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3 years ago

If 17.8 grams of KOH dissolve in enough water to make a 198-gram solution, what is the concentration in percent by mass?

Chemistry

1 answer:

sleet_krkn [62]3 years ago

7 0

Solute of solution = 17.8 g

Solvn = 198 g

% = 17.8 / 198

w% = 0.089 x 100 = 8.9% by mass

hope this helps!

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How many liters of solution will contain 1.5 moles of CaCl2 if the solution is 6.0 M CaCl2?

sashaice [31]

Answer:

0.25

Explanation:

volume= number of moles over concentration

hence v=1.5/6

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3 years ago

When 55.0 grams of metal at 75.0°C is added to 100. grams of water at 15.0°C, the temperature of the water rises to 18.7°C. Assu

olga2289 [7]

Answer:

The specific heat of the metal is 0,50 J/gºC

Explanation:

Assume that no heat is lost to the surroundings

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Let's replace our values.

55g . C . (18,7ºC - 75ºC) + 100g . 4,184 J/g·°C . (18,7ºC - 15ºC) = 0

55g . C . -56,3 ºC + 418,4J/·°C . 3,7ºC = 0

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3 years ago

A 0.100 mile sample of gas is at a temperature of 85.0 degrees C and a volume of 3.47 L. What is the pressure of the gas( in mm

vladimir1956 [14]

Answer: 64.6 mmHg

Explanation:

Given that:

Volume of gas V = 3.47L

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Convert Celsius to Kelvin

(85.0°C + 273 = 358K)

Pressure P = ?

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Note that Molar gas constant R is a constant with a value of 0.0082 ATM dm3 K-1 mol-1

Then, apply ideal gas equation

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p x 3.47dm3 = 0.10 x (0.0082 atm dm3 K-1 mol-1 x 358K)

p x 3.47dm3 = 0.29 atm dm3

p = (0.29 atm dm3 / 3.47 dm3)

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If 1 atm = 760 mm Hg

0.085atm = 0.085 x 760

= 64.6 mm Hg

Thus, the pressure of the gas is 64.6 mm hg

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2 years ago

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