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3 years ago

4HCI + O2 =2H20 + Cl2

Chemistry

1 answer:

Sergio039 [100]3 years ago

6 0

The rate of the backward reaction increases

Explanation:

It is evident that if the reaction is left to proceed spontaneously, the forward reaction is favored because it results in a decrease in pressure in the system (The total reactants have 5 moles and the products have 3 in total).

Increasing H₂O concentration is then reaction, therefore, stymies the forward reaction and favors the reserves reaction. This is because the reverse reaction will lead to reduced pressure.

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A gaseous mixture consisting of nitrogen, argon, and oxygen is in a 3.5-L vessel at 25C. Determine the number of moles of oxygen

Step2247 [10]

Answer:

Number of moles of oxygen = 0.037 mol

Explanation:

Given data:

Total pressure = 98.5 KPa

Partial pressure of nitrogen = 22.0 KPa

Partial pressure of argon = 50.0 KPa

Volume = 3.5 L

Temperature = 25°C (25+273= 298K)

Number of moles of oxygen = ?

Solution:

Total pressure = P(N₂) + P(O₂) + P(Ar)

98.5 KPa = 22.0 KPa +P(O₂) + 50.0 KPa

98.5 KPa = 72.0 KPa +P(O₂)

P(O₂) = 98.5 KPa - 72.0 KPa

P(O₂) = 26.5 KPa

KPa to atm:

26.5 KPa/ 101 = 0.262 atm

Number of moles of oxygen:

PV = nRT

n = PV/RT

n = 0.262 atm × 3.5 L / 0.0821 atm.L/mol.K × 298 K

n = 0.917atm.L /24.47atm.L/ mol

n = 0.037 mol

6 0

3 years ago

Which of these lab safety procedures is INCORRECT?

Ksju [112]

Answer:

Explanation:

D is not necessary to follow lab safety in Laboratory

6 0

3 years ago

How many milliliters of gasoline have a mass of 2.4 kg ( D=0.74g/mL )?

lana66690 [7]

Transform the g into kg by multiplying 0.74 by 10^-3. then divide 2.4 kg by the density

7 0

2 years ago

Read 2 more answers

Witch is an example of a voltaic cell?

Alex777 [14]

A battery is an example of a voltaic cell that is used daily.

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3 years ago

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr. Determine the pH of the solution after the addition of 300.0 mL

Vera_Pavlovna [14]

Answer : The correct option is, (C) 1.7

Explanation :

First we have to calculate the moles of $Ca(OH)_2$ and $HBr$ .

$\text{Moles of }Ca(OH)_2=\text{Concentration of }Ca(OH)_2\times \text{Volume of solution}=0.10M\times 0.1L=0.01mole$

$\text{Moles of }HBr=\text{Concentration of }HBr\times \text{Volume of solution}=0.10M\times 0.3L=0.03mole$

The balanced chemical reaction will be:

$Ca(OH)_2+2HBr\rightleftharpoons CaBr_2+2H_2O$

0.01 mole of $Ca(OH)_2$ dissociate to give 0.01 mole of $Ca^{2+}$ ion and 0.02 mole of $OH^-$ ion

and

0.03 mole of $HBr$ dissociate to give 0.03 mole of $H^+$ ion and 0.03 mole of $Br^-$ ion

That means,

0.02 moles of $OH^-$ ion neutralize by 0.02 moles of $H^+$ ion.

The excess moles of $H^+$ ion = 0.03 - 0.02 = 0.01 mole

Total volume of solution = 100 + 300 = 400 ml = 0.4 L

Now we have to calculate the concentration of $H^+$ ion.

$\text{Concentration of }H^+=\frac{\text{Moles of }H^+}{\text{Total volume}}$

$\text{Concentration of }H^+=\frac{0.01mole}{0.4L}=0.025M$

Now we have to calculate the pH of the solution.

$pH=-\log [H^+]$

$pH=-\log (0.025M)$

$pH=1.7$

Therefore, the pH of the solution is, 1.7

5 0

3 years ago