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balu736 [363]
3 years ago
13

1.00 M aqueous solution of NaOH, a 0.50 M aqueous solution of H2SO4 and a coffee cup calorimeter were allowed to stand at a room

temperature of 25.4 C until the tempurature of all three reached 25.4 C. A 50.0-mL sample of the 1.00 M NaOH was then placed in the calorimeter. 50.0 mL if the 0.50 M H2SO4 was added as rapidly as possible and the two solutions were mixed thrououghly, the temperature rose to 31.9 C. What is the heat of neutralizaion in kJ for one mole of sulfuric acid? Assume that the densities of the NaOH and the H2SO4 solutions are both 1.00 g/mL, and that the specific heat of the solution after reaction is 4.18 J/g-oC.
Chemistry
2 answers:
Kay [80]3 years ago
6 0

Answer:

-108.7 kJ / mol H₂SO₄

Explanation:

The reaction of NaOH with H₂SO₄ is:

2 NaOH + H₂SO₄ → 2H₂O + 2NaSO₄

<em>2 Moles of NaOH reacts per mole of H₂SO₄</em>

This reaction, as all acid-base reactions, produce heat. Moles of NaOH and H₂SO₄ reacting are:

0.0500L × (1.00mol NaOH / L) = 0.0500 moles NaOH

0.0500L × (0.50mol H₂O₄ / L) = 0.0250 moles H₂SO₄

Coffer cup calorimeter formula is:

Q = -C×m×ΔT

<em>Where Q is heat, C is specific heat of solution (4.18J/g°C), m is mass of solution (50g NaOH + 50g H₂SO₄ = 100g of solution -Assuming densities of 1.00g/mL), and ΔT is temperature change (31.9°C-25.4°C = 6.5°C).</em>

Replacing:

Q = -4.18J/g°C × 100g × 6.5°C

Q = -2717J

This is the heat produced in neutralization reaction when 0.0250 moles H₂SO₄ react. Now, heat per mole of H₂SO₄ is:

-2717J / 0.0250 moles H₂SO₄

= -108680 J / mol H₂SO₄ ≡ -<em>108.7 kJ / mol H₂SO₄</em>

iragen [17]3 years ago
6 0

Answer:

ΔH = -108.7 kJ/mol

Explanation:

Step 1: Data given

Molarity of a NaOH solution = 1.00 M

Volume of NaOH = 50.0 mL = 0.050 L

Molarity of a H2SO4 solution = 0.50 M

Volume of H2SO4 = 50.0 mL = 0.050 L

Initial temperature of 25.4 °C

Final temperature = 31.9 °C

Density of NaOH and H2SO4 = 1.00 g/mL

Specific heat of the solution = 4.18 J/g°C

Step 2: The balanced equation

2NaOH + H2SO4 → Na2SO4 + 2H2O

Step 3: Calculate moles

Moles = molarity * volume

Moles NaOH = 1.00 M * 0.050 L

Moles NaOH = 0.050 moles

Moles H2SO4 = 0.50 M * 0.050 L

Moles H2SO4 = 0.0250 moles

Step 4: Calculate the mass

Mass of NaOH = 50 mL * 1g/mL = 50 grams

Mass of H2SO4 = 50 mL * 1g/mL = 50 grams

Step 5: Calculate heat trnasfer

Q = m*C*ΔT

⇒with Q = the heat transfer = TO BE DETERMINED

⇒with m = total mass of the solution = 50 g + 50 g = 100 grams

⇒with c= the specific heat of the solution = 4.18 J/g°C

⇒with ΔT = The change of temperature = T2 - T1 = 31.9 °C - 25.4 °C = 6.5 °C

Q = 100 g * 4.18 J/g°C * 6.5 °C

Q = 2717 J

Since this is an exothermic reaction ΔH is negative (-2717 J)

Step 6: calculate the heat of neutralizaion in kJ for one mole of sulfuric acid

ΔH = -2717 J / 0.0250 moles

ΔH = -108680 J/mol = -108.7kJ/mol

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Calculează masa zaharului si volumul apei necesare pentru prepararea 500g de soluție de zahăr cu partea de masa 20%
Sedbober [7]
T = 20 %  : 20 / 100 = 0.2

m1 = solute 

m2 = Solvent

T = m1 / m1 + m2

0.2 = 500 g / 500 g + m2

0.2 * ( 500 + m2 ) = 500

0.2 * 500 + 0.2 m2 = 500

100 + 0.2 m2 = 500

0.2 m2 = 500 - 100

0.2 m2 = 400

m2 = 400 / 0.2

m2 = 2000 g of water

hope this helps!



7 0
3 years ago
Which is an example of an endothermic reaction? A. combustion of fuels B. burning of wood C. cellular respiration D. photosynthe
kifflom [539]

D. photosynthesis is an endothermic reaction

8 0
3 years ago
Read 2 more answers
Ethylene produced by fermentation has a specific gravity of 0.787 at 25 degree Celsius. What is the volume of 125g of ethanol at
WITCHER [35]

<u>Answer:</u> The volume of given amount of ethanol at this temperature is 159.44 mL

<u>Explanation:</u>

Specific gravity is given by the formula:

\text{Specific gravity}=\frac{\text{Density of a substance}}{\text{Density of water}}

We are given:

Density of water = 0.997 g/mL

Specific gravity of ethanol = 0.787

Putting values in above equation, we get:

0.787=\frac{\text{Density of a substance}}{0.997g/mL}\\\\\text{Density of a substance}=(0.787\times 0.997g/mL)=0.784g/mL

Density is defined as the ratio of mass and volume of a substance.

\text{Density}=\frac{\text{Mass}}{\text{Volume}} ......(1)

Given values:

Mass of ethanol = 125 g

Density of ethanol = 0.784 g/mL

Putting values in equation 1, we get:

\text{Volume of ethanol}=\frac{125g}{0.784g/mL}=159.44mL

Hence, the volume of given amount of ethanol at this temperature is 159.44 mL

6 0
3 years ago
PLEASE HELP CHEMISTRY
eduard

When sodium carbonate is dissolved in water, the equation is Na_2CO_3 (s) --- > 2Na^+ (aq) + CO_3^{2-} (aq).

When carbon dioxide is placed in water, aqueous carbon dioxide is formed:  CO_2 (g) --- > CO_2(aq)

<h3>Dissolution of compounds in water</h3>

Some compounds are water-soluble, some are just partially soluble, while others are insoluble in water. Some soluble or partially soluble substances dissociate in water into their component ions. These substances are said to be ionic.

Sodium carbonate, like every other sodium salt, is soluble in water. It dissolves in water to form an aqueous solution of sodium carbonate.

While in solution, sodium carbonate dissociates into its component ions according to the following equation:

Na_2CO_3 (s) --- > 2Na^+ (aq) + CO_3^{2-} (aq)

Carbon dioxide, on the other hand, does not dissociate in water. Instead, it dissolves in water where most of it remains as aqueous carbon dioxide in equilibrium with a small amount of hydronium ion and hydrogen carbonate ion.

Since the hydronium and hydrogen carbonate ions formed are so minute, the equation of the reaction can be written as: CO_2 (g) --- > CO_2(aq)

More on the dissolution of substances can be found here: brainly.com/question/28580758

#SPJ1

7 0
1 year ago
What is the volume of 0.120 g of C2H2F4<br> vapor at 0.970 atm and 22.4°C?<br> Answer in units of L.
ludmilkaskok [199]

Answer:

V= 0.031L

Explanation:

P= 0.97atm, V= ?, n= 0.12/98 =0.00122mol, R= 0.082, T= 22.4+273= 295.4

Applying

PV=nRT

0.970×V = 0.00122×0.082×295.4

Simplify the above equation

V= 0.031L

6 0
3 years ago
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