / 151.163] * 100% = 63.50%

%H = [(1 * 9) / 151.163] * 100% = 5.954%

%N = [(14 * 1) / 151.163] * 100% = 9.262%

<span>%O = [(16 * 2) / 151.163] * 100% = 21.17% </span>

8 0
2 years ago
What is the final pressure (expressed in atm) of a 3.05 l system initially at 724 mm hg and 298 k, that is compressed to a final
krok68 [10]

<u>Answer:</u>

P2 = 778.05 mm Hg = 1.02 atm

<u>Explanation:</u>

We are to find the final pressure (expressed in atm)  of a 3.05 liter system initially at 724 mm hg and 298 K which is compressed to a final volume of 2.60 liter at 273 K.

For this, we would use the equation:

\frac{P_1V_1}{T_1} =\frac{P_2V_2}{T_2}

where P1 = 724 mm hg

V1 = 3.05 L

T1 = 298 K

P2 = ?

V2 = 2.6 L

T2 = 173 K

Substituting the given values in the equation to get:

\frac{(724)(3.05)}{298} =\frac{P_2(2.6)}{173}

P2 = 778.05 mm Hg = 1.02 atm

7 0
2 years ago
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