19.09.2020

How many grams of KBr are dissolved in 92.7 mL of a 0.955 M solution? Show your work.

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09.07.2023, solved by verified expert
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10.5g of KBr

Explanation:

molarity = moles of solute / litres of solution

we are given the volume of the solution in milliliters but the formula uses litres so we have to convert

to convert to liters we divide the number of milliliters by 1000 ( because 1 liter has 1000 milliliters. )

so liters of solution = 92.7/1000 = 0.0927 L

we can now plug in what we are given and solve for moles of solute

recall molarity = moles of solute / litres of solution

molarity = 0.955M and liters of solution = 0.0927L

so How many grams of KBr are dissolved in 92.7 mL, №18011175, 19.09.2020 17:13

multiply both sides by 0.0927

we're left with moles of solute = 0.0885285 moles

Finally we must convert moles to grams

Molar mass of KBr = 39.0983 + 79.904 =  g/mol

Using dimensional analysis we get How many grams of KBr are dissolved in 92.7 mL, №18011175, 19.09.2020 17:13

the mol KBr cancel out on both sides and we get How many grams of KBr are dissolved in 92.7 mL, №18011175, 19.09.2020 17:13 which is equal to 10.5g (rounded)

So we can conclude that 10.5g of KBr is dissolved in 92.7mL of a 0.955M solution.

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Chemistry
Step-by-step answer
P Answered by Master

10.5g of KBr

Explanation:

molarity = moles of solute / litres of solution

we are given the volume of the solution in milliliters but the formula uses litres so we have to convert

to convert to liters we divide the number of milliliters by 1000 ( because 1 liter has 1000 milliliters. )

so liters of solution = 92.7/1000 = 0.0927 L

we can now plug in what we are given and solve for moles of solute

recall molarity = moles of solute / litres of solution

molarity = 0.955M and liters of solution = 0.0927L

so 0.955M=\frac{moles.of.solute}{0.0927L}

multiply both sides by 0.0927

we're left with moles of solute = 0.0885285 moles

Finally we must convert moles to grams

Molar mass of KBr = 39.0983 + 79.904 =  g/mol

Using dimensional analysis we get \frac{0.0885285molKBr}{} *\frac{119.002g}{1molKBr}

the mol KBr cancel out on both sides and we get 0.0885285 *119.002g which is equal to 10.5g (rounded)

So we can conclude that 10.5g of KBr is dissolved in 92.7mL of a 0.955M solution.

Chemistry
Step-by-step answer
P Answered by Specialist
Answer: b. Fiona is correct because the diagram shows two individual simple machines.

Explanation:
A mechanical device using which we can change the direction or magnitude of force applied is known as simple machine.
For example, in the given diagram there are two individual simple machines.
The machine helps in changing the direction or magnitude of force applied by the man. As a result, it becomes easy for him to carry different things easily from one place to another.
Thus, we can conclude that the statement Fiona is correct because the diagram shows two individual simple machines, is correct.
Answer: b. Fiona is correct because the diagram shows two individual simple machines.

Explanation
Chemistry
Step-by-step answer
P Answered by PhD

Answer:

52.6 gram

Step-by-step explanation:

It is clear by the equation 2(27+3×35.5)= 267 gm of AlCl3 reacts with 6× 80 = 480 gm of Br2 . So 29.2 gm reacts = 480× 29.2/267= 52.6 gm

Chemistry
Step-by-step answer
P Answered by PhD
15 moles.Explanation:Hello,In this case, the undergoing chemical reaction is:Clearly, since carbon and oxygen are in a 1:1 molar ratio, 15 moles of carbon will completely react with 15 moles of oxygen, therefore 15 moles of oxygen remain as leftovers. In such a way, since carbon and carbon dioxide are also in a 1:1 molar ratio, the theoretical yield of carbon dioxide is 15 moles based on the stoichiometry:Best regards.
Chemistry
Step-by-step answer
P Answered by PhD
Answer: 25 g
Explanation: Given:
Original amount (N₀) = 100 g
Number of half-lives (n) = 11460/5730 = 2
Amount remaining (N) = ?
N = 1/2ⁿ × N₀
N = 1/2^2 × 100
N = 0.25 × 100
N = 25 g
Chemistry
Step-by-step answer
P Answered by PhD
Answer: 7.8125 g
Explanation: Given:
Original amount (N₀) = 500 g
Number of half-lives (n) = 9612/1602 = 6
Amount remaining (N) = ?
N = 1/2ⁿ × N₀
N = 1/2^6 × 500
N = 0.015625 × 500
N = 7.8125 g
Chemistry
Step-by-step answer
P Answered by PhD
Answer: The product formed is potassium chloride.
Explanation:
Precipitation reaction is defined as the chemical reaction in which an insoluble salt is formed when two solutions are mixed containing soluble substances. The insoluble salt settles down at the bottom of the reaction mixture.

The chemical equation for the reaction of potassium phosphate and magnesium chloride follows (look at the picture)

2 moles of aqueous solution of potassium phosphate reacts with 3 moles of aqueous solution of magnesium chloride to produce 1 mole of solid magnesium phosphate and 6 moles of aqueous solution of potassium chloride.
Answer: The product formed is potassium chloride.
Explanation:
Precipitation reaction is defined a
Chemistry
Step-by-step answer
P Answered by PhD
Answer: B. carbon tetrachloride, CCI4
Explanation: The other options are incorrect. Let's write the correct formulas:
A. Diarsenic pentoxide - As2O5
C. Sodium dichromate - Na2Cr2O7
D. magnesium phosphide - Mg3P2
Chemistry
Step-by-step answer
P Answered by PhD
Answer: a. basic
b. basic
c. acidic
d. neutral

Explanation: Acids and bases can be classified in terms of hydrogen ions or hydroxide ions, or in terms of electron pairs. (look at the picture)
Let us note that from the pH scale, a pH of;
0 - 6.9 is acidic
7 is neutral
8 - 14 is basic

But pH= - log [H^+]
pOH = -log [OH^-]
Then;
pH + pOH = 14
Hence;
pH = 14 - pOH

a. [H+] = 6.0 x 10-10M
pH= 9.22 is basic
b. [OH-] = 30 × 10-2M
pH = 13.5 is basic
C. IH+1 = 20× 10-7M
pH = 0.56 is acidic
d. [OH-] = 1.0 x 10-7M
pH = 7 is neutral
Answer: a. basic
b. basic
c. acidic
d. neutral

Explanation: Acids and bases can be classified
Chemistry
Step-by-step answer
P Answered by PhD
Answer: 306 L
Explanation: Using the ideal gas law,
PV = nRT
where R = 0.08206 L•atm/(mol•°K), solving for n gives
n = PV/(RT)
n = (845 mmHg) (270 L) / ((0.08206 L•atm/(mol•°K)) (24 °C))

Convert the given temperature to °K and the given pressure to atm:
24 °C = (273.15 + 24) °K ≈ 297.2 °K
(845 mmHg) × (1/760 atm/mmHg) ≈ 1.11 atm

Then the balloon contains
n = (1.11 atm) (270 L) / ((0.08206 L•atm/(mol•°K)) (297.2 °K))
n ≈ 12.3 mol
of He.

Solve the same equation for V :
V = nRT/P

Convert the target temperature to °K:
-50 °C = (273.15 - 50) °K = 223.15 °K

Then the volume under the new set of conditions is
V = (12.3 mol) (0.08206 L•atm/(mol•°K)) (223.15 °K) / (0.735 atm)
V ≈ 306 L

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