Find the number of formula units in 30 moles of h3po4

The reactants of two chemical equations are listed.

Oksi-84 [34.3K]

Answer:

Equation 2, because K being more reactive, exchanges position with Pb in PbNO3.

Explanation:

3 0

3 years ago

Can the structure of an atom similar to our solar system?

nika2105 [10]

<span>its because they're both structured the same way. for example the sun and the nucleus are the same (in the centre) and the electrons and planets orbiting are the same</span>

3 0

3 years ago

What mass of water could be warmed from 21.4 degrees celsius to 43.4 degrees celsius by the pellet dropped inside it? Heat capac

Artist 52 [7]

42.34 g of water could be warmed from 21.4°C to 43.4°C by the pellet dropped inside it

Heat loss by the pellet is equal to the Heat gained by the water.

$q_{w} = -q_{p}$ ….(1)

where, $q_{w}$ is the heat gained by water

$q_{p}$ is the heat loss by pellet

$q_{w}$ = mCΔT

where m = mass of water

C = specific heat capacity of water = 4.184 J/g-°C

ΔT = Increase in temperature

ΔT for water = 43.4 - 21.4 = 22°C

$q_{w}$ = m × 4.184 × 22 …. (2)

Now

$q_{p}$ = $H_{c}$ ×ΔT

where $H_{c}$ = Heat capacity of pellet = 56J/°C

Δ T for pellet = 43.4 - 113 =- 69.6°C

$q_{p}$ = 56 × -69.6 = -3897.6 J

From equation (1) and (2)

-m× 4.184 × 22 =-3897.6

m= 42.34 g

Hence, 42.34 g of water could be warmed from 21.4 degrees Celsius to 43.4 degrees Celsius by the pellet dropped inside it.

Learn more about specific heat here brainly.com/question/16559442

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6 0

2 years ago

If you burn 6 moles of Hydrogen gas how much heat is generated?<br> 2H2 + O2 → 2H20+286 kJ

likoan [24]

Answer:

858 kJ

Explanation:

3 0

3 years ago

When 78.6 g of urea CH4N2O are dissolved in 700. g of a certain mystery liquid X, the freezing point of the solution is 4.9 Â°C

iogann1982 [59]

Answer:

The van't Hoff factor of NaCl in liquid X is 1.69

Explanation:

Step 1: Data given

Mass of urea = 78.6 grams

Molar mass of urea = 60.06 g/mol

Mass of liquid X = 700 grams = 0.700 kg

he freezing point of the solution is 4.9°C lower than the freezing point of pure X

When 78.6 g of sodium chloride are dissolved in the same mass of X, the freezing point of the solution is 8.5°C lower than the freezing point of pure X.

Molar mass of NaCl = 58.44 g/mol

Step 2: Calculate moles

Moles urea = mass / molar mass

Moles urea = 78.6 grams / 60.06 g/mol

Moles urea = 1.31 moles

Moles NaCl = 78.9 grams / 58.44 g/mol

Moles NaCl = 1.35 moles

Step 3: Calculate molality

Molality = moles / mass of liquid

Molality urea = 1.31 moles / 0.700 kg

Molality = 1.87 molal

Molality NaCl = 1.35 moles / 0.700 kg

Molality NaCl = 1.92 molal

Step 4: Calculate the freezing point depression constant of X

ΔT = i*Kf*m

⇒with ΔT = the freezing point depression = 4.9 °C

⇒with i = the van't hoff factor of urea = 1

⇒with Kf =the freezing point depression consant of X = TO BE DETERMINED

⇒with m = the molality of urea solution = 1.87 molal

4.9 °C = 1 * Kf * 1.87 molal

Kf == 4.9 / 1.87

Kf = 2.62 °C/m

Step 5: Calculate the van't Hoff facotr of NaCl in X

ΔT = i*Kf*m

⇒with ΔT = the freezing point depression = 8.5 °C

⇒with i = the van't hoff factor of urea = TO BE DETERMINED

⇒with Kf =the freezing point depression consant of X = 2.62 °C/m

⇒with m = the molality of urea solution = 1.92 molal

8.5 °C = i * 2.62 °C/m * 1.92 m

i = 8.5 / (2.62 * 1.92)

i = 1.69

The van't Hoff factor of NaCl in liquid X is 1.69

5 0

3 years ago