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3 years ago

How many grams of sodium nitrate are needed to make 2.50L of 1.12m solution

Chemistry

1 answer:

Roman55 [17]3 years ago

7 0

Answer: 238 g of sodium nitrate are needed to make 2.50L of 1.12m solution

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.

$Molarity=\frac{n}{V_s}$

where,

n = moles of solute

$V_s$ = volume of solution in L

Now put all the given values in the formula of molality, we get

$1.12=\frac{\text {moles of}NaNO_3}{2.50}$

moles of $NaNO_3$ = 2.8

moles of $NaNO_3=\frac{\text {given mass}}{\text {Molar mass}}$

$2.8mol=\frac{xg}{85g/mol}$

$x=238g$

Thus 238 g of sodium nitrate are needed to make 2.50L of 1.12m solution 

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Answer:

The density of the metal is 0.561 g/mL

Explanation:

The computation of the density of the metal is shown below;

As we know that

The Density of the metal is

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3 years ago

How much thermal energy is added to 10.0 g of ice at −20.0°C to convert it to water vapor at 120.0°C?

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Answer:

7479 cal.

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Explanation:

This is a calorimetry problem where water in its three states changes from ice to vapor.

We must use, the calorimetry formula and the formula for latent heat.

Q = m . C . ΔT

Q = Clat . m

First of all, let's determine the heat for ice, before it melts.

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Now, the ice has melted.

Q = Clat heat of fusion . 10 g

Q = 79.7 cal/g . 10 g → 797 cal

We have water at 0°, so this water has to receive heat until it becomes vapor. Let's determine that heat.

Q = m . C . ΔT

Q = 10 g . 1 cal/g°C (100°C - 0°C) → 1000 cal

Water is ready now, to become vapor so let's determine the heat.

Q = Clat heat of vaporization . m

Q = 539.4 cal/g . 10 g → 5394 cal

Finally we have vapor water, so let's determine the heat gained when this vapor changes the T° from 100°C to 120°

Q = m . C . ΔT

Q = 10 g . 0.470 cal/g°C . (120°C - 100°C) → 94 cal

Now, we have to sum all the heat that was added in all the process.

100 cal + 797 cal + 1000 cal + 5394 cal + 94 cal =7479 cal.

We can convert this unit to joules, which is more acceptable for energy terms.

1 cal is 4.18 Joules.

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3 years ago

Calculate the de broglie wavelength of a subatomic particle that is moving at 351 km/s if its mass is 9.11 Ã 10â31 kg. Î» = hmuh

gregori [183]

The de Broglie wavelength of a subatomic particle is 2.09 nm.

λ = h m v = h

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Frequency is the ratio of velocity and wavelength in relation to hurry. In evaluation, wavelength refers back to the ratio of velocity and frequency.

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de Broglie wavelength λ = h/mv

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Learn more about de Broglie wavelength here:-brainly.com/question/16595523

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2 years ago

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iogann1982 [59]

Answer:

the concentration of PCl5 in the equilibrium mixture = 296.20M

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The detaied steps is as shown in the attached file.

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3 years ago

Solid sodium hydrogen carbonate, NaHCO3, decomposes on heating according to the equation:

tekilochka [14]

Answer:

See explanation

Explanation:

First, let's write the balanced equation again:

2 NaHCO3(s) <-> Na2CO3(s) + H2O(g) + CO2(g)

Now, we know that the total pressure was 7.76 atm. This total pressure, is the sum of the pressure of water and CO2 like this:

Ptotal = Pwat + PCO2 (1)

This is the dalton's law for partial pressures.

The pressure can be also be relationed with the moles

Ratio of mole = Ratio of pressure

so, taking this in consideration we can say the following:

Pwater/PCO2 = moles water / moles CO2

As the only components exerting pressure are CO2 and Water (Because they are in gas phase), the total pressure can be splitted between the two of them so:

Pwater = Ptotal/2

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With this pressure, and using the ideal gas equation, we can know the moles of water:

PV = nRT

n = PV/RT using R = 0.082 L atm / K mol

n = 3.88 * 5 / 0.082 * (160+273)

n = 0.546 moles of water

b) now that we have the moles of water, we can actually know the moles that reacted originally from the sodium carbonate by stechiometry.

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the moles of NaHCO3 initially:

n = 100 / 84

n = 1.19 moles

so, If 1.19 moles of NaHCO3 reacted, and only produces 0.546 moles of water and CO2, then, the remaining moles of NaHCO3 is:

remaining moles = 1.19 - 0.546 = 0.644 moles

therefore the mass remaining:

mCO2 = 0.644 * 84

mCO2 = 54.096 g

c) As it was stated before, only the gaseous components are involved in the pressure, thus, in the kp expression which is:

Kp = Pwater * PCO2

Kp = 3.88 * 3.88

Kp = 15.0544

d) As the total pressure is 7.76 atm and the fact that NaHCO3 is solid, this component is not exerting any pressure in the reaction, as seen in the Kp expression, so it won't matter that if we raise a little the quantity of the reactant, it still has some remaining.

3 0

3 years ago

How many grams of sodium nitrate are needed to make 2.50L of 1.12m solution ​

How many grams of sodium nitrate are needed to make 2.50L of 1.12m solution