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shepuryov [24]
3 years ago
11

PLZZZZZ HELP MEEEEEE

Chemistry
1 answer:
Masja [62]3 years ago
4 0

Answer:

0.0745 mole of hydrogen gas

Explanation:

Given parameters:

Number of H₂SO₄ = 0.0745 moles

Number of moles of Li = 1.5107 moles

Unknown:

Number of moles of H₂ produced = ?

Solution:

To solve this problem, we have to work from the known specie to the unknown one.

The known specie in this expression is the sulfuric acid,  H₂SO₄. We can compare its number of moles with that of the unknown using a balanced chemical equation.

   Balanced chemical equation:

                    2Li   +     H₂SO₄   →   Li₂SO₄   +   H₂

 From the balanced equation;

     

Before proceeding, we need to obtain the limiting reagent. This is the reagent whose given proportion is in short supply. It determines the extent of the reaction.

           2 mole of Li reacted with 1 mole of  H₂SO₄

          1.5107 mole of lithium will react with \frac{1.5107}{2}  = 0.7554mole of H₂SO₄

But we were given 0.0745 moles,

This suggests that the limiting reagent is the sulfuric acid because it is in short supply;

   

   since 1 mole of sulfuric acid produced 1 mole of hydrogen gas;

    0.0745 mole of sulfuric acid will produce 0.0745 mole of hydrogen gas

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What volume of solution gives the desired moles?
motikmotik

Answer:

1. 0.073L

2. 0.028L

3. 0.014L

Explanation:

The volume for the different solutions are obtained as shown below:

1. Mole = 0.53mol

Molarity = 7.25M

Volume =?

Molarity = mole /Volume

Volume = mole /Molarity

Volume = 0.53/7.25

Volume = 0.073L

2. 0.035mol from a 1.25M

Mole = 0. 035mol

Molarity = 1.25M

Volume =?

Molarity = mole /Volume

Volume = mole /Molarity

Volume = 0.035/1.25

Volume = 0.028L

3. Mole = 0.0013mol

Molarity = 0.090M

Volume =?

Molarity = mole /Volume

Volume = mole /Molarity

Volume = 0.0013/0.090

Volume = 0.014L

8 0
3 years ago
Help me with 1 and 2
vladimir1956 [14]
B and c are the correct answers
6 0
3 years ago
Read 2 more answers
Calculate the pH of mixing 24 mL of 1M acetic acid with 76 mL of 1M sodium acetate. For the purpose of this calculation, assume
FromTheMoon [43]

Answer:

pH = 5.24

Explanation:

Mixture of acetic acid with acetate ion is a buffer (Mixture of a weak acid with its conjugate base). The pH of a buffer can be determined using Henderson-Hasselbalch equation:

pH = pKa + log₁₀ [A⁻] / [HA]

<em>Where pKa is -log Ka = 4.74; [A⁻] is the concentration of conjugate base (Acetate ion) and [HA] is molar concentration of the weak acid.</em>

Concentration of the acetic acid in the 100mL≡0.1L (76mL + 24mL) solution is:

[HA] = 0.024L ₓ (1mol / L) / 0.1L = 0.24M

[A⁻] = 0.076L ₓ (1mol / L) / 0.1L = 0.76M

Replacing in H-H equation:

pH = 4.74 + log₁₀ [0.76M] / [0.24M]

<h3>pH = 5.24</h3>

<em />

7 0
3 years ago
Calculate the volume of 5.0 grams of NO gas at STP.
Sveta_85 [38]

Answer:

The volume of  5.0 g CO  2  is  2.6 L CO  2  at STP

Explanation:

STP

STP is currently  

0

∘

C

or  

273.15 K

, which are equal, though the Kelvin temperature scale is used for gas laws; and pressure is  

10

5

.

Pascals (Pa)

, but most people use  

100 kPa

, which is equal to  

10

5

.

Pa

.

You will use the ideal gas law to answer this question. Its formula is:

P

V

=

n

R

T

,

where  

P

is pressure,  

V

is volume,  

n

is moles,  

R

is a gas constant, and  

T

is temperature in Kelvins.

Determine moles

You may have noticed that the equation requires moles  

(

n

)

, but you have been given the mass of  

CO

2

. To determine moles, you multiply the given mass by the inverse of the molar mass of  

CO

2

, which is  

44.009 g/mol

.

5.0

g CO

2

×

1

mol CO

2

44.009

g CO

2

=

0.1136 mol CO

2

Organize your data

.

Given/Known

P

=

100 kPa

n

=

0.1136 mol

R

=

8.3145 L kPa K

−

1

mol

−

1

https://en.wikipedia.org/wiki/Gas_constant

T

=

273.15 K

Unknown:  

V

Solve for volume using the ideal gas law.

Rearrange the formula to isolate  

V

. Insert your data into the equation and solve.

V

=

n

R

T

P

V

=

0.1136

mol

×

8.3145

.

L

kPa

K

−

1

mol

−

1

×

273.15

K

100

kPa

=

2.6 L CO

2

rounded to two significant figures due to  

5.0 g

Answer link

Doc048

May 18, 2017

I got 2.55 Liters

Explanation:

1 mole of any gas at STP = 22.4 Liters

5

g

C

O

2

(

g

)

=

5

g

44

(

g

mole

)

=

0.114

mole

C

O

2

(

g

)

Volume of 0.114 mole  

C

O

2

(

g

)

= (0.114 mole)(22.4 L/mole) = 2.55 Liters  

C

O

2

(g) at STP

6 0
3 years ago
Which of the following is not an example of a chemical change?
tensa zangetsu [6.8K]
The correct answer is cutting paper because it is an example of a physical change. A physical change is a change a change in the properties of matter that does not change the identity of the substance. On the other hand, chemical change is a change where the substance changes in identity after undergoing a process..
4 0
3 years ago
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