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3 years ago

Diluting sulfuric acid with water is highly exothermic:

Chemistry

1 answer:

elena-14-01-66 [18.8K]3 years ago

8 0

Answer:

The correct answer is 51.2 degree C.

Explanation:

The standard enthalpy for H₂SO₄ (l) is -814 kJ/mole and the standard enthalpy for H₂SO₄ (aq) is -909.3 kJ/mole.

Now the dHreaction = dHf (product) - dHf (reactant)

= -909.3 - (-814)

dHreaction or q = -95.3 kJ of energy will be used for dissociating one mole of H₂SO₄.

The heat change in calorimetry can be determined by using the formula,

q = mass * specific heat capacity * change in temperature -----------(i)

Based on the given information, the density of H₂SO₄ is 1.060 g/ml

The volume of H₂SO₄ is 1 Liter

Therefore, the mass of H₂SO₄ will be, density/Volume = 1.060 g/ml / 1 × 10⁻³ ml = 1060 grams

The initial temperature given is 25.2 degrees C, or 273+25.2 = 298.2 K, let us consider the final temperature to be T₂.

ΔT = T₂ -T₁ = T₂ - 298.2 K

Now putting the values in equation (i) we get,

95.3 kJ = 1060 grams × 3.458 j/gK (T₂ - 298.2 K) (the specific heat capacity of the final solution is 3.458 J/gK)

(T₂ - 298.2 K) = 95300 J / 1060 × 3.458 = 26 K

T₂ = 298.2 K + 26 K

T₂ = 324.2 K or 324.2 - 273 = 51.2 degree C.

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consider the reaction of hydrogen and oxygen producing water. If 24.6 g of water is produced and 2.9 g of hydrogen is used, how

Maurinko [17]

Considering the reaction of hydrogen and oxygen to produce water. If 24.6 g of water is produced and 2.9 g of hydrogen is used, the amount of oxygen needed is 21.87 grams

The best way to solve this question is to write out the reaction between hydrogen and oxygen that resulted in the formation of water.

So, we have:

$\mathbf{ 2 H_2{(g)} + O_2{(g)} \to 2H_2O_{(l)}}$

From the above reaction;

2 moles of hydrogen gas reacted with 1 mole of oxygen to produce 2 moles of water.

If;

1 mole of O₂ = 32 grams of O₂
2 mole of H₂O = 2 × 18 grams of H₂O
2 mole of H₂O = 36 grams of H₂O

We can deduce that since 1 mole of O₂ produced 2 moles of H₂O;

Thus, 32 grams of O₂ is needed to produce 36 grams of H₂O.

∴

To produce, 24.6 grams of H₂O, we have:

$\mathbf{=\Big(\dfrac{32 \times 24.6 }{36}\Big) grams }$

= 21.87 grams of oxygen.

Therefore, we can conclude that the amount of oxygen needed is 21.87 grams.

Learn more about chemical reactions here:

brainly.com/question/1689737?referrer=searchResults

5 0

3 years ago

Define the term molecule?

professor190 [17]

Answer:

A termolecular reaction requires the collision of three particles at the same place and time.

Explanation:

This type of reaction is very uncommon because all three reactants must simultaneously collide with each other, with sufficient energy and correct orientation, to produce a reaction.

7 0

3 years ago

At a given temperature, 4.06 atm of H2 and 3.5 atm of Cl2 are mixed and allowed to come to equilibrium. The equilibrium pressure

Llana [10]

Answer: The value of $K_p$ for the given chemical reaction is 0.1415

Explanation:

Equilibrium constant in terms of partial pressure is defined as the ratio of partial pressures of the products and the reactants each raised to the power their stoichiometric ratios. It is expressed as $K_p$

For a general chemical reaction:

$aA+bB\rightarrow cC+dD$

The expression for $K_p$ is written as:

$K_p=\frac{p_{C}^cp_{D}^d}{p_{A}^ap_{B}^b}$

For the given chemical equation:

$H_2(g)+Cl_2(g)\rightleftharpoons 2HCl(g)$

The expression for $K_p$ for the following equation is:

$K_p=\frac{(p_{HCl})^2}{(p_{H_2)}(p_{Cl_2})}$

We are given:

$p_{HCl}=1.418atm\\p_{H_2}=4.06atm\\p_{Cl_2}=3.5atm$

Putting values in above equation, we get:

$K_p=\frac{(1.418)^2}{(4.06)\times (3.5)}\\\\K_p=0.1415$

The value of $K_p$ for the given chemical reaction is 0.1415

5 0

3 years ago

2. How many moles of hydrogen atoms are there in 154 mL of 0.18 M H2SO4? Write your

katrin [286]

2. 0.05544 moles of hydrogen atom are present in 154 mL 0.18 M solution of H2SO4.

3. 15.2506 heat in Joules is absorbed by 150.0 mL of pure water that is heated from 21.2°C to 45.5°C.

4. 0.75 M is the concentration of Na+ ions in 25.0 mL of 1.50 M NaOH is reacted with 25.0 mL of 1.50 M HCI

Explanation:

Number of moles of H2SO4 can be calculated by the given volume and molarity from the formula:

molarity = $\frac{number of moles}{volume of teh solution}$

number of moles = molarity × volume of the solution of H2SO4

number of moles = 0.18 × 0.154 litres

= 0.02772 moles of H2SO4.

Since 1 mole of H2SO4 contains 2 moles of hydrogen

so, 0.02772 moles of H2SO4 will have x moles

$\frac{1}{2}$ = $\frac{0.0272}{x}$

2 × 0.02772 = x

0.05544 moles of hydrogen atom are present in 154 mL 0.18 M solution of H2SO4.

3. The heat absorbed is calculated from the formula:

ΔH = cp × m × ΔT ( ΔT = change in temperature in Kelvin, m in kg, cp= specific heat of water)

putting the values in formula:

ΔH = 4.184 × 0.15 × ( 318.65-294.35)

= 4.184 × 0.15× 24.3

= 15.2506 Joules of heat is absorbed.

4. The concentration of Na+ ions

the balanced equation is

NaOH + HCl⇒ NaCl + H20

from one mole of NaCl 1 mole of NaCl i.e one 1 mole of Na+ ions is formed.

number of moles of NaOH is calculated by the formula:

Molarity = $\frac{number of moles}{volume of the solution}$

number of moles = 0.025L × 1.50M

= 0.0375 moles of NaOH

so 1 mole of NaOH produces 1 mole of Na= ions

hence, 0.0375 moles produces x moles of Na+ ions

$\frac{1}{1}$ = $\frac{0.0375}{x}$

moles of Na+ is produced.

concentration of NaOH in 50 ml solution because NaOH and HCl of 25 ml reacted.

applying the molarity formula from above

Molarity = $\frac{0.0375}{0.05}$

= 0.75 M

6 0

3 years ago

Consider reaction AgCIO3(aq)+Mgl2(aq)

mash [69]

Answer:

the product is Mg(Clo3)2 + AgI

6 0

3 years ago