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Sonbull [250]
3 years ago
11

Write the balanced chemical equation where liquid decane burns in oxygen gas to form carbon dioxide gas and water vapor. Use the

smallest whole number coefficients. Indicate the states of the reactants and products.
Chemistry
1 answer:
Allushta [10]3 years ago
3 0

Answer:

2C_{10} H_{22(l)} + 31O2(g)--> 20CO_{2(g)} + 22H_{2}O_{(g)}

Explanation:

2C_{10} H_{22(g)} + 31O2(g)--> 20CO_{2(g)} + 22H_{2}O_{(g)}

From the question, one can work out which states of matter to assign to which species. The trick with organic equations of this nature is to try to balance everything but oxygen first. Make sure you balance oxygen last because it is the easiest to balance.

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A solution contains 3.95 g of carbon disulfide (CS2, molar mass = 76.13 g/mol) and 2.43 g of acetone ((CH3)2CO, molar mass = 58.
Feliz [49]

Answer:

The solution is not ideal and shows a positive deviation from Raoult’s law since Psolution (experimental) > Psolution (actual).

Explanation:

Number of moles of CS2 = 3.95g/76.13gmol-1 = 0.0519 moles

Number of moles of acetone = 2.43g/58.08gmol-1 = 0.0418 moles

Total number of moles = 0.0937 moles

Mole fraction of CS2 = 0.0519/0.0937 = 0.5538

Mole fraction of acetone = 0.0418/0.0937 = 0.4461

From Raoult’s law;

PCS2 = 0.5538 × 515 torr = 285.207 torr

Pacetone = 0.4461 × 332 torr = 148.1052 torr

Total pressure = 285.207 torr + 148.1052 torr = 433.3 torr

6 0
2 years ago
Enter the net ionic equation, including phases, for the reaction of AgNO3 (aq) and KCl(aq). Refer to the solubility rules as nee
artcher [175]

Answer:

Explanation: you need to remove the subscript of 5

3 0
3 years ago
Read 2 more answers
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
2 years ago
For a particular redox reaction NO is oxidized to NO3– and Ag is reduced to Ag. Complete and balance the equation for this react
mote1985 [20]

It has been given that,

NO + Ag⁺ → NO₃⁻ + Ag

The oxidation half reaction is,

NO + Ag⁺ = NO₃⁻ + Ag

The reduction half reaction is,

Ag⁺ +e⁻ → Ag

The overall balanced reaction is:

3Ag⁺ + NO + 2H₂O → 3Ag + NO₃⁻

6 0
3 years ago
Read 2 more answers
For a certain chemical reaction, the bond energy of the reactants is 43 kJ, and 35 kJ of energy is released. For energy to be co
ASHA 777 [7]

Answer:

78kJ

Explanation:

Energy change = Energy in (reactants) - Energy out (products)

According to this question, energy is released, meaning that the reaction is EXOTHERMIC. Hence, the energy change will be negative (-) i.e bond energy of reactants is greater than bond energy of products.

Energy in = bond energy of reactants = 43kJ

Energy out = bond energy of products = ?

Energy change of exothermic reaction = -35kJ

Therefore;

-35kJ = 43kJ - x

x = 35kJ + 43kJ

x = 78kJ

The bond energy of the products is 78kJ.

8 0
3 years ago
Read 2 more answers
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