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Sauron [17]
2 years ago
6

a solution k is saturated at 33 g solute in 100g solvent if a 50g solute is added to 200g solvent solution k is​

Chemistry
1 answer:
Alenkinab [10]2 years ago
3 0

Answer:

33 100gc50 is a 100

Explanation:

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Liquid Q is a polar solvent and liquid R is a nonpolar solvent. On the basis of this information, you would expect:
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Can metals have covalent radius and van der Waal's radius instead of metallic radius?​
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3 years ago
The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1580 L of nitrogen gas and 351
ikadub [295]

Answer : The volume of reactant measured at STP left over is 409.9 L

Explanation :

First we have to calculate the moles of N_2 and H_2 by using ideal gas equation.

<u>For N_2 :</u>

PV_{N_2}=n_{N_2}RT

where,

P = Pressure of gas at STP = 1 atm

V = Volume of N_2 gas = 1580 L

n = number of moles N_2 = ?

R = Gas constant = 0.0821L.atm/mol.K

T = Temperature of gas at STP = 273 K

Putting values in above equation, we get:

1atm\times 1580L=n_{N_2}\times (0.0821L.atm/mol.K)\times 273K

n_{N_2}=70.49mole

<u>For H_2 :</u>

PV_{H_2}=n_{H_2}RT

where,

P = Pressure of gas at STP = 1 atm

V = Volume of H_2 gas = 3510 L

n = number of moles H_2 = ?

R = Gas constant = 0.0821L.atm/mol.K

T = Temperature of gas at STP = 273 K

Putting values in above equation, we get:

1atm\times 3510L=n_{H_2}\times (0.0821L.atm/mol.K)\times 273K

n_{H_2}=156.6mole

Now we have to calculate the limiting and excess reagent.

The balanced chemical reaction is,

N_2(g)+3H_2(g)\rightarrow 2NH_3(g)

From the balanced reaction we conclude that

As, 3 mole of H_2 react with 1 mole of N_2

So, 156.6 moles of H_2 react with \frac{156.6}{3}\times 1=52.2 moles of N_2

From this we conclude that, N_2 is an excess reagent because the given moles are greater than the required moles and H_2 is a limiting reagent and it limits the formation of product.

Now we have to calculate the excess moles of N_2 reactant (unreacted gas).

Excess moles of N_2 reactant = 70.49 - 52.2 = 18.29 moles

Now we have to calculate the volume of reactant, measured at STP, is left over.

PV=nRT

where,

P = Pressure of gas at STP = 1 atm

V = Volume of gas = ?

n = number of moles of unreacted gas = 18.29 moles

R = Gas constant = 0.0821L.atm/mol.K

T = Temperature of gas at STP = 273 K

Putting values in above equation, we get:

1atm\times V=18.29mole\times (0.0821L.atm/mol.K)\times 273K

V=409.9L

Therefore, the volume of reactant measured at STP left over is 409.9 L

8 0
2 years ago
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