Answer:

**Answer:**** The amount of carbon dioxide formed in the reaction is 5.663 grams**

**Explanation:**

**To calculate the number of moles, we use the equation:**

** .....(1)**

Given mass of oxygen gas = 8 g

Molar mass of oxygen gas = 32 g/mol

**Putting values in equation 1, we get:**

**For the given chemical equation:**

**By Stoichiometry of the reaction:**

7 moles of oxygen gas produces 4 moles of carbon dioxide

So, 0.25 moles of oxygen gas will produce = of carbon dioxide

**Now, calculating the mass of carbon dioxide from equation 1, we get:**

Molar mass of carbon dioxide = 44 g/mol

Moles of carbon dioxide = 0.143 moles

**Putting values in equation 1, we get:**

**To calculate the experimental yield of carbon dioxide, we use the equation:**

Percentage yield of carbon dioxide = 90 %

Theoretical yield of carbon dioxide = 6.292 g

**Putting values in above equation, we get:**

**Hence, the amount of carbon dioxide formed in the reaction is 5.663 grams**

Which notations represent atoms that have the same number of protons but a different number of neutrons?

Claims • Evidence • Reasoning Makea claim about ways people can stay safeduring storms with high wind and heavyrains. Summarize evidence to support theclaim and explain your reasoning.

Which species is a conjugate acid of OH-?

The sun warming the surface of a rock isconductionconvectionradiation

What is the mass of oxygen in 250 go of sulfiric acid, H2CO4

Claims • Evidence • Reasoning Makea claim about ways people can stay safeduring storms with high wind and heavyrains. Summarize evidence to support theclaim and explain your reasoning.

Which species is a conjugate acid of OH-?

The sun warming the surface of a rock isconductionconvectionradiation

What is the mass of oxygen in 250 go of sulfiric acid, H2CO4

**Answer:**

The value of Keq is 4e-9. See the solution below

**Explanation:**

We need to balanced rhe equation and use the formula of the Keq

**Answer:**

** 3.7L**

**Explanation:**

Given parameters:

Initial volume = 5.6L

Initial temperature = 25°C = 273 + 25 = 298K

Final temperature = -78°C = 273 + (-78) = 195K

Unknown:

New volume of the balloon = ?

Solution:

We are going to assume that the pressure is constant and then we apply the charles's law;

"the volume of fixed mass of a gas varies directly as its absolute temperature if its pressure is constant"

mathematically;

=

Where V and T are temperature

1 and 2 are initial and final states

Insert the parameters and solve;

=

298V₂ = 1092

V₂ =** 3.7L**

**Answer:**

8.0 mol O₂

**Explanation:**

Let's consider the **complete combustion** reaction of C₉H₁₂.

C₉H₁₂ + 12 O₂ → 9 CO₂ + 6 H₂O

The **molar ratio of C₉H₁₂ to O₂** is 1:12. The moles of O₂ required to react with 0.67 moles of C₉H₁₂ are:

0.67 mol C₉H₁₂ × (12 mol O₂/1 mol C₉H₁₂) = 8.0 mol O₂

8.0 moles of O₂ are required to completely react with 0.67 moles of C₉H₁₂.

**Answer:**

To react with 0.67 moles C9H12 we need 8.04 moles of O2

**Explanation:**

Step 1: Data given

Number of moles C9H12 = 0.67 moles

Step 2: The balanced equation

C9H12 + 12O2 → 9CO2 + 6H2O

Step 3: Calculate moles of O2 required

For 1 mol C9H12 we need 12 moles of O2 to produce 9 moles of CO2 and 6 moles of H2O

For 0.67 moles of C9H12 we need 12 *0.67 = 8.04 moles of O2

To produce 9*0.67 = 6.03 moles of CO2 and 6*0.67 = 4.02 moles H2O

To react with 0.67 moles C9H12 we need 8.04 moles of O2

**Answer:**

balanced............

b. Isotope 48Ti Abundance 10.000% Mass(amu) 47.94795

c. Isotope 50Ti Abundance 19.100% Mass(amu) 49.94479

d. What is the average atomic mass of titanium on that planet?

e. I got 46.9 amu but it is wrong.

**Answer:**

Average atomic mass = 46.91466 amu

**Explanation:**

Step 1: Data given

Isotopes of titanium

46Ti = 70.900% ⇒ 45.95263 amu

48Ti = 10.000 % ⇒ 47.94795 amu

50Ti = 19.100 % ⇒ 49.94479 amu

Step 2: Calculate the average atomic mass of titanium

Average atomic mass = 0.7090 * 45.95263 + 0.10 * 47.94795 + 0.1910 * 49.94479

Average atomic mass = 46.91466 amu

**Answer:**

verdadero/a

falso/b

verdadero/c

**Explanation:**