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3 years ago

What is the standard heat of reaction for the following reaction?

Chemistry

1 answer:

8090 [49]3 years ago

5 0

Answer:

The correct answer to the question is

The standard heat of reaction for the reaction is

a. 216.8 kJ released per mole

Explanation:

The heat of reaction is given by [Heat of formation of products] - [Heat of formation of reactants]

In the question we have, heat of formation of the products Zn+2 (aq) = -152.4 kJ/mole and the heat of formation of the reactants = 64.4 kJ/mole

Therefore, the heat of formation of the reaction = (-152-64.4) kJ/mole or

-216.8 kJ/mole released

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Assuming that gasoline is 100% isooctane, that isooctane burns to produce only CO2CO2 and H2OH2O, and that the density of isooct

Aleksandr [31]

Answer:

1.12×10¹¹ kg of CO₂ are produced with 4.6×10¹⁰ L of isooctane

Explanation:

Let's state the combustion reaction:

C₈H₁₈ + 25/2O₂ → 8CO₂ + 9H₂O

Let's calculate the mass of isooctane that reacts.

Density = Mass / Volume

Density . Volume = Mass

First of all, let's convert the volume in L to mL, so we can use density.

4.6×10¹⁰ L . 1000 mL / 1L = 4.6×10¹³ mL

0.792 g/mL . 4.6×10¹³ mL = 3.64 ×10¹³ g

This mass of isooctane reacts to produce CO₂ and water, so let's determine the moles of reaction

3.64 ×10¹³ g . 1mol / 114 g = 3.19×10¹¹ mol

Ratio is 1:8 so 1 mol of isooctane can produce 8 moles of dioxide

Therefore 3.19×10¹¹ mol would produce (3.19×10¹¹ mol . 8) = 2.55×10¹² moles of CO₂

Now, we can determine the mass of produced CO₂ by multipling:

moles . molar mass

2.55×10¹² mol . 44 g/mol = 1.12×10¹⁴ g of CO₂

If we convert to kg 1.12×10¹⁴ g / 1000 = 1.12×10¹¹ kg

6 0

3 years ago

The molar solubility of C a ( O H ) 2 C a ( O H ) 2 was experimentally determined to be 0.019 M. Based on this value, what is th

Anuta_ua [19.1K]

Answer:

Ksp = 2.74 x 10⁻⁵

Explanation:

The solubility equilibrium for Ca(OH)₂ is the following:

Ca(OH)₂(s) ⇄ Ca²⁺(aq) + 2 OH⁻(aq)

I 0 0

C + s + 2s

E s 2s

According to the ICE table, the expression for the solubility product constant (Kps) is:

Ksp = [Ca²⁺] x ([OH⁻])² = s x (2s)² = 4s³

Then, we calculate Ksp from the solubility value (s):

s = 0.019 M

⇒ Ksp = 4s³ = 4 x (0.019)³ = 2.74 x 10⁻⁵

8 0

3 years ago

Most chemical reactions take place in labs true or false

arsen [322]

The answer would most likely be False

7 0

3 years ago

Read 2 more answers

What is the solution to the problem expressed to the correct number of significant figures?

anyanavicka [17]

Answer:

8700

Explanation:

First, do the operations inside parentheses.

102 900/12 = 8600 2 sfs because of 12

170/1.27 = 130 2 sfs because of trailing 0 in 170

===============

Now, do the addition.

8600

+ 130

8700

The answer has two significant figures because when adding, you must round your answer to the same "place" as the measurement with its last significant figure furthest to the left.

The last significant figure in 8600 (the 6, in the hundreds place) is further to the left than the last significant figure in 130 (the 3, in the tens place).

We round off to the nearest hundred and get the answer, 8700.

6 0

3 years ago

What is the concentration in molarity of S2O32- (aq) in a solution prepared by mixing 150 mLmL of 0.149 MM Na2S2O3 (aq) with eno

Artist 52 [7]

Answer:

0.0890 M

Explanation:

Since the concentration of KCl is irrelevant in this case, the concentration of Na2S2O3 can be determined using a simple dilution equation:

C1V1 = C2V2, where C1 = 0.149 M, V1 = 150 mL, V2 = 250 mL

C2 = 0.149 x 150/250

= 0.089 M

To determine the concentration of S2O32- (aq), consider the equation:

$Na_2S_2O_3 => 2Na^+_{(aq)} + S_2O^2^-_3_{(aq)}$

The concentration of Na2S2O3 and S2O32- (aq) is 1:1

Hence, the concentration in molarity of S2O32- (aq) is 0.089 M.

To 3 significant figures = 0.0890 M

7 0

3 years ago