Answer:
They are able to perform all necessary functions within one cell.
Explanation:
Answer:
1.8 g
Explanation:
Step 1: Write the balanced equation
CH₃CH₃(g) + 3.5 O₂(g) ⇒ 2 CO₂(g) + 3 H₂O(g)
Step 2: Determine the limiting reactant
The theoretical mass ratio of CH₃CH₃ to O₂ is 30.06:112.0 = 0.2684:1.
The experimental mass ratio of CH₃CH₃ to O₂ is 0.60:3.52 = 0.17:1.
Thus, the limiting reactant is CH₃CH₃
Step 3: Calculate the mass of CO₂ produced
The theoretical mass ratio of CH₃CH₃ to O₂ is 30.06:88.02.
0.60 g CH₃CH₃ × 88.02 g CO₂/30.06 g CH₃CH₃ = 1.8 g
Answer:
3.7 atm
General Formulas and Concepts:
<u>Atomic Structure</u>
<u>Gas Laws</u>
Ideal Gas Law: PV = nRT
- <em>P</em> is pressure
- <em>V</em> is volume
- <em>n</em> is number of moles
- <em>R</em> is gas constant
- <em>T</em> is temperature
Explanation:
<u>Step 1: Define</u>
<em>Identify variables</em>
[Given] <em>n</em> = 0.68 mol H
[Given] <em>T</em> = 298 K
[Given] <em>V</em> = 4.5 L
[Given] <em>R</em> = 0.0821 L · atm · mol⁻¹ · K⁻¹
[Solve] <em>P</em>
<em />
<u>Step 2: Find Pressure</u>
- Substitute in variables [Ideal Gas Law]: P(4.5 L) = (0.68 mol)(0.0821 L · atm · mol⁻¹ · K⁻¹)(298 K)
- Multiply [Cancel out units]: P(4.5 L) = (0.055828 L · atm · K⁻¹)(298 K)
- Multiply [Cancel out units]: P(4.5 L) = 16.6367 L · atm
- Isolate <em>P</em> [Cancel out units]: P = 3.69705 atm
<u>Step 3: Check</u>
<em>Follow sig fig rules and round. We are given 2 sig figs as our lowest.</em>
3.69705 atm ≈ 3.7 atm
The rms speed of a gas can be calculated using the following rule:
Vrms = sqrt ( 3RT / M) where:
R is the gas constant = 8.314
T is the temperature = 29 + 273 = 302 degrees kelvin
M is the molar mass of the gas (oxygen) = 2*16 = 32 grams = 0.032 kg
Substitute in the equation to get Vrms as follows:
Vrms = sqrt [(3*8.314*302) / (0.032)] = 485.05 meters/sec